Chem solubility test

Podcast

Play an AI-generated podcast conversation about this lesson

Download our mobile app to listen on the go

Get App

Questions and Answers

What is the term for the substance being dissolved?

Solute

What is the term for the substance doing the dissolving?

Solvent

Describe the characteristic properties of particles in a true solution.

Particles are too small to be seen, cannot be separated by filtration, do not settle out upon standing, and do not scatter light (exhibit the Tyndall effect).

What is the Tyndall effect?

The scattering of a beam of light as it passes through a medium containing particles large enough to scatter it. Signup and view all the answers

What is an aqueous solution?

An aqueous solution is a solution in which water is the solvent. Signup and view all the answers

What is the general term for the process by which a solute dissolves in a solvent?

Solvation Signup and view all the answers

Describe the molecular process of solvation when an ionic compound dissolves in water.

Water molecules, being polar, collide with the ionic crystal lattice. The partially negative oxygen ends of water molecules attract the positive cations, while the partially positive hydrogen ends attract the negative anions. These attractions pull the ions away from the crystal and surround them. Signup and view all the answers

What is the key difference in how ionic compounds and molecular (covalent) compounds behave during solvation in water?

Ionic compounds dissociate into individual ions, whereas most molecular compounds dissolve as intact, neutral molecules. Signup and view all the answers

In calorimetry experiments involving solutions, what does the mass 'm' represent in the equation $q = mc\Delta T$?

The total mass of the solution, which is the sum of the mass of the solute and the mass of the solvent. Signup and view all the answers

What value is commonly used for the specific heat capacity, 'c' ($c_p$), in the equation $q = mc\Delta T$ when dealing with dilute aqueous solutions?

$4.18 , \text{J/g}\cdot^\circ\text{C}$ (or $4.18 , \text{J/g}\cdot\text{K}$) Signup and view all the answers

If the temperature of the solution increases during the solvation process, is the process exothermic or endothermic?

Exothermic Signup and view all the answers

If the temperature of the solution decreases during the solvation process, is the process exothermic or endothermic?

Endothermic Signup and view all the answers

Under what energy conditions is the overall solvation process endothermic?

Solvation is endothermic if the energy required to separate solute particles from each other and solvent molecules from each other is greater than the energy released when solute particles interact with solvent molecules. Signup and view all the answers

Under what energy conditions is the overall solvation process exothermic?

Solvation is exothermic when the energy released during the interaction between solute particles and solvent molecules is greater than the energy required to separate the solute particles and solvent molecules. Signup and view all the answers

Which steps in the dissolving process typically require energy input (are endothermic)?

Separating the solute particles from each other (overcoming solute-solute forces) and separating the solvent molecules from each other (overcoming solvent-solvent forces). Signup and view all the answers

Which step in the dissolving process typically releases energy (is exothermic)?

The formation of attractions between the solvent molecules and the solute particles (solvation). Signup and view all the answers

What is an electrolyte?

A compound that conducts electricity when dissolved in water (aqueous solution) or when in the molten state. Signup and view all the answers

Give general examples of substances that typically behave as electrolytes.

Ionic compounds (salts), acids, and bases. Signup and view all the answers

What types of substances are considered strong electrolytes?

Strong acids, strong bases, and soluble ionic compounds. Signup and view all the answers

What types of substances are considered weak electrolytes?

Weak acids, weak bases, and slightly soluble ionic compounds (salts). Signup and view all the answers

What is a nonelectrolyte?

A compound that does not conduct electricity when dissolved in water or in the molten state. Signup and view all the answers

Give a general example of substances that typically behave as nonelectrolytes.

Most molecular (covalent) compounds that are not acids or bases. Signup and view all the answers

List the formulas of the seven common strong acids.

HCl, HBr, HI, HNO$_3$, H$_2$SO$_4$, HClO$_4$, HClO$_3$ Signup and view all the answers

Identify the common strong, soluble bases.

Hydroxides of the alkali metals (Group 1, e.g., NaOH, KOH) and the heavier alkaline earth metals: Ca(OH)$_2$, Sr(OH)$_2$, Ba(OH)$_2$. Signup and view all the answers

How does the brightness of a light bulb in a conductivity apparatus relate to a strong electrolyte solution?

The light bulb glows brightly. Signup and view all the answers

How does the brightness of a light bulb in a conductivity apparatus relate to a nonelectrolyte solution?

The light bulb does not glow. Signup and view all the answers

How does the brightness of a light bulb in a conductivity apparatus relate to a weak electrolyte solution?

The light bulb glows dimly. Signup and view all the answers

Do nonelectrolytes ionize when dissolved in solution?

No, they do not ionize; they typically dissolve as intact molecules. Signup and view all the answers

To what extent do strong electrolytes ionize in solution?

They ionize extensively, meaning they dissociate or ionize completely or nearly completely. Signup and view all the answers

To what extent do weak electrolytes ionize in solution?

They ionize only partially, establishing an equilibrium between the non-ionized substance and its ions. Signup and view all the answers

How does decreasing the particle size of a solid solute generally affect the rate at which it dissolves?

Decreasing the particle size increases the rate of dissolution because it exposes a larger total surface area to the solvent. Signup and view all the answers

How does increasing the temperature of the solvent generally affect the rate at which a solid solute dissolves?

Increasing the temperature increases the rate of dissolution because the solvent molecules have higher kinetic energy, leading to more frequent and forceful collisions with the solute. Signup and view all the answers

How does agitation (stirring or shaking) affect the rate at which a solute dissolves?

Agitation increases the rate of dissolution by continuously bringing fresh solvent molecules into contact with the solute surface and dispersing dissolved solute away from the surface. Signup and view all the answers

What property of the water molecule makes it such an effective solvent for many ionic and polar compounds?

Water is a highly polar molecule, with partially positive hydrogen atoms and a partially negative oxygen atom. Signup and view all the answers

Explain why polar and ionic compounds tend to be soluble in water.

They are generally soluble because the polar water molecules can effectively surround and stabilize the charged ions (of ionic compounds) or the polar molecules (of polar covalent compounds) through electrostatic attractions. Signup and view all the answers

Explain why nonpolar compounds tend not to be soluble in water.

They are generally insoluble because nonpolar molecules lack significant charge separation and cannot form strong attractions with polar water molecules. The strong hydrogen bonding between water molecules tends to exclude nonpolar solutes. Signup and view all the answers

Are nonpolar substances generally soluble in other nonpolar substances? Why?

Yes, nonpolar substances tend to dissolve well in other nonpolar substances. Signup and view all the answers

How does increasing the pressure above a liquid affect the solubility of a gaseous solute in that liquid?

Increasing the pressure increases the solubility of the gas in the liquid. Signup and view all the answers

How does changing the pressure generally affect the solubility of solid or liquid solutes dissolved in a liquid solvent?

Changing the pressure has very little or no significant effect on the solubility of solid or liquid solutes in liquid solvents. Signup and view all the answers

How does increasing the temperature affect the solubility of most gaseous solutes in liquids?

Increasing the temperature typically decreases the solubility of gases in liquids. Signup and view all the answers

How does increasing the temperature generally affect the solubility of most solid solutes in liquid solvents?

For most solid solutes, solubility increases as the temperature increases. Signup and view all the answers

Explain the meaning of the phrase 'like dissolves like' in the context of solution formation.

This principle states that substances with similar polarities and types of intermolecular forces tend to be soluble in one another. Polar solvents dissolve polar and ionic solutes, while nonpolar solvents dissolve nonpolar solutes. Signup and view all the answers

To maximize the amount of carbon dioxide dissolved in soda water, under what conditions of temperature and pressure should it be bottled?

Low temperature and high pressure. Signup and view all the answers

What is the general relationship between the temperature and the solubility of most solid substances in liquid solvents?

The solubility of most solids in liquids increases as the temperature increases. Signup and view all the answers

Does stirring a mixture of sugar and water change the maximum amount of sugar that can dissolve (solubility) or just how quickly it dissolves (rate)?

Stirring only increases the rate of solution formation (how quickly it dissolves); it does not affect the solubility (the maximum amount that can dissolve at a given temperature). Signup and view all the answers

Write the balanced molecular equation for the reaction between aqueous potassium phosphate and aqueous aluminum nitrate.

K$_3$PO$_4$(aq) + Al(NO$_3$)$_3$(aq) $\rightarrow$ 3KNO$_3$(aq) + AlPO$_4$(s) Signup and view all the answers

Write the complete ionic equation for the reaction K$_3$PO$_4$(aq) + Al(NO$_3$)$_3$(aq) $\rightarrow$ 3KNO$_3$(aq) + AlPO$_4$(s).

3K$^+$(aq) + PO$_4^{3-}$(aq) + Al$^{3+}$(aq) + 3NO$_3^-$(aq) $\rightarrow$ 3K$^+$(aq) + 3NO$_3^-$(aq) + AlPO$_4$(s) Signup and view all the answers

Write the net ionic equation for the reaction K$_3$PO$_4$(aq) + Al(NO$_3$)$_3$(aq) $\rightarrow$ 3KNO$_3$(aq) + AlPO$_4$(s).

Al$^{3+}$(aq) + PO$_4^{3-}$(aq) $\rightarrow$ AlPO$_4$(s) Signup and view all the answers

Identify the spectator ions in the reaction between aqueous potassium phosphate and aqueous aluminum nitrate.

K$^+$ and NO$_3^-$ Signup and view all the answers

What defines a saturated solution?

A saturated solution contains the maximum possible amount of dissolved solute in a given amount of solvent at a specific temperature (and pressure). If more solute is added, it will not dissolve. Signup and view all the answers

What defines an unsaturated solution?

An unsaturated solution contains less than the maximum possible amount of dissolved solute in a given amount of solvent at a specific temperature. More solute can still be dissolved. Signup and view all the answers

What is a supersaturated solution, and how is one typically prepared?

A supersaturated solution contains more dissolved solute than a saturated solution can normally hold at that temperature. It is typically prepared by creating a saturated solution at a higher temperature and then carefully cooling it without disturbing it. Signup and view all the answers

What does the term 'concentration' describe in relation to a solution?

Concentration is a measure of the amount of solute dissolved in a specific amount of solvent or solution. Signup and view all the answers

What is meant qualitatively by a 'concentrated' solution?

A concentrated solution has a relatively large amount of solute dissolved per unit amount of solvent or solution. Signup and view all the answers

What is meant qualitatively by a 'dilute' solution?

A dilute solution has a relatively small amount of solute dissolved per unit amount of solvent or solution. Signup and view all the answers

Define molarity (M) as a unit of concentration.

Molarity (M) is defined as the number of moles of solute per liter of solution. Signup and view all the answers

Briefly outline the steps to prepare 500.0 mL of a 0.10 M NaCl solution (Molar mass of NaCl = 58.44 g/mol).

<ol> <li>Calculate mass needed: $(0.10 , \text{mol/L}) \times (0.5000 , \text{L}) \times (58.44 , \text{g/mol}) = 2.92 , \text{g NaCl}$. 2. Weigh out 2.92 g of NaCl. 3. Add the NaCl to a 500.0 mL volumetric flask. 4. Add some distilled water and swirl to dissolve the NaCl. 5. Carefully add more distilled water until the bottom of the meniscus reaches the calibration mark. 6. Stopper the flask and invert several times to ensure thorough mixing.</li> </ol> Signup and view all the answers

How would you prepare 1.00 L of a 0.495 M urea solution starting with a 3.07 M urea stock solution?

<ol> <li>Use the dilution formula $M_1V_1 = M_2V_2$: $(3.07 , M) V_1 = (0.495 , M) (1.00 , L)$. 2. Solve for $V_1$: $V_1 = \frac{(0.495 , M)(1.00 , L)}{3.07 , M} = 0.161 , L$ or $161 , mL$. 3. Measure 161 mL of the 3.07 M stock solution using a suitable measuring device (e.g., graduated cylinder or pipette). 4. Transfer the measured stock solution to a 1.00 L volumetric flask. 5. Add distilled water until the bottom of the meniscus reaches the calibration mark. 6. Stopper and invert to mix thoroughly.</li> </ol> Signup and view all the answers

To what extent do soluble ionic compounds and strong acids/bases ionize when dissolved in water?

They ionize (or dissociate) completely or nearly completely in aqueous solution. Signup and view all the answers

Generally, do gases, pure liquids, insoluble solids (precipitates), weak acids, weak bases, and most covalent compounds ionize significantly in aqueous solution?

No, these substances generally do not ionize significantly (or at all) in aqueous solution. Weak acids and weak bases ionize partially. Signup and view all the answers

Write the mathematical formula for calculating molarity (M).

$M = \frac{\text{moles of solute}}{\text{Liters of solution}}$ Signup and view all the answers

What is the common formula used for dilution calculations?

$M_1V_1 = M_2V_2$ Signup and view all the answers

Describe how to prepare 1.00 L of a 0.500 M solution of copper(II) sulfate, CuSO$_4$ (Molar mass $\approx$ 159.61 g/mol).

<ol> <li>Calculate mass needed: $(0.500 , \text{mol/L}) \times (1.00 , \text{L}) \times (159.61 , \text{g/mol}) = 79.8 , \text{g CuSO}_4$. 2. Weigh out 79.8 g of anhydrous CuSO$_4$. 3. Add the solid to a 1.00 L volumetric flask containing some distilled water. 4. Swirl the flask to dissolve the solid completely. 5. Carefully add distilled water until the bottom of the meniscus reaches the 1.00 L calibration mark. 6. Stopper and invert the flask repeatedly to ensure a homogeneous solution.</li> </ol> Signup and view all the answers

Is ammonia (NH$_3$) soluble in water, and why?

Yes, ammonia is highly soluble in water because it is a polar molecule that can form hydrogen bonds with water molecules. Signup and view all the answers

On a typical graph plotting solubility versus temperature, what trend do the curves for most gaseous solutes exhibit?

The curves for gaseous solutes typically show a negative slope, indicating that the solubility of gases decreases as temperature increases. Signup and view all the answers

How can you prepare a saturated solution of a solid solute in water at a specific temperature?

Continuously add the solid solute to the water while stirring at the desired temperature. Keep adding solute until no more dissolves and some undissolved solid remains at the bottom. Signup and view all the answers

What is a solute?

The substance being dissolved. Signup and view all the answers

What is a solvent?

The substance doing the dissolving. Signup and view all the answers

List the key properties of true solutions.

Particles are too small to be seen, do not scatter light (no Tyndall effect), cannot be filtered out, and do not settle upon standing. Signup and view all the answers

What is the Tyndall effect?

The scattering of a light beam as it passes through a medium containing dispersed particles. Signup and view all the answers

What is an aqueous solution?

A solution in which water is the solvent. Signup and view all the answers

What is solvation?

The process by which solvent molecules surround and interact with solute particles (ions or molecules) to dissolve them. Signup and view all the answers

Describe the process of solvation for an ionic compound in water.

Polar water molecules collide with the ionic crystal. The negative (oxygen) ends of water molecules attract and surround the positive cations, while the positive (hydrogen) ends attract and surround the negative anions, pulling them away from the crystal lattice. Signup and view all the answers

What is the main difference between the solvation of an ionic compound and a molecular (covalent) compound?

Ionic compounds typically dissociate into ions during solvation, whereas covalent compounds usually remain as intact molecules. Signup and view all the answers

In the calorimetry equation $q=mc\Delta T$ applied to solutions, what does 'm' represent?

The total mass of the solution, which is the mass of the solute plus the mass of the solvent. Signup and view all the answers

In the equation $q=mc\Delta T$ applied to dilute aqueous solutions, what value is commonly used for 'c' (specific heat capacity)?

$4.18 \text{ J/g}^{\circ}\text{C}$ Signup and view all the answers

In solution calorimetry ($q=mc\Delta T$), if the temperature of the solution increases, is the dissolution process exothermic or endothermic?

Exothermic. Heat is released by the dissolving process into the solution, causing the solution's temperature to rise ($"Delta T$ is positive). Signup and view all the answers

In solution calorimetry ($q=mc\Delta T$), if the temperature of the solution decreases, is the dissolution process exothermic or endothermic?

Endothermic. Heat is absorbed by the dissolving process from the solution, causing the solution's temperature to fall ($"Delta T$ is negative). Signup and view all the answers

Under what energy conditions is the solvation process endothermic overall?

The process is endothermic if the energy required to break solute-solute and solvent-solvent interactions is greater than the energy released when solute-solvent interactions form. Signup and view all the answers

Under what energy conditions is the solvation process exothermic overall?

The process is exothermic if the energy required to break solute-solute and solvent-solvent interactions is less than the energy released when solute-solvent interactions form. Signup and view all the answers

Which steps involved in the dissolving process are typically endothermic?

Separating the solute particles from each other and separating the solvent molecules from each other both require energy input, making them endothermic. Signup and view all the answers

Which step involved in the dissolving process is typically exothermic?

The formation of attractions between the solvent particles and the solute particles releases energy, making it exothermic. Signup and view all the answers

What is an electrolyte?

A compound that conducts an electric current when dissolved in water (aqueous solution) or in the molten state. Signup and view all the answers

Give general examples of substances that are electrolytes.

Ionic compounds (salts), acids, and bases. Signup and view all the answers

Give examples of strong electrolytes.

Strong acids (e.g., HCl, H$_2$SO$_4$), strong bases (e.g., NaOH, Ba(OH)$_2$), and soluble ionic compounds (e.g., NaCl, KNO$_3$). Signup and view all the answers

Give examples of weak electrolytes.

Weak acids (e.g., HC$_2$H$_3$O$_2$, HF), weak bases (e.g., NH$_3$), and slightly soluble ionic compounds. Signup and view all the answers

What is a nonelectrolyte?

A compound that does not conduct an electric current in aqueous solutions or in the molten state. Signup and view all the answers

Give examples of nonelectrolytes.

Most molecular (covalent) compounds that are not acids or bases, such as sugar (sucrose, C${12}$H${22}$O$_{11}$), ethanol (C$_2$H$_5$OH), and urea ((NH$_2$)$_2$CO). Signup and view all the answers

List the seven common strong acids.

HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HNO$_3$ (nitric acid), H$_2$SO$_4$ (sulfuric acid), HClO$_4$ (perchloric acid), HClO$_3$ (chloric acid). Signup and view all the answers

Which common bases are considered strong and soluble?

Hydroxides of alkali metals (Group 1, e.g., NaOH, KOH) and the heavier alkaline earth metals (Ca(OH)$_2$, Sr(OH)$_2$, Ba(OH)$_2$). Signup and view all the answers

How does the brightness of a lightbulb in a conductivity tester relate to a strong electrolyte solution?

The light bulb glows brightly. Signup and view all the answers

How does the brightness of a lightbulb in a conductivity tester relate to a nonelectrolyte solution?

The light bulb does not glow. Signup and view all the answers

How does the brightness of a lightbulb in a conductivity tester relate to a weak electrolyte solution?

The light bulb glows dimly. Signup and view all the answers

Describe the extent of ionization for a nonelectrolyte in solution.

It does not ionize in solution. Signup and view all the answers

Describe the extent of ionization for a strong electrolyte in solution.

It ionizes extensively (essentially 100% complete ionization or dissociation). Signup and view all the answers

Describe the extent of ionization for a weak electrolyte in solution.

It partially ionizes in solution. Signup and view all the answers

How does particle size affect the rate at which a solid solute dissolves?

Smaller particles dissolve faster because they have a larger total surface area exposed to the solvent, allowing for more frequent contact between solvent molecules and the solute. Signup and view all the answers

How does temperature generally affect the rate at which a solid solute dissolves?

Increasing the temperature increases the rate of dissolving. Higher temperature gives solvent molecules more kinetic energy, leading to more frequent and more forceful collisions with the solute. Signup and view all the answers

How does agitation (stirring or shaking) affect the rate at which a solid solute dissolves?

Agitation increases the rate of dissolving by bringing fresh solvent molecules into contact with the solute surface and moving dissolved solute away from the surface. Signup and view all the answers

What property of the water molecule makes it such an effective solvent for many ionic and polar substances?

Water is a highly polar molecule, with partially negative oxygen end and partially positive hydrogen ends. This polarity allows it to effectively attract and solvate charged ions and other polar molecules. Signup and view all the answers

Why are many polar and ionic compounds soluble in water?

They are generally soluble because the attractions between the polar water molecules and the charged ions (or polar solute molecules) are strong enough to overcome the forces holding the solute particles together. Signup and view all the answers

Why are most nonpolar compounds not soluble in water?

Nonpolar compounds have an even charge distribution and lack strong attractions to the polar water molecules. Furthermore, the strong hydrogen bonding between water molecules tends to exclude nonpolar molecules. Signup and view all the answers

Are nonpolar substances typically soluble in other nonpolar substances? Explain.

Yes, nonpolar substances are generally soluble in other nonpolar solvents because their intermolecular forces (primarily London dispersion forces) are similar, allowing them to mix easily. Signup and view all the answers

How does changing the pressure affect the solubility of gaseous solutes in liquid solvents?

Increasing the pressure above the liquid increases the solubility of a gas in the liquid. There is a direct relationship. Signup and view all the answers

How does changing the pressure affect the solubility of solid or liquid solutes dissolved in a liquid solvent?

Changing the pressure has almost no effect on the solubility of solid or liquid solutes in liquid solvents. Signup and view all the answers

How does changing the temperature affect the solubility of gaseous solutes in liquid solvents?

Increasing the temperature generally decreases the solubility of gases in liquids. Lower temperatures favor higher gas solubility. Signup and view all the answers

How does changing the temperature generally affect the solubility of solid or liquid solutes dissolved in a liquid solvent?

For most solid solutes, increasing the temperature increases their solubility in liquid solvents. Signup and view all the answers

Explain the general principle of 'like dissolves like'.

This principle states that substances with similar types of intermolecular forces and polarity tend to be soluble in each other. Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes. Signup and view all the answers

Under what conditions of temperature and pressure should carbonated beverages (soda) be bottled to maximize the dissolved CO$_2$?

Soda should be bottled under conditions of low temperature and high pressure. Signup and view all the answers

What is the general relationship between the solubility of solid substances in liquids and temperature?

The solubility of most solids in liquids increases as the temperature increases. Signup and view all the answers

What is the effect of stirring when dissolving a solid like sugar in water?

Stirring increases the rate at which the sugar dissolves but does not increase the solubility (the maximum amount that can dissolve) at a given temperature. Signup and view all the answers

Write the balanced molecular equation for the precipitation reaction between aqueous potassium phosphate (K$_3$PO$_4$) and aqueous aluminum nitrate (Al(NO$_3$)$_3$).

K$_3$PO$_4$(aq) + Al(NO$_3$)$_3$(aq) $\rightarrow$ 3KNO$_3$(aq) + AlPO$_4$(s) Signup and view all the answers

Write the complete ionic equation for the reaction: K$_3$PO$_4$(aq) + Al(NO$_3$)$_3$(aq) $\rightarrow$ 3KNO$_3$(aq) + AlPO$_4$(s).

3K$^+$(aq) + PO$_4^{3-}$(aq) + Al$^{3+}$(aq) + 3NO$_3^-$(aq) $\rightarrow$ 3K$^+$(aq) + 3NO$_3^-$(aq) + AlPO$_4$(s) Signup and view all the answers

Write the net ionic equation for the reaction between aqueous potassium phosphate and aqueous aluminum nitrate.

Al$^{3+}$(aq) + PO$_4^{3-}$(aq) $\rightarrow$ AlPO$_4$(s) Signup and view all the answers

Identify the spectator ions in the reaction between aqueous potassium phosphate and aqueous aluminum nitrate.

The spectator ions are K$^+$ (potassium ion) and NO$_3^-$ (nitrate ion). Signup and view all the answers

What is a saturated solution?

A solution that contains the maximum amount of solute that can be dissolved in a specific amount of solvent at a given temperature. In a saturated solution with excess solid present, a dynamic equilibrium exists between dissolving and crystallization. Signup and view all the answers

What is an unsaturated solution?

A solution that contains less than the maximum amount of solute that can be dissolved in a specific amount of solvent at a given temperature. Signup and view all the answers

What is a supersaturated solution?

A solution that contains more dissolved solute than is normally possible at a given temperature; it holds more solute than a saturated solution. These solutions are unstable. Signup and view all the answers

Define concentration in the context of solutions.

Concentration is a measure of the amount of solute dissolved in a given amount of solvent or solution. Signup and view all the answers

What is meant by a concentrated solution?

A solution that has a relatively large amount of solute dissolved per unit amount of solvent or solution. Signup and view all the answers

What is meant by a dilute solution?

A solution that has a relatively small amount of solute dissolved per unit amount of solvent or solution. Signup and view all the answers

Define Molarity (M).

Molarity is a unit of concentration defined as the number of moles of solute per liter of solution. Signup and view all the answers

Outline the procedure for preparing 500.0 mL of a 0.100 M NaCl solution using solid NaCl.

<ol> <li>Calculate the mass of NaCl needed: (0.100 mol/L) * (0.5000 L) * (58.44 g/mol) = 2.92 g NaCl.</li> <li>Accurately weigh out 2.92 g of NaCl.</li> <li>Transfer the NaCl to a 500.0 mL volumetric flask.</li> <li>Add some distilled water to dissolve the NaCl, swirling gently.</li> <li>Carefully add distilled water until the bottom of the meniscus reaches the calibration mark on the flask neck.</li> <li>Stopper the flask and invert multiple times to ensure thorough mixing.</li> </ol> Signup and view all the answers

Outline the procedure for preparing 1.00 L of a 0.495 M solution of urea by diluting a 3.07 M stock solution.

<ol> <li>Use the dilution formula $M_1V_1 = M_2V_2$ to find the required volume of stock solution ($V_1$): $V_1 = (M_2V_2) / M_1 = (0.495 \text{ M} \times 1.00 \text{ L}) / 3.07 \text{ M} = 0.161 \text{ L}$ or 161 mL.</li> <li>Measure 161 mL of the 3.07 M urea stock solution using a graduated cylinder or pipette.</li> <li>Transfer this volume to a 1.00 L volumetric flask.</li> <li>Carefully add distilled water to the flask until the bottom of the meniscus reaches the calibration mark.</li> <li>Stopper the flask and invert multiple times to ensure thorough mixing.</li> </ol> Signup and view all the answers

To what extent do soluble ionic compounds, strong acids, and strong bases ionize in aqueous solution?

They ionize (or dissociate) essentially completely in aqueous solution. Signup and view all the answers

How do substances like gases, pure liquids, insoluble solids (precipitates), weak acids, weak bases, and most covalent compounds typically behave regarding ionization in aqueous solution?

They generally do not ionize, or in the case of weak acids and weak bases, they ionize only partially. Signup and view all the answers

What is the formula for calculating Molarity (M)?

Molarity (M) = $\frac{\text{moles of solute}}{\text{Liters of solution}}$ Signup and view all the answers

What is the formula commonly used for dilution calculations?

$M_1V_1 = M_2V_2$ Signup and view all the answers

Outline the steps to prepare 1.00 L of a 0.500 M solution of copper(II) sulfate (CuSO$_4$) starting from solid CuSO$_4$.

<ol> <li>Calculate the mass of CuSO$_4$ needed. The molar mass of anhydrous CuSO$_4$ is approx. 159.61 g/mol. Mass = (0.500 mol/L) * (1.00 L) * (159.61 g/mol) $\approx$ 79.8 g.</li> <li>Weigh out 79.8 g of solid CuSO$_4$.</li> <li>Transfer the solid to a 1.00 L volumetric flask.</li> <li>Add some distilled water (perhaps half full) and swirl to dissolve the solid completely.</li> <li>Carefully add more distilled water until the bottom of the meniscus reaches the 1.00 L calibration mark.</li> <li>Stopper the flask and invert repeatedly to ensure homogeneity.</li> </ol> Signup and view all the answers

True or False: Ammonia (NH$_3$) is insoluble in water.

False (B) Signup and view all the answers

On a graph plotting solubility versus temperature, what characteristic typically distinguishes the solubility curves of gases from those of most solids?

The solubility curves for gases typically show a decrease in solubility as temperature increases (negative slope), while the solubility curves for most solids show an increase in solubility as temperature increases (positive slope). Signup and view all the answers

How can you prepare a saturated solution of a solid solute in a laboratory setting?

Gradually add the solid solute to a fixed amount of solvent at a constant temperature, stirring continuously. Keep adding solute until no more dissolves and a small amount of undissolved solid remains at the bottom. The liquid above the solid is the saturated solution. Signup and view all the answers

What is a solute?

The substance being dissolved. Signup and view all the answers

What is a solvent?

The substance doing the dissolving. Signup and view all the answers

What are the characteristic properties of solutions?

Particles are too small to be seen, too small to be filtered, particles don't settle when the solution is allowed to stand, and particles don't exhibit the Tyndall effect. Signup and view all the answers

What is the Tyndall effect?

Scattering of a light beam as it hits larger particles. Signup and view all the answers

What is an aqueous solution?

A solution where water is the solvent. Signup and view all the answers

What is solvation?

The process by which a solute dissolves in a solvent. Signup and view all the answers

Describe the process of solvation for an ionic compound in water.

The water molecules separate from each other and collide with the surface of the solid solute. The water molecule is polar. The oxygen end of the water molecule attracts the cations, separates them from the anions, and surrounds them. The hydrogen end of the water molecule attracts the anions, separates them from the cations, and surrounds them. Signup and view all the answers

What is the main difference between the solvation of an ionic compound and a molecular compound?

Ionic compounds dissociate into ions during solvation. Covalent (molecular) compounds generally do not dissociate and remain as intact molecules. Signup and view all the answers

In the equation $q=mc\Delta T$ applied to solutions, what does 'm' represent?

The total mass of the solution (mass of solute + mass of solvent). Signup and view all the answers

In the equation $q=mc\Delta T$ applied to aqueous solutions, what value is typically used for 'c' (specific heat capacity)?

4.18 J/gC Signup and view all the answers

If the temperature of the solution increases during the solvation process, is the process exothermic or endothermic?

Exothermic Signup and view all the answers

If the temperature of the solution decreases during the solvation process, is the process exothermic or endothermic?

Endothermic Signup and view all the answers

Under what energy conditions is the solvation process endothermic?

If the amount of energy required to separate the solvent molecules and solute particles from each other is more than the energy released when the solvent molecules surround the solute particles. Signup and view all the answers

Under what energy conditions is the solvation process exothermic?

When the amount of energy required to separate the solvent and solute molecules from each other is less than the energy released when the solvent molecules surround the solute particles. Signup and view all the answers

Which steps in the dissolving process are endothermic?

Breaking the intermolecular forces (IMFs) or ionic bonds between solute particles and breaking the IMFs between solvent particles. Signup and view all the answers

Which step in the dissolving process is exothermic?

Forming the attractions as the solvent surrounds the solute particles (solvation/hydration). Signup and view all the answers

What is an electrolyte?

A compound that conducts an electric current in aqueous solution or in the molten state. Signup and view all the answers

Provide examples of substances that are electrolytes.

Ionic compounds (salts), acids, and bases. Signup and view all the answers

Give examples of strong electrolytes.

Strong acids (e.g., HCl, H2SO4), strong bases (e.g., NaOH, Ba(OH)2), and soluble ionic compounds (e.g., NaCl, KNO3). Signup and view all the answers

Give examples of weak electrolytes.

Weak acids (e.g., HC2H3O2), weak bases (e.g., NH3), and slightly soluble salts (e.g., AgCl, though its dissolved portion is fully ionized). Signup and view all the answers

What is a nonelectrolyte?

A compound that does not conduct an electric current in aqueous solutions or in the molten state. Signup and view all the answers

Provide examples of substances that are nonelectrolytes.

Most covalent compounds (that are not acids or bases), such as sugars (sucrose, glucose) and alcohols (ethanol, methanol). Signup and view all the answers

Which list contains the seven common strong acids?

HCl, HBr, HI, H2SO4, HNO3, HClO4, HClO3 (B) Signup and view all the answers

List the common strong, soluble bases.

Hydroxides of alkali metals (Group 1: LiOH, NaOH, KOH, RbOH, CsOH) and heavier alkaline earth metals (Group 2: Ca(OH)2, Sr(OH)2, Ba(OH)2). Signup and view all the answers

How brightly would a lightbulb glow in a conductivity apparatus containing a strong electrolyte solution?

The light bulb glows brightly. Signup and view all the answers

How brightly would a lightbulb glow in a conductivity apparatus containing a nonelectrolyte solution?

The light bulb does not glow. Signup and view all the answers

How brightly would a lightbulb glow in a conductivity apparatus containing a weak electrolyte solution?

The light bulb glows dimly. Signup and view all the answers

To what extent does a nonelectrolyte ionize in solution?

It does not ionize in solution. Signup and view all the answers

To what extent does a strong electrolyte ionize in solution?

Ionizes extensively (essentially 100%). Signup and view all the answers

To what extent does a weak electrolyte ionize in solution?

Partially ionizes in solution. Signup and view all the answers

How does decreasing the particle size of a solid solute affect the rate of solution formation?

Decreasing particle size increases the rate of solution formation because it exposes a greater surface area of the solute to the solvent molecules. Signup and view all the answers

How does increasing the temperature of the solvent affect the rate of solution formation for most solid solutes?

Increasing temperature increases the rate of solution formation because solvent molecules have more kinetic energy, move faster, and collide more frequently and forcefully with the solute. Signup and view all the answers

How does agitation (stirring or shaking) affect the rate of solution formation?

Agitation increases the rate of solution formation by allowing fresh solvent molecules to continually come into contact with the solute surface and dispersing dissolved solute away from the surface. Signup and view all the answers

What property of water makes it such an effective solvent for many substances?

Water is a highly polar molecule. Signup and view all the answers

Why are many polar and ionic compounds soluble in water?

Because the polar water molecules can form strong attractions (ion-dipole or dipole-dipole/hydrogen bonds) with the charged ions or polar solute molecules, overcoming the solute-solute and solvent-solvent attractions. Signup and view all the answers

Why are most nonpolar compounds not significantly soluble in water?

Because nonpolar molecules have an even charge distribution and cannot form strong attractions with the polar water molecules. The strong hydrogen bonding between water molecules excludes the nonpolar molecules. Signup and view all the answers

Are nonpolar substances generally soluble in other nonpolar substances? Why?

Yes, nonpolar substances are generally soluble in other nonpolar substances due to the "like dissolves like" principle. Signup and view all the answers

How does a change in pressure affect the solubility of gas solutes dissolved in liquids?

An increase in the partial pressure of the gas above the liquid increases the solubility of the gas in the liquid. It is a direct relationship. Signup and view all the answers

How does a change in pressure affect the solubility of solid or liquid solutes dissolved in a liquid solvent?

Changes in pressure have virtually no effect on the solubility of solid and liquid solutes in liquid solvents. Signup and view all the answers

How does a change in temperature affect the solubility of gas solutes dissolved in liquids?

The solubility of gases in liquids generally decreases as temperature increases. Signup and view all the answers

How does a change in temperature generally affect the solubility of solid solutes dissolved in liquid solvents?

The solubility of most solid solutes in liquid solvents increases as temperature increases. Signup and view all the answers

Explain the principle "like dissolves like".

This principle summarizes the observation that substances with similar types and strengths of intermolecular forces tend to be soluble in each other. Polar solvents dissolve polar and ionic solutes, while nonpolar solvents dissolve nonpolar solutes. Signup and view all the answers

Under what conditions of temperature and pressure should soda (carbonated beverages) be bottled to maximize the solubility of carbon dioxide gas?

Soda should be bottled under conditions of low temperature and high pressure. Signup and view all the answers

What is the general relationship between the solubility of solids in liquids and temperature?

Most solids become more soluble in liquids as the temperature increases. Signup and view all the answers

What is the effect of stirring while dissolving a solid like sugar in water? Does it increase solubility?

Stirring only increases the rate (speed) at which the sugar dissolves. It does not increase the solubility (the maximum amount that can dissolve). Signup and view all the answers

Identify the type of chemical equation shown: `K3PO4(aq) + Al(NO3)3(aq) 3KNO3(aq) + AlPO4(s)`

Molecular equation Signup and view all the answers

Identify the type of chemical equation shown: `3K+(aq) + PO4^3-(aq) + Al^3+(aq) + 3NO3^-(aq) 3K+(aq) + 3NO3^-(aq) + AlPO4(s)`

Complete ionic equation Signup and view all the answers

Identify the type of chemical equation shown: `PO4^3-(aq) + Al^3+(aq) AlPO4(s)`

Net ionic equation Signup and view all the answers

In the reaction between aqueous potassium phosphate and aqueous aluminum nitrate, which ions are the spectator ions? The molecular equation is `K3PO4(aq) + Al(NO3)3(aq) 3KNO3(aq) + AlPO4(s)`.

Potassium ions (K+) and nitrate ions (NO3-). Signup and view all the answers

What is a saturated solution?

A solution that contains the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature and pressure. In a saturated solution, the dissolved solute is in dynamic equilibrium with any undissolved solute. Signup and view all the answers

What is an unsaturated solution?

A solution that contains less than the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature and pressure. Signup and view all the answers

What is a supersaturated solution, and how is it typically prepared?

A solution that contains more dissolved solute than is normally possible in a saturated solution at a given temperature and pressure. It is typically prepared by creating a saturated solution at a high temperature and then slowly cooling it without disturbance. Signup and view all the answers

What does the term 'concentration' refer to in the context of solutions?

The amount of solute present in a given quantity of solvent or solution. Signup and view all the answers

Describe a concentrated solution.

A solution containing a relatively large amount of solute dissolved in a given amount of solvent or solution. Signup and view all the answers

Describe a dilute solution.

A solution containing a relatively small amount of solute dissolved in a given amount of solvent or solution. Signup and view all the answers

Define Molarity (M).

Moles of solute per liter of solution. Signup and view all the answers

Briefly outline the procedure for preparing 500.0 mL of a 0.100 M NaCl solution (Molar mass NaCl = 58.44 g/mol).

<ol> <li>Calculate mass of NaCl needed: (0.100 mol/L) * (0.5000 L) * (58.44 g/mol) = 2.92 g NaCl.</li> <li>Weigh out 2.92 g of NaCl using an electronic balance.</li> <li>Add the NaCl to a 500.0 mL volumetric flask.</li> <li>Add distilled water to dissolve the NaCl, swirling gently.</li> <li>Carefully add more distilled water until the bottom of the meniscus reaches the calibration mark on the flask's neck.</li> <li>Stopper the flask and invert it several times to ensure the solution is homogeneous.</li> </ol> Signup and view all the answers

Describe the procedure for preparing 1.00 L of a 0.495 M solution of urea starting with a 3.07 M stock solution.

<ol> <li>Use the dilution equation $M_1V_1 = M_2V_2$: (3.07 M)(V1) = (0.495 M)(1.00 L).</li> <li>Solve for the volume of stock solution needed: $V1 = (0.495 M * 1.00 L) / 3.07 M = 0.161 L$ or 161 mL.</li> <li>Measure 161 mL of the 3.07 M urea stock solution using a graduated cylinder or pipette.</li> <li>Transfer the measured stock solution into a 1.00 L volumetric flask.</li> <li>Carefully add distilled water to the volumetric flask until the bottom of the meniscus reaches the 1.00 L calibration mark.</li> <li>Stopper the flask and invert it several times to mix thoroughly.</li> </ol> Signup and view all the answers

How completely do soluble ionic compounds and strong acids/bases ionize or dissociate in aqueous solution?

They ionize or dissociate completely (or nearly completely) in aqueous solution. Signup and view all the answers

Do gases (like O2, N2), pure liquids (like H2O), solids/precipitates (like AgCl), weak acids (like HC2H3O2), weak bases (like NH3), and most covalent compounds ionize significantly in aqueous solution?

No, these substances generally do not ionize significantly in aqueous solution. Weak acids and weak bases ionize partially, establishing an equilibrium. Signup and view all the answers

What is the formula for Molarity (M)?

$M = \frac{\text{moles of solute}}{\text{Liters of solution}}$ Signup and view all the answers

What is the formula used for dilution calculations?

$M_1V_1 = M_2V_2$ Signup and view all the answers

How would you prepare 1.00 L of a 0.500 M solution of copper(II) sulfate (CuSO4)? (Molar mass of anhydrous CuSO4 159.61 g/mol)

<ol> <li>Calculate the mass of CuSO4 needed: (0.500 mol/L) * (1.00 L) * (159.61 g/mol) = 79.8 g CuSO4.</li> <li>Weigh out 79.8 g of anhydrous CuSO4.</li> <li>Add the CuSO4 to a 1.00 L volumetric flask.</li> <li>Add about half the required distilled water and swirl until the solid is completely dissolved.</li> <li>Carefully add more distilled water until the bottom of the meniscus reaches the 1.00 L calibration mark.</li> <li>Stopper and invert several times to ensure a homogeneous solution.</li> </ol> Signup and view all the answers

Ammonia (NH3) is insoluble in water because it is a gas at room temperature.

False (B) Signup and view all the answers

On a typical solubility graph plotting solubility versus temperature, what trend distinguishes the curves for gaseous solutes from those of most solid solutes?

Gaseous solutes typically show decreasing solubility as temperature increases (negative slope), whereas most solid solutes show increasing solubility as temperature increases (positive slope). Signup and view all the answers

Describe a practical method to prepare a saturated solution of a solid solute in water at a specific temperature.

Maintain the water at the desired temperature. Add the solid solute gradually while stirring continuously. Continue adding solute until some solid remains undissolved at the bottom, even after thorough mixing. This indicates the solution is saturated. The clear solution above the excess solid is the saturated solution. Signup and view all the answers

Flashcards

Solute

The substance being dissolved in a solution.

Solvent

The substance that dissolves the solute.