Chemistry: Solutions and Solubility
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Questions and Answers

Which component of a solution is present in the greatest amount?

  • Mixture
  • Colloidal substance
  • Solute
  • Solvent (correct)

What defines solubility in a solution?

  • The maximum amount of solute that can dissolve in a given amount of solvent (correct)
  • The process of a solute returning to its original state
  • The ability of the solute to affect the solvent's properties
  • The temperature at which a solution becomes saturated

Which statement about solutions is true?

  • Solutions are always composed of liquid solvents.
  • The solvent is always a gas.
  • A solution is a homogeneous mixture of substances. (correct)
  • Solutes alter their chemical identity when dissolved.

Which factor is likely to influence solubility?

<p>The size of the solute particles (A)</p> Signup and view all the answers

Which of the following correctly identifies a solute?

<p>A component present in a lesser amount (C)</p> Signup and view all the answers

What happens to a solute when it dissolves in a solvent?

<p>It retains its chemical identity while becoming part of the solution. (B)</p> Signup and view all the answers

The term 'homogeneous mixture' most closely describes which characteristic?

<p>All components are uniform and indistinguishable. (A)</p> Signup and view all the answers

Which scenario would likely decrease the solubility of a solute in a solvent?

<p>Decreasing the surface area of the solute (C)</p> Signup and view all the answers

How does temperature generally affect the solubility of solids in water?

<p>Increases solubility with increasing temperature (D)</p> Signup and view all the answers

What is the effect of pressure on the solubility of solids and liquids in water?

<p>Pressure has little effect on solubility (C)</p> Signup and view all the answers

How does temperature affect the solubility of gases in water?

<p>Decreases solubility with increasing temperature (C)</p> Signup and view all the answers

According to Henry's Law, what happens to the amount of gas dissolved in a liquid if the partial pressure of that gas is increased?

<p>It increases (C)</p> Signup and view all the answers

What is primarily true about the solubility of gases compared to that of solids?

<p>Gas solubility is significantly affected by temperature and pressure (D)</p> Signup and view all the answers

Which of the following best describes the relationship between partial pressure and gas solubility as indicated by Henry's Law?

<p>Direct relationship (B)</p> Signup and view all the answers

What effect does increasing temperature have on the solubility of most solids in water?

<p>It enhances solubility (B)</p> Signup and view all the answers

Which statement regarding solubility changes with pressure is correct?

<p>Pressure significantly affects the solubility of gases (A)</p> Signup and view all the answers

What is defined as a solution in which water is the solvent?

<p>Aqueous solution (B)</p> Signup and view all the answers

Which interparticle attraction must be overcome for a solute to dissolve in a solvent?

<p>Attractions between solute–solute particles (B)</p> Signup and view all the answers

What generally happens when there is a greater difference in solute–solvent polarity?

<p>The solute is less likely to dissolve (C)</p> Signup and view all the answers

What does the phrase 'like dissolves like' imply about solubility?

<p>Similar polarities enhance solubility (B)</p> Signup and view all the answers

Which of the following is NOT a method for expressing concentration?

<p>Mass concentration (D)</p> Signup and view all the answers

What type of attraction arises from solute and solvent interacting?

<p>Solute–solvent attraction (A)</p> Signup and view all the answers

In which situation would you expect a solute to be less soluble?

<p>When the solute and solvent are of different polarities (B)</p> Signup and view all the answers

What concept does the term 'percent concentration' refer to?

<p>The amount of solute in a specified amount of solution (C)</p> Signup and view all the answers

What defines an unsaturated solution?

<p>It contains less than the maximum amount of solute that can be dissolved. (D)</p> Signup and view all the answers

Which statement accurately describes a saturated solution?

<p>It contains the maximum amount of solute that can be dissolved. (A)</p> Signup and view all the answers

What is a characteristic of a supersaturated solution?

<p>It temporarily contains more dissolved solute than that present in a saturated solution. (A)</p> Signup and view all the answers

How is a concentrated solution defined?

<p>It contains a large amount of solute relative to the amount that could dissolve. (C)</p> Signup and view all the answers

What is the primary difference between a concentrated solution and a dilute solution?

<p>A concentrated solution has a larger amount of solute relative to what could dissolve. (B)</p> Signup and view all the answers

What occurs over time in a supersaturated solution?

<p>Excess solute will crystallize out, leading to saturation. (A)</p> Signup and view all the answers

Which of the following solutions is considered most commonly encountered?

<p>Unsaturated solutions are the most common type of solution. (D)</p> Signup and view all the answers

In which scenario would you typically find a concentrated solution?

<p>In scenarios where a large amount of solute is present relative to the solvent. (D)</p> Signup and view all the answers

How many grams of sodium chloride are required to create 150 mL of a 0.9% (m/v) solution?

<p>1.35 g (D)</p> Signup and view all the answers

What is the molarity of a solution containing 1.00 mol of sugar in 125.0 mL?

<p>8.0 M (A)</p> Signup and view all the answers

If you have a 10.0 M sugar solution, what volume do you need to obtain 2.00 mol of sugar?

<p>0.2 L (A)</p> Signup and view all the answers

What is the formula for calculating molarity?

<p>moles of solute / liters of solution (D)</p> Signup and view all the answers

How would you express a 0.9% (m/v) solution in terms of grams per 100 mL?

<p>0.9 g (A)</p> Signup and view all the answers

Which of the following statements is true regarding a 10.0 M solution?

<p>It contains 10 moles of solute in 1000 mL. (C)</p> Signup and view all the answers

What is the effect of increasing the volume of solvent on the molarity of a solution?

<p>Molarity decreases. (A)</p> Signup and view all the answers

What would be the molarity of 0.5 mol of sodium chloride dissolved in 250 mL?

<p>1.0 M (D)</p> Signup and view all the answers

What is the definition of dilution?

<p>The process of adding more solvent to a solution to lower its concentration. (C)</p> Signup and view all the answers

To prepare a 100 mL of 0.9% saline solution from a 10% saline solution, which combination is correct?

<p>9 mL of 10% saline solution + 91 mL of water (B)</p> Signup and view all the answers

Which action would decrease the concentration of a 0.50 M sodium chloride solution?

<p>Add water to the solution. (A), Pour some of the solution down the sink drain. (C)</p> Signup and view all the answers

Using the dilution formula, Cs × Vs = Cd × Vd, what do 'Cs' and 'Vs' represent?

<p>Concentration and volume of the stock solution. (B)</p> Signup and view all the answers

How can you calculate the minimum volume of a 2.00 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?

<p>Using the formula Cs × Vs = Cd × Vd. (C)</p> Signup and view all the answers

When diluting solutions, which factor must remain consistent to ensure accuracy?

<p>The initial concentration of the solute. (A)</p> Signup and view all the answers

In what scenario would the concentration of a salt solution increase?

<p>Adding more sodium chloride to the solution. (A)</p> Signup and view all the answers

If 60.0 mL of a 2.00 M NaOH solution is used to make a 0.800 M solution, what will be the total volume of the resulting solution?

<p>150.0 mL (A)</p> Signup and view all the answers

Flashcards

What is a Solution?

A homogeneous mixture of two or more substances where each substance keeps its original chemical properties.

Solvent

The component of a solution present in the largest amount.

Solute

The component of a solution present in a smaller amount compared to the solvent.

What is Solubility?

The maximum amount of a solute that can dissolve in a specific amount of solvent at a given temperature and pressure.

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What factors affect Solubility?

Factors that affect solubility include temperature, pressure, and the nature of the solute and solvent.

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Solution formation

The process of dissolving a solute in a solvent to create a homogeneous mixture.

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Solubility of Solids in Water

The amount of solid that can dissolve in a certain amount of water. Most solids become more soluble as the temperature increases.

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Solubility of Gases in Water

The amount of gas that can dissolve in a certain amount of water. Gases become less soluble as the temperature increases.

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Pressure's Effect on Solid/Liquid Solubility

Pressure has little effect on the solubility of solids or liquids in water.

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Pressure's Effect on Gas Solubility

Pressure significantly impacts the solubility of gases in water. As pressure increases, more gas dissolves in water.

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Henry's Law

This law describes the relationship between gas pressure and solubility. Higher pressure leads to higher solubility of a gas in a liquid.

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What Happens to the Solubility of a Gas as Temperature Increases?

The solubility of a gas in a liquid decreases as the temperature increases.

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What Happens to the Solubility of a Solid as Temperature Increases?

The solubility of a solid in a liquid typically increases as the temperature increases.

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What Happens to the Solubility of a Solid or Liquid as Pressure Increases?

Pressure has very little effect on the solubility of solids or liquids in water.

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Aqueous solution

A solution where water is the solvent.

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Nonaqueous solution

A solution where a substance other than water is the solvent.

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Solute-Solvent Interactions

When a solute dissolves, it breaks apart from other solute particles and forms new attractions with solvent particles.

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Like Dissolves Like

Substances with similar polarity (how strongly they attract electrons) tend to dissolve in each other.

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Concentration

The amount of solute present in a specific amount of solution.

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Percent Concentration

A way to express concentration as a percentage of solute in the solution.

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Molarity

A concentration unit that expresses the number of moles of solute per liter of solution.

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Molality

A concentration unit that expresses the number of moles of solute per kilogram of solvent.

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Unsaturated Solution

A solution that contains less solute than it can hold at a given temperature and pressure.

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Saturated Solution

A solution that contains the maximum amount of solute that can dissolve at a given temperature and pressure. Any more solute added will not dissolve.

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Supersaturated Solution

A solution that holds more solute than a saturated solution at a given temperature and pressure, but is unstable.

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What happens to a supersaturated solution?

Over time, excess solute will crystallize out, returning the solution to a saturated state.

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Concentrated Solution

A solution with a large amount of solute relative to the amount that could dissolve.

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Dilute Solution

A solution with a small amount of solute relative to the amount that could dissolve.

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What's the difference between a saturated and concentrated solution?

A saturated solution contains the maximum amount of solute that can dissolve, while a concentrated solution simply has a large amount of solute, which may not be the maximum possible.

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What's the relationship between solubility and concentration?

Solubility determines the maximum concentration a solution can reach, while concentration describes the amount of solute present, which may be less than the solubility limit.

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Percent Concentration (m/v)

The mass of solute (in grams) per 100 mL of solution. It expresses the amount of solute in a given volume of solution.

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Molarity (M)

The concentration of a solution expressed as moles of solute per liter of solution. It reflects the number of moles of solute dissolved in a specific volume of solution.

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How to Calculate Percent Concentration (m/v)

Divide the mass of solute (in grams) by the volume of solution (in mL) and multiply by 100%.

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How to Calculate Molarity

Divide the moles of solute by the volume of solution (in liters).

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Percent Concentration Example

To make 150 mL of 0.9% (m/v) sodium chloride solution, you need 1.35 grams of sodium chloride.

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Molarity Example

If you have 1 mole of sugar in 125 mL of solution, the molarity is 8 M.

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What volume do you need for a given number of moles?

Divide the desired number of moles by the molarity of the solution.

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Molarity and Dilution

Changing the volume of a solution will affect the concentration, but the total number of moles of solute remains the same.

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Dilution

The process of decreasing the concentration of a solution by adding more solvent.

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Dilution Formula

The formula used to calculate the relationship between the concentration and volume of a stock solution and its diluted form: Cs × Vs = Cd × Vd, where Cs is the concentration of the stock solution, Vs is the volume of the stock solution, Cd is the concentration of the diluted solution, and Vd is the volume of the diluted solution.

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How to prepare a diluted solution

To prepare a diluted solution, you need to determine the volume of the concentrated solution (stock solution) and the volume of solvent to add.

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What decreases the concentration of a solution?

Adding more solvent to the solution decreases the concentration.

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Calculating volume needed for dilution

To calculate the minimum volume of a concentrated solution needed to make a specific volume of a diluted solution, use the dilution formula (Cs × Vs = Cd × Vd) and solve for Vs.

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Common Dilution Scenarios

Examples of dilution include preparing a 0.9% saline solution from a 10% saline solution or making a weaker NaOH solution from a concentrated one.

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Dilution: Concentration change

Dilution results in a decrease in the concentration of a solution because the amount of solute remains constant while the volume of the solution increases.

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Dilution: Importance

Dilution is a fundamental technique commonly used in laboratories and industries to prepare solutions of desired concentrations for various purposes and experiments.

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Study Notes

  • Solutions are homogeneous mixtures of two or more substances, where each substance retains its own chemical identity.
  • A solution comprises a solvent (the component present in the greatest amount) and a solute (the component present in a lesser amount).
  • Solubility is the maximum amount of solute that can dissolve in a given amount of solvent under specific conditions.
  • Solubility of solids generally increases with temperature, while gas solubility decreases with temperature.
  • Pressure has little effect on the solubility of solids and liquids in water, but significantly impacts the solubility of gases (Henry's Law). The solubility of a gas is directly proportional to the partial pressure of the gas above the liquid.
  • Solutions can be unsaturated (more solute can dissolve), saturated (no more solute can dissolve), or supersaturated (more solute is dissolved than should be possible at the given conditions).
  • Concentrated solutions contain a large amount of solute relative to the amount that could dissolve, while dilute solutions contain a small amount of solute relative to the maximum possible amount in a given amount of solvent.
  • Aqueous solutions have water as the solvent, while non-aqueous solutions have a solvent other than water.
  • For a solute to dissolve in a solvent, two types of interparticle attractions must be broken: solute-solute and solvent-solvent attractions. A new type of attraction, solute-solvent, forms.
  • "Like dissolves like" is a general rule—substances with similar polarities tend to be more soluble in each other.
  • Concentration can be expressed using different units: percent concentration (by mass, by volume, or mass-volume), molarity, and molality.
  • Molarity is the moles of solute per liter of solution, while molality is the moles of solute per kilogram of solvent.
  • Dilutions involve adding more solvent to a solution to decrease its concentration.
  • Osmolarity is a measure of osmotic pressure based on the number of solute particles in a solution.
  • Osmosis is the movement of solvent (like water) across a semi-permeable membrane from a region of higher solvent concentration to a region of lower solvent concentration.
  • Osmotic pressure is the pressure required to prevent osmosis across a semipermeable membrane.
  • Tonicity refers to the ability of an extracellular solution to cause water movement into or out of a cell. There are three types of tonicity: hypotonic (lower solute concentration than the cell), hypertonic (higher solute concentration than the cell), and isotonic (equal solute concentration to the cell).
  • IV fluid types are an example of isotonic, hypertonic or hypotonic solutions.

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Description

Test your knowledge on solutions and solubility concepts in chemistry. This quiz covers topics such as solute and solvent interactions, factors affecting solubility, and the impact of temperature and pressure. Perfect for students looking to reinforce their understanding of solution chemistry.

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