Podcast
Questions and Answers
What occurs when ionic compounds are separated into their individual ions?
What occurs when ionic compounds are separated into their individual ions?
- Dissociation (correct)
- Precipitation
- Solvation
- Hydration
Which statement accurately describes a saturated solution?
Which statement accurately describes a saturated solution?
- It is at equilibrium with the solute and solvent. (correct)
- It contains no undissolved solute.
- It contains more solute than can usually dissolve.
- It is unable to dissolve any solute.
Which factor does NOT affect the solubility of a solute in a solvent?
Which factor does NOT affect the solubility of a solute in a solvent?
- Temperature of the solution
- Size of the solute particles (correct)
- Nature of the solute and solvent
- Pressure of the environment
What happens to the solubility of most solid solutes as temperature increases?
What happens to the solubility of most solid solutes as temperature increases?
Which of the following is an example of a covalent solid dissolving in water?
Which of the following is an example of a covalent solid dissolving in water?
What is the definition of 'hydration' in the context of solubility?
What is the definition of 'hydration' in the context of solubility?
What is true regarding the solubility of gases in liquids as temperature increases?
What is true regarding the solubility of gases in liquids as temperature increases?
What characterizes the particles in a colloid compared to those in a suspension?
What characterizes the particles in a colloid compared to those in a suspension?
What does 'like dissolves like' refer to in the context of solubility?
What does 'like dissolves like' refer to in the context of solubility?
In a dissociation equation, what are the products generated when a chemical dissolves?
In a dissociation equation, what are the products generated when a chemical dissolves?
What is the molarity of a solution if 0.75 moles of CaCl are dissolved in 2.5 liters of solution?
What is the molarity of a solution if 0.75 moles of CaCl are dissolved in 2.5 liters of solution?
How many grams of KCl are needed to create a 0.2 M solution in 1.8 L of water?
How many grams of KCl are needed to create a 0.2 M solution in 1.8 L of water?
If you need to dilute 18 M H2SO4 to create 2 M H2SO4, how much of the concentrated solution is required for 1.5 L of the diluted solution?
If you need to dilute 18 M H2SO4 to create 2 M H2SO4, how much of the concentrated solution is required for 1.5 L of the diluted solution?
To what volume does 10 g of NaCl increase the molarity of an existing 180 mL solution to get the new molarity?
To what volume does 10 g of NaCl increase the molarity of an existing 180 mL solution to get the new molarity?
What does Henry's law state regarding the solubility of gases?
What does Henry's law state regarding the solubility of gases?
What is the relationship between molarity (M) and concentration?
What is the relationship between molarity (M) and concentration?
Which of the following is NOT a factor affecting the rate of dissolving?
Which of the following is NOT a factor affecting the rate of dissolving?
What does a chemical need to be classified as an electrolyte?
What does a chemical need to be classified as an electrolyte?
What characterizes an undersaturated solution?
What characterizes an undersaturated solution?
Which colligative property relates to the need for more heat to boil a solution?
Which colligative property relates to the need for more heat to boil a solution?
How does the presence of a solute in a solution affect vapor pressure?
How does the presence of a solute in a solution affect vapor pressure?
What is a key characteristic of a suspension?
What is a key characteristic of a suspension?
What happens to the freezing point of water when a solute is added?
What happens to the freezing point of water when a solute is added?
What differentiates a solution from a mixture?
What differentiates a solution from a mixture?
What is the molarity of the new solution after adding 10g of NaCl to the original 0.18L solution?
What is the molarity of the new solution after adding 10g of NaCl to the original 0.18L solution?
How many moles of HCl are present in 1.5L of a 3.5M solution?
How many moles of HCl are present in 1.5L of a 3.5M solution?
Using reaction stoichiometry, how many moles of Mg are required to react with 5.25 moles of HCl?
Using reaction stoichiometry, how many moles of Mg are required to react with 5.25 moles of HCl?
What is the molarity of the solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?
What is the molarity of the solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?
What is the final mass of Na2SO4 formed when 500ml of a 4.5M solution of H2SO4 is mixed with excess NaOH?
What is the final mass of Na2SO4 formed when 500ml of a 4.5M solution of H2SO4 is mixed with excess NaOH?
How many grams of magnesium (Mg) are needed to react with 5.25 moles of HCl?
How many grams of magnesium (Mg) are needed to react with 5.25 moles of HCl?
Which balanced equation correctly represents the reaction between sulfuric acid and sodium hydroxide?
Which balanced equation correctly represents the reaction between sulfuric acid and sodium hydroxide?
What is the total volume of the resulting solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?
What is the total volume of the resulting solution when 150 ml of a 2M solution is mixed with 550 ml of a 3.5M solution?
What is the term used when solvent molecules surround solute molecules?
What is the term used when solvent molecules surround solute molecules?
What happens to the solubility of gases in liquids at higher temperatures?
What happens to the solubility of gases in liquids at higher temperatures?
Which of the following best describes a saturated solution?
Which of the following best describes a saturated solution?
What does the term 'crystallization' refer to in the context of solutions?
What does the term 'crystallization' refer to in the context of solutions?
What characteristic best illustrates the phrase 'like dissolves like'?
What characteristic best illustrates the phrase 'like dissolves like'?
Which condition is required for a solution to be classified as super-saturated?
Which condition is required for a solution to be classified as super-saturated?
In which scenario would you expect an increase in the solubility of a solid solute?
In which scenario would you expect an increase in the solubility of a solid solute?
What is the primary factor that affects the rate of dissolving an ionic solid in water?
What is the primary factor that affects the rate of dissolving an ionic solid in water?
What is the molarity of a solution that contains 50g of sodium chloride (NaCl) dissolved in 1L of water? (Molar mass of NaCl = 58.44 g/mol)
What is the molarity of a solution that contains 50g of sodium chloride (NaCl) dissolved in 1L of water? (Molar mass of NaCl = 58.44 g/mol)
How many grams of potassium chloride (KCl) are in a 0.5 M solution with a total volume of 3 L? (Molar mass of KCl = 74.55 g/mol)
How many grams of potassium chloride (KCl) are in a 0.5 M solution with a total volume of 3 L? (Molar mass of KCl = 74.55 g/mol)
What is the final concentration of sodium chloride after mixing 100 mL of a 3M solution with 400 mL of a 1.5M solution?
What is the final concentration of sodium chloride after mixing 100 mL of a 3M solution with 400 mL of a 1.5M solution?
What volume of water is needed to dilute 500 mL of a 5M solution of HCl to a 1M solution?
What volume of water is needed to dilute 500 mL of a 5M solution of HCl to a 1M solution?
To create a 0.5 M solution, how many moles of solute are needed in 1.5 L of solution?
To create a 0.5 M solution, how many moles of solute are needed in 1.5 L of solution?
What final concentration results from combining 250 mL of a 2M solution and 750 mL of a 4M solution?
What final concentration results from combining 250 mL of a 2M solution and 750 mL of a 4M solution?
If 10g of NaCl are added to 500 mL of a solution already at 1 M, what will be the new molarity? (NaCl = 58.44 g/mol)
If 10g of NaCl are added to 500 mL of a solution already at 1 M, what will be the new molarity? (NaCl = 58.44 g/mol)
What is the number of moles in 2 L of a 2.5M solution?
What is the number of moles in 2 L of a 2.5M solution?
What effect does increasing the surface area of a solute have on its rate of dissolving?
What effect does increasing the surface area of a solute have on its rate of dissolving?
How does the presence of a solute affect the boiling point of a solution compared to pure solvent?
How does the presence of a solute affect the boiling point of a solution compared to pure solvent?
Which of the following correctly describes an undersaturated solution?
Which of the following correctly describes an undersaturated solution?
What happens to the freezing point of a solution when a solute is added?
What happens to the freezing point of a solution when a solute is added?
Which of the following is NOT a colligative property?
Which of the following is NOT a colligative property?
What is the relationship described by Henry's law?
What is the relationship described by Henry's law?
What characterizes a suspension compared to a colloid?
What characterizes a suspension compared to a colloid?
What is indicated by a high vapor pressure in a liquid?
What is indicated by a high vapor pressure in a liquid?
What is the final molarity of the new solution after adding 10g of NaCl to the original 0.18L solution with a molarity of 1.5M?
What is the final molarity of the new solution after adding 10g of NaCl to the original 0.18L solution with a molarity of 1.5M?
How many moles of magnesium (Mg) are needed to react with 5.25 moles of hydrochloric acid (HCl)?
How many moles of magnesium (Mg) are needed to react with 5.25 moles of hydrochloric acid (HCl)?
What is the total volume of the resulting solution when mixing 150 mL of a 2M solution with 550 mL of a 3.5M solution?
What is the total volume of the resulting solution when mixing 150 mL of a 2M solution with 550 mL of a 3.5M solution?
How many grams of Na2SO4 are produced when 500 mL of a 4.5M solution of H2SO4 is reacted with excess NaOH?
How many grams of Na2SO4 are produced when 500 mL of a 4.5M solution of H2SO4 is reacted with excess NaOH?
Given the molar masses of Na (22.989 g/mol) and Cl (35.457 g/mol), what is the total mass of NaCl produced from 0.17 moles?
Given the molar masses of Na (22.989 g/mol) and Cl (35.457 g/mol), what is the total mass of NaCl produced from 0.17 moles?
What is the molarity of HCl if 1.5L of 3.5M solution provides how many moles of HCl?
What is the molarity of HCl if 1.5L of 3.5M solution provides how many moles of HCl?
What stoichiometric relationship can be established from the reaction between Mg and HCl?
What stoichiometric relationship can be established from the reaction between Mg and HCl?
When diluting a solution, what would be the correct formula to calculate molarity after mixing different volumes?
When diluting a solution, what would be the correct formula to calculate molarity after mixing different volumes?
Flashcards
Solubility
Solubility
The maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature.
Dissolving ionic solids
Dissolving ionic solids
Ionic compounds separate into their constituent ions when mixed with a polar solvent like water.
Solvation
Solvation
A process where solute molecules are surrounded by solvent molecules.
Saturated solution
Saturated solution
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Solubility of solids
Solubility of solids
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Solubility of gases
Solubility of gases
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Like dissolves like
Like dissolves like
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Crystal Structure/Lattice
Crystal Structure/Lattice
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Solubility of gases in liquids & Pressure
Solubility of gases in liquids & Pressure
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Factors affecting dissolving rate
Factors affecting dissolving rate
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Types of solutions
Types of solutions
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Colligative Properties
Colligative Properties
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Vapor Pressure
Vapor Pressure
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Vapor Pressure Reduction
Vapor Pressure Reduction
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Boiling Point Elevation
Boiling Point Elevation
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Freezing Point Depression
Freezing Point Depression
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Dissociation Equation
Dissociation Equation
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Electrolyte
Electrolyte
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Molarity (M)
Molarity (M)
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Molarity Calculation
Molarity Calculation
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Dilution
Dilution
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Mixing Solution Calculation, M1V1=M2V2
Mixing Solution Calculation, M1V1=M2V2
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Mole Calculation
Mole Calculation
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Steps to find moles of solute from mass and concentration
Steps to find moles of solute from mass and concentration
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Molarity of NaCl solution
Molarity of NaCl solution
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Calculate moles of NaCl
Calculate moles of NaCl
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Calculate the total moles of final solution
Calculate the total moles of final solution
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Calculate final molarity
Calculate final molarity
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Reaction Stoichiometry
Reaction Stoichiometry
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Moles of HCl calculation
Moles of HCl calculation
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Convert Moles to Grams
Convert Moles to Grams
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Calculate Moles from Balanced Equation
Calculate Moles from Balanced Equation
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Dissociation
Dissociation
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What happens to the solubility of a solid as temperature increases?
What happens to the solubility of a solid as temperature increases?
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What happens to the solubility of a gas as temperature increases?
What happens to the solubility of a gas as temperature increases?
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What is the 'like dissolves like' rule?
What is the 'like dissolves like' rule?
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Undersaturated solution
Undersaturated solution
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Supersaturated solution
Supersaturated solution
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Henry's Law
Henry's Law
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Surface Area & Dissolving
Surface Area & Dissolving
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Solute Concentration & Dissolving
Solute Concentration & Dissolving
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How many moles of solute are in a solution?
How many moles of solute are in a solution?
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How many grams of solute are in a solution?
How many grams of solute are in a solution?
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M1V1=M2V2
M1V1=M2V2
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Mixing Solutions
Mixing Solutions
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Molarity Formula
Molarity Formula
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Calculating Moles from Molarity
Calculating Moles from Molarity
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Final Molarity
Final Molarity
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Balanced Chemical Equation
Balanced Chemical Equation
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Calculating Moles from a Balanced Equation
Calculating Moles from a Balanced Equation
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Study Notes
Solubility Unit
- Ionic compounds arrange themselves to increase attractive forces between ions and decrease repulsive forces. This arrangement is known as a crystal structure or lattice.
- Polar solvent molecules surround each ion.
- Separation of ions is called dissociation.
- Solvation is when solute molecules are surrounded by solvent molecules.
- Hydration is solvation when the solvent is water.
- Covalent molecules are held together by weak intermolecular forces.
- During solvation, each molecule is surrounded by solvent molecules.
- Solvents do not appear in dissolving equations.
- Ionic solids separate into ions (e.g., NH₄NO₃ → NH₄⁺(aq) + NO₃⁻(aq)).
- Covalent solids just separate between molecules (e.g., C₆H₁₂O₆(s) → C₆H₁₂O₆(aq)).
Definitions
- Undersaturated: A solution containing less than the maximum amount of solute that can be dissolved (dissolving > crystallization).
- Saturated: A solution containing the maximum amount of solute that can be dissolved (dissolving = crystallization).
- Supersaturated: A solution containing more than the maximum amount of solute under special conditions, but crystallization does not occur.
Factors Affecting Solubility
- Nature of Solute and Solvent ("Like Dissolves Like"):
- Substances with similar intermolecular forces dissolve each other more readily.
- Polar substances dissolve polar substances, and nonpolar substances dissolve nonpolar substances.
- Temperature:
- Generally, the solubility of a solid or liquid solute increases with temperature. (e.g., sugar in hot tea vs. cold tea).
- Solubility of gases decreases with increasing temperature.
- Particles with more kinetic energy can escape the solution more quickly (e.g., cold pop vs. warm pop).
- Pressure:
- Only applies to solutions of gases in liquids.
- Henry's Law: The solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid.
Rate of Dissolving
- Surface Area: Increasing surface area increases solute-solvent collisions, leading to faster dissolving (e.g., dissolving a cube of sugar vs. a teaspoon of sugar).
- Amount of Solute Already Dissolved: As a solution approaches saturation, dissolving becomes slower.
- Equilibrium: Dissolving and crystallization occur at the same rate in a saturated solution. This is called equilibrium.
- Solubility: The maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature.
Colligative Properties
- Colligative properties depend on the concentration of solute particles (number), not the type of solute.
- Vapor Pressure Reduction: Solute particles interfere with evaporation, lowering the vapor pressure of a solution.
- Boiling Point Elevation: Increased pressure requires a higher temperature for boiling.
- Freezing Point Depression: Solute particles disrupt the formation of the solid phase, lowering the freezing point of a solution.
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Description
Test your knowledge on the solubility unit, covering key concepts such as ionic and covalent solvation, dissociation, and hydration. This quiz will challenge your understanding of how different types of compounds interact with solvents and the definitions of supersaturated, saturated, and undersaturated solutions.
