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Questions and Answers
What is the mass percent concentration of a solution containing 50 g of solute in a solution with a total mass of 200 g?
What is the mass percent concentration of a solution containing 50 g of solute in a solution with a total mass of 200 g?
- 25% (correct)
- 30%
- 15%
- 20%
If a solution has a volume of 250 mL and contains 25 mL of alcohol, what is the percent by volume of the solute in this solution?
If a solution has a volume of 250 mL and contains 25 mL of alcohol, what is the percent by volume of the solute in this solution?
- 12%
- 30%
- 25% (correct)
- 10%
What is the formula for calculating percent by mass-volume concentration?
What is the formula for calculating percent by mass-volume concentration?
- (mass of solute in grams / volume of solution in mL) * 100 (correct)
- (mass of solute in grams / mass of solution in grams) * 100
- (volume of solute in mL / volume of solution in mL) * 100
- (volume of solute in mL / mass of solution in grams) * 100
In a solution where the mole fraction of solute is 0.2, what is the mole fraction of the solvent?
In a solution where the mole fraction of solute is 0.2, what is the mole fraction of the solvent?
If a saline solution weighs 400 g and contains 40 g of NaCl, what is the mass percent of the NaCl in the solution?
If a saline solution weighs 400 g and contains 40 g of NaCl, what is the mass percent of the NaCl in the solution?
How many grams of solute are in 150 mL of a 20% by mass-volume solution?
How many grams of solute are in 150 mL of a 20% by mass-volume solution?
What is the molarity of a solution that contains 5 moles of solute in 2 liters of solution?
What is the molarity of a solution that contains 5 moles of solute in 2 liters of solution?
What is the total number of moles of solute if 30 g of NaCl (molar mass = 58.44 g/mol) is dissolved in a solution?
What is the total number of moles of solute if 30 g of NaCl (molar mass = 58.44 g/mol) is dissolved in a solution?
In the solution of 25 grams of salt dissolved in 95 mL of water, which substance is the solute?
In the solution of 25 grams of salt dissolved in 95 mL of water, which substance is the solute?
Which of the following is an example of a gas-liquid solution?
Which of the following is an example of a gas-liquid solution?
What is the primary characteristic of a saturated solution?
What is the primary characteristic of a saturated solution?
Which of the following correctly defines a colligative property?
Which of the following correctly defines a colligative property?
In which solution type is the solute present in a larger quantity than the solvent?
In which solution type is the solute present in a larger quantity than the solvent?
Which term describes a solution that contains more solute than can typically be dissolved at a given temperature?
Which term describes a solution that contains more solute than can typically be dissolved at a given temperature?
What is the role of the solvent in a solution?
What is the role of the solvent in a solution?
Which of the following states a property unique to electrolyte solutions compared to nonelectrolyte solutions?
Which of the following states a property unique to electrolyte solutions compared to nonelectrolyte solutions?
What characterizes an unsaturated solution?
What characterizes an unsaturated solution?
What happens in a supersaturated solution when a seed crystal is added?
What happens in a supersaturated solution when a seed crystal is added?
Which step is NOT involved in the formation of a liquid solution?
Which step is NOT involved in the formation of a liquid solution?
What does a positive enthalpy of solution indicate?
What does a positive enthalpy of solution indicate?
Why is it important to express solutions in correct concentration units?
Why is it important to express solutions in correct concentration units?
When is a solution considered saturated?
When is a solution considered saturated?
Which of the following best describes the process of seeding in a supersaturated solution?
Which of the following best describes the process of seeding in a supersaturated solution?
What is true about the categorization of solutions based on their concentrations?
What is true about the categorization of solutions based on their concentrations?
What is the molar mass of NaF?
What is the molar mass of NaF?
How many moles of solvent are in 200 g of water (H2O)?
How many moles of solvent are in 200 g of water (H2O)?
What is the total moles of the solution when combining 0.60 moles of NaF and 11.11 moles of H2O?
What is the total moles of the solution when combining 0.60 moles of NaF and 11.11 moles of H2O?
What is the mole fraction of NaF in the solution?
What is the mole fraction of NaF in the solution?
In calculating mole fractions, what does the formula $X_{solute} + X_{solvent} = 1$ signify?
In calculating mole fractions, what does the formula $X_{solute} + X_{solvent} = 1$ signify?
What is the molality of a solution containing 16.5 g of dissolved naphthalene in 0.0543 kg of benzene?
What is the molality of a solution containing 16.5 g of dissolved naphthalene in 0.0543 kg of benzene?
When 25 g of NaF is added to 200 g of H2O, what would be the expected change in the mole fraction of water?
When 25 g of NaF is added to 200 g of H2O, what would be the expected change in the mole fraction of water?
What is the combined effect of solute and solvent on the overall mole fraction calculations?
What is the combined effect of solute and solvent on the overall mole fraction calculations?
What is the molar mass of naphthalene (C10H8) based on its composition?
What is the molar mass of naphthalene (C10H8) based on its composition?
How many moles of C10H8 are present in a solution with 16.5 g of naphthalene?
How many moles of C10H8 are present in a solution with 16.5 g of naphthalene?
What is the weight of the solvent in kilograms used in the calculation of molality for the naphthalene solution?
What is the weight of the solvent in kilograms used in the calculation of molality for the naphthalene solution?
Which formula is used to calculate the molality of a solution?
Which formula is used to calculate the molality of a solution?
If 25 grams of sodium chloride (NaCl) are dissolved in 100 grams of water, what is the primary concentration measure being calculated?
If 25 grams of sodium chloride (NaCl) are dissolved in 100 grams of water, what is the primary concentration measure being calculated?
Calculate the molality of a solution containing 0.132 moles of solute in 0.0543 kg of solvent. What is the result?
Calculate the molality of a solution containing 0.132 moles of solute in 0.0543 kg of solvent. What is the result?
What is the given mass of NaCl in the example problem for molarity calculation?
What is the given mass of NaCl in the example problem for molarity calculation?
What is the total molar mass of sodium chloride (NaCl) based on its atomic constituents?
What is the total molar mass of sodium chloride (NaCl) based on its atomic constituents?
Flashcards
Solution
Solution
A homogeneous mixture where one substance (the solute) dissolves in another substance (the solvent).
Solute
Solute
The substance that is dissolved in a solution. It is usually present in a smaller amount.
Solvent
Solvent
The substance that dissolves the solute in a solution. It is usually present in a larger amount.
Saturated solution
Saturated solution
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Unsaturated solution
Unsaturated solution
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Supersaturated solution
Supersaturated solution
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Gas in solid solution
Gas in solid solution
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Liquid in solid solution
Liquid in solid solution
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Enthalpy of Solution
Enthalpy of Solution
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Concentration of Solution
Concentration of Solution
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Percent by Mass
Percent by Mass
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Solution Formation
Solution Formation
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Energy of Solution Formation
Energy of Solution Formation
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Percent by Volume
Percent by Volume
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Percent by Mass-Volume
Percent by Mass-Volume
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Mole Fraction
Mole Fraction
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Molality
Molality
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Molarity
Molarity
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Parts per Million (ppm)
Parts per Million (ppm)
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What is the formula for mole fraction?
What is the formula for mole fraction?
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What is mole fraction?
What is mole fraction?
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What is the rule regarding mole fractions in a solution?
What is the rule regarding mole fractions in a solution?
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How do you calculate the mole fraction of a solute?
How do you calculate the mole fraction of a solute?
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What is molality?
What is molality?
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How do you calculate molality?
How do you calculate molality?
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What is naphthalene?
What is naphthalene?
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What is benzene?
What is benzene?
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What is ethanol?
What is ethanol?
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What are parts per million (ppm)?
What are parts per million (ppm)?
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What are parts per billion (ppb)?
What are parts per billion (ppb)?
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What are the different ways to express concentration?
What are the different ways to express concentration?
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When are different concentration units used?
When are different concentration units used?
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Study Notes
General Chemistry II - Chapter 2: Solutions and Their Properties
- This chapter covers solutions and their properties, including different concentration expressions, stoichiometric calculations for reactions in solution, and the effect of concentration on colligative properties.
Most Essential Learning Competencies
- Competency 1: Express solution concentration using various methods: percent by mass, mole fraction, molarity, molality, percent by volume, and parts per million (ppm).
- Competency 2: Perform stoichiometric calculations for reactions in solution.
- Competency 3: Describe the effect of concentration on colligative properties of solutions.
- Competency 4: Differentiate colligative properties of nonelectrolyte and electrolyte solutions.
- Competency 5: Calculate boiling point elevation and freezing point depression based on solute concentration.
- Competency 6: Calculate molar mass from colligative property data.
- Competency 7: Describe laboratory procedures for determining solution concentration.
Section 2.1: Types of Solutions
- EQ: What types of solutions are encountered everyday?
- A solution is a homogenous mixture of two or more substances.
- Atoms, ions, or molecules are uniformly distributed in a single phase.
- Solutions consist of a solute (substance dissolved) and a solvent (dissolving medium). Typically, the solute is present in a smaller amount.
Types of Solutions (examples)
- Gas in gas (e.g., oxygen in nitrogen)
- Gas in liquid (e.g., carbon dioxide in water)
- Gas in solid (e.g., hydrogen in palladium)
- Liquid in liquid (e.g., ethanol in water)
- Liquid in solid (e.g., mercury in silver)
- Solid in liquid (e.g., salt in water)
- Solid in solid (e.g., copper in tin, bronze)
Types of Solutions
- Unsaturated Solution: Contains less solute than the solvent's capacity to dissolve more.
- Saturated Solution: Contains the maximum amount of solute that can dissolve at a given temperature.
- Supersaturated Solution: Contains more solute than a saturated solution at the same temperature. This type of solution is unstable. Excess solute can crystallize by adding a 'seed crystal' or by scratching the container.
Section 2.2: Energy of Solution Formation
- EQ: How do liquid solutions form?
- For substances to form a solution, they generally need similar polarities.
- Solution formation takes three steps:
- 1. Overcoming intermolecular forces in the solvent: Enables space for the solute.
- 2. Separating the solute into its individual components: Breaking attractions between solute particles.
- 3. Allowing solute–solvent interactions to form the solution: Developing attractive forces between solute and solvent.
Enthalpy of Solution
- The enthalpy change associated with solution formation.
- It’s the sum of the enthalpy changes for the three steps.
- A positive enthalpy change indicates an endothermic process (absorbing heat). A negative enthalpy change indicates an exothermic process (releasing heat).
Section 2.3: Concentration of Solutions
- EQ: Why must solution concentrations be expressed correctly?
- Concentration measures the amount of solute in a given amount of solvent or solution.
- Different solution types can have different concentrations.
Concentration of a Solution (Examples of Units)
- Percent by Mass: (mass of solute / mass of solution) x 100
- Percent by Volume: (volume of solute / volume of solution) x 100
- Percent by Mass-Volume: (mass of solute / volume of solution) x 100
- Mole Fraction: Moles of component / Total moles in solution
- Molality: Moles of solute / Kilograms of solvent
- Molarity: Moles of solute / Liters of solution
- Parts Per Million (ppm): (mass of solute / mass of solution) x 106
- Parts Per Billion (ppb): (mass of solute / mass of solution) x 109
Sample Problems (examples)
- Various calculations are provided using the different concentration units, including calculations to determine different concentrations.
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Description
Test your knowledge on various concentration calculations, including mass percent, volume percent, and molarity. This quiz features problems related to solutions and their components, providing an opportunity to apply your understanding of chemistry concepts. Perfect for students tackling solution chemistry topics!
