the proportional relationship between the concentration of dissolved gas in a solution and the partial pressure of the gas in contact with the solution

of negligible mutual solubility; typically refers to liquid substances

mutually soluble in all proportions; typically refers to liquid substances

of moderate mutual solubility; typically refers to liquid substances

of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure

extent to which a solute may be dissolved in water, or any solvent

of concentration that exceeds solubility; a nonequilibrium state

of concentration less than solubility

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Chemistry 2e · 11.3 Solubility

Solubility: practice problems

5 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 17
Supersaturated solutions of most solids in water are prepared by cooling saturated solutions. Supersaturated solutions of most gases in water are prepared by heating saturated solutions. Explain the reasons for the difference in the two procedures.
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Exercises 19
Calculate the percent by mass of KBr in a saturated solution of KBr in water at 10 °C. See Figure 11.16 for useful data, and report the computed percentage to one significant digit.
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Exercises 21
At 0 °C and 1.00 atm, as much as 0.70 g of O₂ can dissolve in 1 L of water. At 0 °C and 4.00 atm, how many grams of O₂ dissolve in 1 L of water?
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Exercises 23
The Henry’s law constant for CO₂ is 3.4 $\times$ 10⁻² M/atm at 25 °C. Assuming ideal solution behavior, what pressure of carbon dioxide is needed to maintain a CO₂ concentration of 0.10 M in a can of lemon-lime soda?
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Exercises 25
Assuming ideal solution behavior, how many liters of HCl gas, measured at 30.0 °C and 745 torr, are required to prepare 1.25 L of a 3.20-M solution of hydrochloric acid?
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Key terms · 8

Henry’s law: the proportional relationship between the concentration of dissolved gas in a solution and the partial pressure of the gas in contact with the solution
immiscible: of negligible mutual solubility; typically refers to liquid substances
miscible: mutually soluble in all proportions; typically refers to liquid substances
partially miscible: of moderate mutual solubility; typically refers to liquid substances
saturated: of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure
solubility: extent to which a solute may be dissolved in water, or any solvent
supersaturated: of concentration that exceeds solubility; a nonequilibrium state
unsaturated: of concentration less than solubility

Learn 11.3 on the whiteboard

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.

Read 11.3 in the textbook · This section on openstax.org

Solubility: practice problems

5 problems from the book, with its answers. Check your working, or have any of them explained to you on the whiteboard.

Exercises 17

Supersaturated solutions of most solids in water are prepared by cooling saturated solutions. Supersaturated solutions of most gases in water are prepared by heating saturated solutions. Explain the reasons for the difference in the two procedures.

Exercises 19

Calculate the percent by mass of KBr in a saturated solution of KBr in water at 10 °C. See Figure 11.16 for useful data, and report the computed percentage to one significant digit.

Exercises 21

At 0 °C and 1.00 atm, as much as 0.70 g of O₂ can dissolve in 1 L of water. At 0 °C and 4.00 atm, how many grams of O₂ dissolve in 1 L of water?

Exercises 23

The Henry’s law constant for CO₂ is 3.4 $\times$ 10⁻² M/atm at 25 °C. Assuming ideal solution behavior, what pressure of carbon dioxide is needed to maintain a CO₂ concentration of 0.10 M in a can of lemon-lime soda?

Exercises 25

Assuming ideal solution behavior, how many liters of HCl gas, measured at 30.0 °C and 745 torr, are required to prepare 1.25 L of a 3.20-M solution of hydrochloric acid?

Key terms · 8

Henry’s law: the proportional relationship between the concentration of dissolved gas in a solution and the partial pressure of the gas in contact with the solution
immiscible: of negligible mutual solubility; typically refers to liquid substances
miscible: mutually soluble in all proportions; typically refers to liquid substances
partially miscible: of moderate mutual solubility; typically refers to liquid substances
saturated: of concentration equal to solubility; containing the maximum concentration of solute possible for a given temperature and pressure
solubility: extent to which a solute may be dissolved in water, or any solvent
supersaturated: of concentration that exceeds solubility; a nonequilibrium state
unsaturated: of concentration less than solubility

Learn 11.3 on the whiteboard

The tutor teaches the whole section, drawing it out step by step and answering your questions as you go.

Read 11.3 in the textbook · This section on openstax.org