Q: A closed canister contains $$0.103 \ \mathrm{M}$$ nitrogen. If Henry's Law constant for nitrogen in water is $$1.67 \times 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, which equation would you use to find the pressure?

$$P = \dfrac{C_{\text{gas}}}{k_H}$$

Q: The solubility of carbon dioxide in water at $$3.29 \ \mathrm{atm} is $$calculated using Henry's Law constant $$8.20 \times 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}. $$What is the solubility?

$$2.70 \times 10$$^{-3}$$ \ \mathrm{M}$$

Q: A patient is administered oxygen at $$2.0 \ \mathrm{atm}$$ pressure. If the Henry's Law constant for oxygen in blood is $$1.3 \times 10$$^{-3}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the concentration of dissolved oxygen in the blood?

$$2.6 \times 10$$^{-3}$$ \ \mathrm{M}$$

Q: A scuba diver descends to a depth where the partial pressure of nitrogen is $$3.0 \ \mathrm{atm}. If$$ $$k_H$$ for nitrogen in blood is $$6.0 \times 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the concentration of nitrogen dissolved in the diver's blood?

$$1.8 \times 10$$^{-3}$$ \ \mathrm{M}$$

Question 1

Which of the following best describes Henry's Law?

Accepted Answer

The solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

Question 2

Given Henry's Law constant for nitrogen in water is $$1.67 	imes 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the partial pressure (in atm) required to dissolve $$0.103 \ \mathrm{M}$$ nitrogen in water?

Accepted Answer

$$617.964 \ \mathrm{atm}$$

Question 3

If the solubility of oxygen gas in water at $$1.00 \ \mathrm{atm} is$$ $$0.84 \ \mathrm{g}$$ per $$1.0 \ \mathrm{L}$$, what would be the solubility at $$4.00 \ \mathrm{atm}$$?

Accepted Answer

$$3.36 \ \mathrm{g}$$

Question 4

A closed canister contains $$0.103 \ \mathrm{M}$$ nitrogen. If Henry's Law constant for nitrogen in water is $$1.67 	imes 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, which equation would you use to find the pressure?

Accepted Answer

$$P = \dfrac{C_{	ext{gas}}}{k_H}$$

Question 5

The solubility of carbon dioxide in water at $$3.29 \ \mathrm{atm} is $$calculated using Henry's Law constant $$8.20 	imes 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}. $$What is the solubility?

Accepted Answer

$$2.70 	imes 10$$^{-3}$$ \ \mathrm{M}$$

Question 6

If the solubility of dichloromethane, CH$$_2Cl$_2$$, at $$2.88 \ \mathrm{atm} is$$ $$0.384 \ \mathrm{mg/L}$$, what is the pressure when the solubility decreases to $$0.225 \ \mathrm{mg/L}$$?

Accepted Answer

$$1.69 \ \mathrm{atm}$$

Question 7

Which of the following is the correct two-point form of Henry's Law?

Accepted Answer

$$\dfrac{C_1$}{P_1$} = \dfrac{C_2$}{P_2$}$$

Question 8

A laboratory has an atmospheric pressure of $$1.3 \ \mathrm{atm}. If $$oxygen gas contributes $$62\% of $$this pressure, and Henry's Law constant for oxygen in water is $$5.3 	imes 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the mass of oxygen dissolved in $$2.5 \ \mathrm{L} of $$water at room temperature? (Molar mass of O$$_2 is$$ $$32.00 \ \mathrm{g/mol})$$

Accepted Answer

$$0.026 \ \mathrm{g}$$

Question 9

Which of the following would increase the solubility of a gas in water according to Henry's Law?

Accepted Answer

Increasing the partial pressure of the gas above the water.

Question 10

A patient is administered oxygen at $$2.0 \ \mathrm{atm}$$ pressure. If the Henry's Law constant for oxygen in blood is $$1.3 	imes 10$$^{-3}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the concentration of dissolved oxygen in the blood?

Accepted Answer

$$2.6 	imes 10$$^{-3}$$ \ \mathrm{M}$$

Question 11

If the partial pressure of a gas is doubled, what happens to its solubility in a liquid according to Henry's Law?

Accepted Answer

It doubles.

Question 12

Which of the following is NOT a correct unit for Henry's Law constant ($$k_H$$)?

Accepted Answer

$$\mathrm{atm} \cdot \mathrm{M}^{-1}$$

Question 13

A scuba diver descends to a depth where the partial pressure of nitrogen is $$3.0 \ \mathrm{atm}. If$$ $$k_H$$ for nitrogen in blood is $$6.0 	imes 10$$^{-4}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the concentration of nitrogen dissolved in the diver's blood?

Accepted Answer

$$1.8 	imes 10$$^{-3}$$ \ \mathrm{M}$$

Question 14

Which scenario best illustrates the application of Henry's Law in medicine?

Accepted Answer

Calculating the amount of anesthetic gas dissolved in blood at different pressures.

Question 15

If the Henry's Law constant for a gas decreases with increasing temperature, what does this imply about the solubility of the gas?

Accepted Answer

The solubility decreases as temperature increases.

Question 16

A soda bottle is sealed at $$4.0 \ \mathrm{atm} CO$_2$$ pressure. If the Henry's Law constant for CO$$_2 in $$water is $$3.4 	imes 10$$^{-2}$$ \ \mathrm{mol/L} \cdot \mathrm{atm}^{-1}$$, what is the concentration of CO$$_2 in $$the soda?

Accepted Answer

$$0.136 \ \mathrm{mol/L}$$

Question 17

Which of the following is a common misconception about Henry's Law?

Accepted Answer

The solubility of a gas in a liquid is only affected by pressure, not by temperature.

Question 18

A hospital uses nitrous oxide (N$$_2O) as an $$anesthetic. If the partial pressure of N$$_2O is$$ $$0.75 \ \mathrm{atm}$$ and $$k_H is$$ $$1.2 	imes 10$$^{-3}$$ \ \mathrm{M} \cdot \mathrm{atm}^{-1}$$, what is the concentration of N$$_2O $$dissolved in blood?

Accepted Answer

$$9.0 	imes 10$$^{-4}$$ \ \mathrm{M}$$

Question 19

If a gas has a very low Henry's Law constant, what does this indicate about its solubility in water?

Accepted Answer

It is not very soluble in water.

Henry's Law: Solubility of Gases in Liquids

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