QuestionMay 27, 2025

Which of these factors will NOT decrease the solubility of gases in solution? a decrease in the partial pressure of that gas an increase in temperature an increase in ionic concentration All three factors will decrease the solubility of a gas in solution.

Which of these factors will NOT decrease the solubility of gases in solution? a decrease in the partial pressure of that gas an increase in temperature an increase in ionic concentration All three factors will decrease the solubility of a gas in solution.
Which of these factors will NOT decrease the solubility of gases in solution?
a decrease in the partial pressure of that gas
an increase in temperature
an increase in ionic concentration
All three factors will decrease the solubility of a gas in solution.

Solution
4.6(353 votes)

Answer

All three factors will decrease the solubility of a gas in solution. Explanation 1. Analyze the effect of partial pressure According to **Henry's Law**, solubility of a gas is directly proportional to its partial pressure. A decrease in partial pressure decreases solubility. 2. Analyze the effect of temperature Generally, an increase in temperature decreases the solubility of gases in liquids because gases tend to escape from the solution at higher temperatures. 3. Analyze the effect of ionic concentration An increase in ionic concentration can lead to the "salting out" effect, which decreases the solubility of gases.

Explanation

1. Analyze the effect of partial pressure<br /> According to **Henry's Law**, solubility of a gas is directly proportional to its partial pressure. A decrease in partial pressure decreases solubility.<br /><br />2. Analyze the effect of temperature<br /> Generally, an increase in temperature decreases the solubility of gases in liquids because gases tend to escape from the solution at higher temperatures.<br /><br />3. Analyze the effect of ionic concentration<br /> An increase in ionic concentration can lead to the "salting out" effect, which decreases the solubility of gases.
Click to rate:

Similar Questions