The solubility of NH₃ gas in water at an NH₃ pressure of 760.0 mmHg and 25°C is 51.8 g/100 mL and 27.0 g/100 mL at 50°C. a.What is the solubility of NH₃ if its partial pressure is reduced to 225.0 mmHg?

Verified step by step guidance

1. Identify that the problem involves the solubility of a gas (NH₃) in a liquid (water) and how it changes with pressure, which is described by Henry's Law.
2. Recall Henry's Law: $S_1/P_1=S_2/P_2$, where $S$ is the solubility and $P$ is the pressure.
3. Use the given solubility at 760.0 mmHg and 25°C to find the Henry's Law constant: $k_H=S_1/P_1$.
4. Set up the equation using the Henry's Law constant to find the new solubility $S_2$ at the reduced pressure of 225.0 mmHg: $S_2=k_H\times P_2$.
5. Solve for $S_2$ using the calculated Henry's Law constant and the new pressure.

Key Concepts

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is directly proportional to the partial pressure of that gas above the liquid. This principle is crucial for understanding how changes in pressure affect the solubility of gases, such as NH₃, in water.

Solubility

Solubility refers to the maximum amount of a substance that can dissolve in a given quantity of solvent at a specific temperature and pressure. In this context, it is important to know how solubility values change with temperature and pressure to calculate the solubility of NH₃ at different conditions.

Temperature Effects on Solubility

Temperature can significantly influence the solubility of gases in liquids. Generally, as temperature increases, the solubility of gases decreases. Understanding this relationship helps in predicting how the solubility of NH₃ will change when the temperature is altered, as seen in the provided data.