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. b.How many moles of NH₃ would be released from 1.0 L of a saturated NH₃ solution if the temperature was increased from 25 to 50 °C?

Verified step by step guidance

1. Determine the solubility of NH₃ at both temperatures: 51.8 g/100 mL at 25°C and 27.0 g/100 mL at 50°C.
2. Calculate the mass of NH₃ in 1.0 L (1000 mL) of solution at 25°C using the solubility value.
3. Calculate the mass of NH₃ in 1.0 L (1000 mL) of solution at 50°C using the solubility value.
4. Find the difference in mass of NH₃ between the two temperatures to determine how much NH₃ is released.
5. Convert the mass of NH₃ released to moles using the molar mass of NH₃ (17.03 g/mol).

Key Concepts

Solubility

Solubility refers to the maximum amount of a substance that can dissolve in a given volume of solvent at a specific temperature and pressure. In this case, the solubility of ammonia (NH₃) in water is provided at two different temperatures, indicating how temperature affects the amount of gas that can be dissolved in the liquid.

Molarity and Moles

Molarity is a measure of concentration, defined as the number of moles of solute per liter of solution. To find the number of moles of NH₃ released when the temperature increases, one must calculate the difference in solubility at the two temperatures and then convert that difference into moles using the volume of the solution.

Henry's Law

Henry's Law states that the amount of gas that dissolves in a liquid at a given temperature is proportional to the partial pressure of that gas above the liquid. This principle helps explain the changes in solubility of NH₃ with temperature, as increasing temperature typically decreases gas solubility, leading to the release of dissolved gas when the temperature rises.