Question

At 25 %C, only 0.0450 mol of the generic salt AB is soluble in 1.00 L of water: What is the Ksp of the salt at 25 %C? AB(s) ~^ A+(aq) + B (aq) Ksp

Answer 1

The Ksp of the generic salt AB at 25°C is calculated by squaring the solubility in moles per liter (0.0450 mol/L), resulting in a Ksp value of 0.002025.

Step-by-step explanation:

The solubility product constant, or Ksp, is a value that indicates the solubility of a sparingly soluble salt in water. For a simple salt such as AB, which dissociates into A+ and B- in solution, the Ksp can be calculated if the solubility is known.

In this case, the solubility given is 0.0450 mol/L for AB at 25 ℃. When AB dissolves in water, it forms equal molar amounts of A+ and B- ions:

• AB(s) ⇌ A+(aq) + B-(aq)

The Ksp expression is:

Ksp = [A+][B-] = (s)(s) = s2

where s represents the solubility in moles per litre (mol/L). Substituting the value of s (0.0450 mol/L), we get:

Ksp = (0.0450)2 = 0.002025

The Ksp for AB at 25 ℃ is therefore 0.002025.

Answer 2

The solubility product constant (Ksp) for the salt AB, with a 1:1 stoichiometry, is calculated by squaring the solubility in moles per liter. The given solubility is 0.0450 M, so the Ksp is 2.025 × 10^-3 at 25 °C.

Step-by-step explanation:

To determine the solubility product constant (Ksp) of the salt AB at 25 °C, we can refer to the dissolution reaction AB(s) → A+(aq) + B-(aq). Given that 0.0450 mol of AB dissolves in 1.00 L of water, we can state the molar solubility of A+ and B- is also 0.0450 M, assuming a 1:1 stoichiometry as implied by the formula AB. The Ksp can be calculated using the molar solubility of the ions.

The formula to calculate Ksp is:

Ksp = [A+][B-]

Substituting the molar solubility:

Ksp = (0.0450 M)(0.0450 M) = 0.0450^2 M²

The calculated Ksp is therefore:

Ksp = 2.025 × 10^-3

Note that the stoichiometry of the dissolution reaction directly affects the relationship between solubility and Ksp.