Question

How do we determine Ksp and Kspo for 1:1 salts (like NaCl, AgCl, etc)?

a) By measuring solvation energy.
b) By conducting titrations.
c) By calculating ionic strength.
d) By assessing solubility product.

Answer 1

The solubility product constant (Ksp) for salts like NaCl or AgCl is determined by measuring their solubility and using the equilibrium concentrations of the resulting ions to calculate Ksp, not by other means such as solvation energy or titrations.

Step-by-step explanation:

We determine the solubility product constant (Ksp) for 1:1 salts such as NaCl or AgCl by assessing their solubility product, not by measuring solvation energy, conducting titrations, or calculating ionic strength. The Ksp can be derived from the measured solubility of the compound in water. When a salt dissolves and dissociates into its constituent ions, the concentrations of these ions at equilibrium can be used to calculate the Ksp value. In the case of AgCl in a KCl solution, for instance, if the solubility of AgCl is represented as x, the ion concentrations at equilibrium would be [Ag+] = x M and [Cl­] = (1.0 + x) M. By assuming x is significantly smaller than 1.0, the Ksp can be approximated as [Ag+][Cl­] = x(1.0).