Solubility of AgCl in 10–2M NaCl solution is (Ksp(AgCl) = 1.8 × 10–10)10–2 M1.8 × 10–12 M1.8 × 10–8 M1.8 × 10–2 M

The solubility of AgCl in a NaCl solution can be calculated using the solubility product constant (Ksp) and the common ion effect.

Step 1: Write the balanced chemical equation for the dissolution of AgCl in water: AgCl(s) ⇌ Ag+(aq) + Cl-(aq)

Step 2: Write the expression for the solubility product constant: Ksp = [Ag+][Cl-]

Step 3: In a 10^-2 M NaCl solution, the concentration of Cl- ions is 10^-2 M due to the NaCl. When AgCl dissolves, it will also contribute to the Cl- concentration, but we will assume this contribution is small compared to the Cl- from NaCl, so we can approximate [Cl-] as 10^-2 M.

Step 4: Substitute the known values into the Ksp expression: 1.8 x 10^-10 = Ag+

Step 5: Solve for [Ag+], which represents the solubility of AgCl in the NaCl solution: [Ag+] = 1.8 x 10^-10 / 10^-2 = 1.8 x 10^-8 M

So, the solubility of AgCl in a 10^-2 M NaCl solution is approximately 1.8 x 10^-8 M.