What is the molar solubility of AgCl (K_sp = 1.6 × 10^-10) in 0.0020 M sodium chloride at 25°C?

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Quizplus · Accepted Answer

The molar solubility of AgCl in pure water is given by:K_sp = [Ag+][Cl-] = 1.6 × 10^-10In the presence of 0.0020 M sodium chloride, the common ion effect will decrease the solubility of AgCl. The new equilibrium expression is:K_sp = [Ag+][Cl-] = 1.6 × 10^-10 = [Ag+][0.0020 + x]Solving for x, we get:x = [Ag+] = 8.0 × 10^-8 MTherefore, the molar solubility of AgCl in 0.0020 M sodium chloride is 8.0 × 10^-8 M.

What Is the Molar Solubility of AgCl (Ksp = 1

What Is the Molar Solubility of AgCl (K_sp = 1