What is the Ksp of AgCl if the solubility of AgCl in water is 1.0 x 10^-5 M?

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Question: What is the Ksp of AgCl if the solubility of AgCl in water is 1.0 x 10^-5 M?

Options:

Correct Answer: 1.0 x 10^-10

Solution:

Ksp = [Ag+][Cl-] = (1.0 x 10^-5)(1.0 x 10^-5) = 1.0 x 10^-10.

What is the Ksp of AgCl if the solubility of AgCl in water is 1.0 x 10^-5 M?

What is the Ksp of AgCl if the solubility of AgCl in water is 1.0 x 10^-5 M?

Step 1: Understand that Ksp (solubility product constant) is calculated using the concentrations of the ions in a saturated solution.
Step 2: Recognize that AgCl (silver chloride) dissociates in water into Ag+ (silver ions) and Cl- (chloride ions).
Step 3: Write the dissociation equation: AgCl (s) ⇌ Ag+ (aq) + Cl- (aq).
Step 4: Note that the solubility of AgCl is given as 1.0 x 10^-5 M. This means that in a saturated solution, the concentration of Ag+ is 1.0 x 10^-5 M and the concentration of Cl- is also 1.0 x 10^-5 M.
Step 5: Use the Ksp formula: Ksp = [Ag+][Cl-].
Step 6: Substitute the values into the formula: Ksp = (1.0 x 10^-5)(1.0 x 10^-5).
Step 7: Calculate the result: Ksp = 1.0 x 10^-10.

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