If the solubility product (Ksp) of AgCl is 1.77 x 10^-10, what is the molar solu
Practice Questions
Q1
If the solubility product (Ksp) of AgCl is 1.77 x 10^-10, what is the molar solubility of AgCl?
1.77 x 10^-5 M
1.77 x 10^-10 M
1.77 x 10^-7 M
1.77 x 10^-3 M
Questions & Step-by-Step Solutions
If the solubility product (Ksp) of AgCl is 1.77 x 10^-10, what is the molar solubility of AgCl?
Step 1: Understand that Ksp (solubility product) is a constant that represents the solubility of a salt in water.
Step 2: Write the dissociation equation for AgCl: AgCl (s) ⇌ Ag+ (aq) + Cl- (aq).
Step 3: Recognize that when AgCl dissolves, it produces equal amounts of Ag+ and Cl- ions. If 's' is the molar solubility, then [Ag+] = s and [Cl-] = s.
Step 4: Write the expression for Ksp: Ksp = [Ag+][Cl-]. Since both concentrations are 's', we can write Ksp = s * s = s^2.
Step 5: Substitute the given Ksp value into the equation: 1.77 x 10^-10 = s^2.
Step 6: Solve for 's' by taking the square root of both sides: s = sqrt(1.77 x 10^-10).
Step 7: Calculate the square root: s = 1.77 x 10^-5 M.
Solubility Product (Ksp) – The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of ionic compounds in water, representing the product of the concentrations of the ions, each raised to the power of their coefficients in the balanced equation.
Molar Solubility – Molar solubility is the number of moles of solute that can dissolve in a liter of solution at equilibrium, often calculated from Ksp for sparingly soluble salts.
Square Root Calculation – Understanding how to manipulate equations to isolate variables, particularly the square root in the context of Ksp calculations.
