Question

Will a precipitate form if 175 ml of 0.0055 M KCl is mixed with 145 ml of 0.0015 M AgNO3? Kₛₚ for AgCl is 1.77x10⁻¹⁰

a) Yes, a precipitate will form
b) No, a precipitate will not form
c) The formation of a precipitate depends on temperature
d) Insufficient information to determine

Answer 1

When KCl is mixed with AgNO3, no precipitate will form.

Step-by-step explanation:

When KCl is mixed with AgNO3, it forms KNO3 and AgCl. To determine if a precipitate will form, we need to compare the reaction quotient, Q, to the solubility product constant, Ksp, for AgCl. The equation for Q is Q = [K+][Cl-]. Given the concentrations of KCl and AgNO3, we can calculate the concentrations of K+ and Cl- ions in the mixture and compare Q to Ksp. If Q is greater than Ksp, a precipitate will form.

In this case, we have 175 ml of 0.0055 M KCl and 145 ml of 0.0015 M AgNO3. To calculate the concentrations of K+ and Cl- ions, we need to convert the volumes to liters and use the formula C = n/V, where C is the concentration, n is the number of moles, and V is the volume in liters. Plugging in the values, we get [K+] = (0.0055 mol/0.175 L) = 0.0314 M and [Cl-] = (0.0015 mol/0.145 L) = 0.0103 M.

Now we can calculate Q = (0.0314)(0.0103) = 0.000322, which is less than Ksp for AgCl (1.77 × 10^-10). Since Q is less than Ksp, no precipitate will form.