A solution containing AgNO3 is mixed with a solution of NaCl to form a solution that is 0.10 M in AgNO3 and 0.075 M in NaCl. What will happen once these solutions are mixed? Ksp (AgCl) = 1.77 × 10-10.

Since Q > Ksp, a precipitate of AgCl will form.

Explanation:

Step 1: Data given

Molarity AgNO3 = 0.10 M

Molarity of NaCl = 0.075 M

Ksp AgCl = 1.77 * 10^-10

Step 2: The balanced equation

AgNO3 + NaCl → AgCl(s) + NaNO3(aq)

For 0.10 moles AgNO3 we have 0.10 moles Ag+ ( molarity = 0.10 M)

For 0.075 moles NaCl we have 0.075 moles Cl- (molarity = 0.075 M)

Step 3: Calculate Q

Q = [Ag+][Cl-]

Q = (0.10 M )(0.075 M ) = 0.0075

Ksp = 1.77 * 10^-10

Q >>> Ksp

Since Q > Ksp, a precipitate of AgCl will form.

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