will AgIO3 precipitate when 100 mL of 0.010 M AgIO3 is mixed with 10 mL of 0.0015 M NaIo3
Look up Ksp for AgIO3 and see if Kion product exceeds Ksp.
To determine whether AgIO3 will precipitate when the two solutions are mixed, we need to compare the solubility product constant (Ksp) of AgIO3 with the reaction quotient (Q) for the given concentrations.
The balanced equation for the dissociation of AgIO3 is:
AgIO3 (s) ⇌ Ag+ (aq) + IO3- (aq)
The Ksp expression for AgIO3 is:
Ksp = [Ag+][IO3-]
Given that the concentration of AgIO3 is 0.010 M in 100 mL, we can calculate the concentration of Ag+ and IO3- ions using stoichiometry:
AgIO3 (s) ⇌ Ag+ (aq) + IO3- (aq)
0.010 M x x
Since AgIO3 dissociates in a 1:1 ratio, the concentration of Ag+ and IO3- will also be 0.010 M.
Now, let's calculate the concentration of Ag+ and IO3- ions when 10 mL of 0.0015 M NaIO3 is added:
NaIO3 (s) ⇌ Na+ (aq) + IO3- (aq)
0.0015 M x x
Since NaIO3 dissociates in a 1:1 ratio, the concentration of IO3- ions will be 0.0015 M. However, Na+ ions are spectator ions in this case and do not participate in the precipitation of AgIO3.
Therefore, the concentration of IO3- ions in the final solution will be 0.010 M + 0.0015 M = 0.0115 M.
Now, we can compare the reaction quotient (Q) with the solubility product constant (Ksp) to determine if a precipitate will form:
Q = [Ag+][IO3-] = (0.010 M)(0.0115 M) = 0.000115
If Q > Ksp, a precipitate will form. If Q < Ksp, no precipitate will form.
Unfortunately, the solubility product constant (Ksp) for AgIO3 was not provided, so we cannot determine if a precipitate will form without that information.