Precipitation of Ag+ with KOHa) Using the Ksp values provided in Table 2, predict whether it would form using 3 M KOH and 0.10 M of the metal nitrate solution.b) Using calculated Qsp values, now predict whether a precipitate would form after adding an additional 2 mL (excess) of 3 M KOH to each cation solution. CationEquilibrium EquationKspAg*AgClo) 5 Ag*(ад)+ CI(aq)1.8 x 10-10Ag,CrO4(9) 52 Ag*(aq) + CrO,²-(aq)-121.9 x 10+ OH (ag)+AgOH() S Ag*(aq)2.8 x 10-8Hg*HgClo) S Hg(aq) + Cl (ag)2.0 x 10-18Hg.CrO4() 5 2 Hg*(aq) + CrO4 (aq)2.0 x 10-9Pb2+PBC126) S Pb² (aq) + 2 Cl (aq)2+1.6 x 10-5PbCrO4(6) 5 Pb?* (aq) + CrO4 (ag)-141.7 × 10-Pb(OH)2(s)S Pb2* (aq) + 2 OH (ag)2.8 x 10-16IonEquilibrium EquationKwH* or OH-H2O) 2 H*(ag) + OH (ag)1.0 x 10-14

Dissociation equilibrium of AgOH: AgOH(s)⇔Ag+(aq)+OH-(aq)

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Precipitation of Ag⁺ with KOH

a) Using the Ksp values provided in Table 2, predict whether it would form using 3 M KOH and 0.10 M of the metal nitrate solution.

b) Using calculated Qsp values, now predict whether a precipitate would form after adding an additional 2 mL (excess) of 3 M KOH to each cation solution.

Cation
Equilibrium Equation
Ksp
Ag*
AgClo) 5 Ag*
(ад)
+ CI
(aq)
1.8 x 10-10
Ag,CrO4(9) 52 Ag*(aq) + CrO,²-(aq)
-12
1.9 x 10
+ OH (ag)
+
AgOH() S Ag*(aq)
2.8 x 10-8
Hg*
HgClo) S Hg(aq) + Cl (ag)
2.0 x 10-18
Hg.CrO4() 5 2 Hg*(aq) + CrO4 (aq)
2.0 x 10-9
Pb2+
PBC126) S Pb² (aq) + 2 Cl (aq)
2+
1.6 x 10-5
PbCrO4(6) 5 Pb?* (aq) + CrO4 (ag)
-14
1.7 × 10-
Pb(OH)2(s)
S Pb2* (aq) + 2 OH (ag)
2.8 x 10-16
Ion
Equilibrium Equation
Kw
H* or OH-
H2O) 2 H*(ag) + OH (ag)
1.0 x 10-14

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