Consider the dissociation of strong versus weak acids:
HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)HF(a q)+H2O(l)⇌H3O+(aq)+F−(aq)
The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, F−, can react with H3O+. Now consider the solubility of insoluble salts:
AgCl(s)⇌Ag+(aq)+Cl−(aq)AgF(s)⇌Ag+(a q)+F−(aq)
The addition of acid has no effect on silver chloride. But for the second reaction, H3O+ will react with F−, decreasing its concentration and driving the equilibrium to the right. Thus, salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases.
Part A
Identify the effect of increasing acidity on the solubility of the given compounds.
Drag the appropriate items to their respective bins.
Ca3(PO4)2
ZnS
BaCO3
AgI
Mg(OH)2
MgBr2
Answers: 2
Chemistry, 22.06.2019 04:00, lucasrandall
Asolution contains 225 g of sodium chloride, nacl, dissolved in enough water to make a 0.25 l of solution. what is the molarity of the solution?
Answers: 2
Consider the dissociation of strong versus weak acids:
HCl(aq)+H2O(l)→H3O+(aq)+Cl−(aq)HF(a q)+H2O(...
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