Question
Find the pH of a 0.010M solution of NH4ClO4 and the pH of a 0.010M solution of NH4C2H3O2.
Answers
after finding the ph of the corresponding ions in these two questions, would you add the two ph's together to determine the final ph of the solution?
I assume these are two separate solutions; i.e., two separate problems.
The pH of the NH4ClO4 solution is determined by the hydrolysis of the salt. NH4ClO4 is the salt of a weak base (NH3) and a strong acid (HClO4), therefore, the NH4^+ is hydrolyzed.
NH4^+ + HOH ==> NH3 + H3O^+
Make an ICE table.
Plug in the numbers and calculate H3O^+ and pH from that.
For NH4C2H3O2, both NH4^+ and C2H3O2^- are hydrolyzed since that is the salt of a weak acid (HC2H3O2) and a weak base (NH3). The formula for the pH of such a solution is
(H^+) = sqrt(Kw/KaKb)
The pH of the NH4ClO4 solution is determined by the hydrolysis of the salt. NH4ClO4 is the salt of a weak base (NH3) and a strong acid (HClO4), therefore, the NH4^+ is hydrolyzed.
NH4^+ + HOH ==> NH3 + H3O^+
Make an ICE table.
Plug in the numbers and calculate H3O^+ and pH from that.
For NH4C2H3O2, both NH4^+ and C2H3O2^- are hydrolyzed since that is the salt of a weak acid (HC2H3O2) and a weak base (NH3). The formula for the pH of such a solution is
(H^+) = sqrt(Kw/KaKb)
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