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anonymous
 one year ago
Enough of a monoprotic acid is dissolved in water to produce a 0.0116 M solution. The pH of the resulting solution is 2.35. Calculate the Ka for the acid.
anonymous
 one year ago
Enough of a monoprotic acid is dissolved in water to produce a 0.0116 M solution. The pH of the resulting solution is 2.35. Calculate the Ka for the acid.

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RamiroCruzo
 one year ago
Best ResponseYou've already chosen the best response.1Convert pH 2.68 to (H^+) with pH = log(H^+). Then HA > H^+ + A^ Ka = (H^+)(A^)/(HA) Substitute for (H^+) and (A^). For (HA) substitute 0.0169(H^+)

Rushwr
 one year ago
Best ResponseYou've already chosen the best response.1monoprotic acid is an acid that can donate only one proton. So this acid is like HCl. \[HCl \rightarrow H ^{+} + Cl ^{}\] We know the concentration of HCl solution. \[K _{a} = \frac{ [H ^{+}][Cl ^{}] }{ [HCl] }\] \[[H ^{+}] = [Cl ^{}]\] We can find H^+ concentration using pH \[pH = \log_{10} [H ^{+}]\] HCl concentration is 0.0116M So \[K _{a}= \frac{ [H ^{+}]^{2} }{ [HCl] }\]
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