Acetic acid is a weak acid that ionizes in solution as follows: CH3COOH(aq) ⇌ CH3COO-(aq) + H+(aq) If the freezing point of a 0.106 M CH3COOH solution is -0.250°C, calculate the percent of the acid that has undergone ionization.
Added by Kevin M.
Step 1
First, we need to calculate the freezing point depression. The freezing point of pure water is 0°C, so the depression is 0 - (-0.250) = 0.250°C. Show more…
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Acetic acid is a weak acid that ionizes in solution as follows: CH3COOH(aq) Δ CH3COO2(aq) 1 H1(aq) If the freezing point of a 0.106 m CH3COOH solution is 20.203°C, calculate the percent of the acid that has undergone ionization.
David C.
Acetic acid is a weak acid that ionizes in solution as follows: $$\mathrm{CH}_{3} \mathrm{COOH}(a q) \rightleftharpoons \mathrm{CH}_{3} \mathrm{COO}^{-}(a q)+\mathrm{H}^{+}(a q)$$ If the freezing point of a $0.106 \mathrm{m} \mathrm{CH}_{3} \mathrm{COOH}$ solution is $-0.203^{\circ} \mathrm{C},$ calculate the percent of the acid that has undergone ionization.
A $0.109 \mathrm{~mol} / \mathrm{kg}$ aqueous solution of formic acid, HCOOH, freezes at $-0.210^{\circ} \mathrm{C}$. Calculate the percent dissociation of formic acid.
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