By Sunil Bhardwaj

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Calculate the degree of ionization and the hydrogen ion concentration of a $${ 10 }^{ -3 }M$$ acetic acid solution at 298 K $$({ K }_{ a } = 1.85 \times { 10 }^{ -5 })$$.

Ionization reaction for acetic acid is $$\underset { C\left( 1-\alpha \right) }{ C{ H }_{ 3 }COOH } \rightleftharpoons \underset { C\alpha }{ C{ H }_{ 3 }CO{ O }^{ - } } + \underset { C\alpha }{ { H }^{ + } }$$ $$C = { 10 }^{ -3 }M { K }_{ a } = 1.85 \times { 10 }^{ -5 }$$ from the formula, $$\alpha = \sqrt { \frac { { K }_{ a } }{ C } }$$ $$= \sqrt { \frac { 1.85 \times { 10 }^{ -5 } }{ { 10 }^{ -3 } } }$$ $$= \sqrt { 0.0185 } = 0.136$$ Hydrogen ion concentration can be given as, $$\left[ { H }^{ + } \right] = C{ \alpha } = 0.136 \times { 10 }^{ -3 } M$$

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