Calculate the ration of pH of a solution containing 1 mole of ${C H}_{2} C O O N a$ + 1 mole of HCI per litre and of other solution containing 1 mole of ${C H}_{2} C O O N a$ + 1 mole of acetic acid per litre.

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Solution

$\begin{matrix} C H_{3} C O O N a + H C l ⟶ & {C H}_{3} C O O H + & N a C l \begin{matrix} m o l e s b e f o r e r x n 1 m o l e s a f t e r r x n 0 \end{matrix} \begin{matrix} 10 \end{matrix} & \begin{matrix} 01 \end{matrix} & \begin{matrix} 01 \end{matrix} \end{matrix} [C H_{3} C O O H] = \frac{1}{1} = 1 m o l e [H^{+}] = c α = c \sqrt{\frac{K_{a}}{c}} = \sqrt{K_{a} c} = \sqrt{K_{a}} c = 1 p H_{1} = \frac{1}{2} l o g K_{a} f o r C H_{3} C O O N a + C H_{3} C O O H \begin{matrix} 1 m o l e + & 1 m o l e \end{matrix} p H_{2} = - log K_{a} + log \frac{1}{1} = - log K_{a} H e n c e t h e r a t i o w i l l b e p H_{1} + p H_{2} = 1 : 2$

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