100 ml of 0.3N acetic acid solution is mixed with same volume of 0.2N sodium hydroxide solution. Ionisation constant of acetic acid is $2 \times 10^{- 5}$ . The pH of the mixture is :

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Solution

The correct option is C 5
The reaction will follow as:
$C H_{3} C O O H + N a O H \to C H_{3} C O O N a + H_{2} O$
$100 \times 0.3$ $100 \times 0.2$ initially
$100 \times 0.1$ $100 \times 0.2$ at equilibrium

$⟹ p H = p K_{a} + l o g \frac{[s o d i u m a c e t a t e]}{[a c e t i c a c i d]}$
$⟹ p H = 5 - l o g (2) + l o g \frac{20}{10}$

$⟹ p H = 4.99 = 5$

Option C is correct.

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Solutions of sodium hydroxide and acetic acid are mixed by the reaction: $N a O H + C H_{3} C O O H ⟶ C H_{3} C O O N a + H_{2} O$

Acetic acid is a weak acid. If equal volumes of equal molar solutions are mixed, the pH of the solution will be:

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