Calculate the pH of a solution obtained by mixing equal volume of 10-10 M HOCl and 2 - 10-9 M CH 3 COOH solutions-Given-K a HOCl -2 - 10-4 K a CH 3 COOH -2 - 10-5 and log 2-0-3 A- 7B- 6-98C- 6-7D- 10

The correct option is C 6.7Considering it to be a mixture of two weak acids, we have nbsp; [H^+]_Total = √(K_a_1C_1+K_a_2C_2) = √(10^ 14 + 2× nbsp;10^ 14) ...

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Standard XII

Chemistry

Ostwald Dilution Law

Calculate the...

Question

Calculate the $p H$ of a solution obtained by mixing equal volume of $10^{- 10} M H O C l$ and $2 \times 10^{- 9} M C H_{3} C O O H$ solutions.(Given: $K_{a} H O C l = 2 \times 10^{- 4}$ $K_{a} C H_{3} C O O H = 2 \times 10^{- 5} a n d l o g 2 = 0.3$ )

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6.98

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6.7

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Solution

The correct option is C 6.7
Considering it to be a mixture of two weak acids, we have
$[H^{+}]_{T o t a l} = \sqrt{K_{a_{1}} C_{1} + K_{a_{2}} C_{2}}$
$= \sqrt{10^{- 14} + 2 \times 10^{- 14}}$
Now, we can observe that $[H^{+}]$ is very close to $10^{- 7}$ so $[H^{+}]$ from water will also be considered. in this case the formula for the total $[H^{+}]$ will be
$[H^{+}]_{T o t a l} = \sqrt{K_{a_{1}} C_{1} + K_{a_{2}} C_{2} + K_{w}}$
So,
$[H^{+}]_{T o t a l} = \sqrt{10^{- 14} + 2 \times 10^{- 14} + 10^{- 14}}$
$∴ [H^{+}]_{T o t a l} = 2 \times 10^{- 7}$
$p H = 7 - l o g 2 = 6.7$

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Calculate the pH of a solution obtained by mixing equal volume of 10−10 M HOCl and 2×10−9 M CH3COOH solutions.(Given: Ka HOCl=2×10−4 Ka CH3COOH=2×10−5 and log2=0.3)

Calculate the $p H$ of a solution obtained by mixing equal volume of $10^{- 10} M H O C l$ and $2 \times 10^{- 9} M C H_{3} C O O H$ solutions.(Given: $K_{a} H O C l = 2 \times 10^{- 4}$ $K_{a} C H_{3} C O O H = 2 \times 10^{- 5} a n d l o g 2 = 0.3$ )