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Industrial Preparation of Ammonia

final pH of t...

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final pH of the solution obtained on mixing 100 ml 0.01 M HCl and 100 ml 0.01 M CH3COOH (Ka= 10^-5) is [log 5=0.7]

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100

0.01

C H_{3} C O O H

40

0.01

N a O H

(K_{a} = 10^{- 5})

p H

1

0.01

H C l

Q. Calculate the pH of the solution obtained by mixing

200

0.1

C H_{3} C O O H

50

0.2

C a (O H)_{2}

K_{a} = 10^{- 5}

100

0.01

C H_{3} C O O H

200

0.02

C H_{3} C O O N a

are mixed to form a buffer solution.

700

mL of water is added to this solution. The pH before and after dilution are:
(pKa = 4.74, log 4 =0.6)

Q. The following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations
1. 60 mL

\frac{M}{10}

\frac{M}{10}

\frac{M}{10}

\frac{M}{10}

\frac{M}{5}

\frac{M}{5}

NaOH

4. 100 mL

\frac{M}{10}

\frac{M}{10}

NaOH

pH of which one of them will be equal to 1?

100 m l

M / 10 N a O H

50 m l

M / 5 H C l

solution mixed, then

p H

of resulting solution would be:

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