the pH of 0.1M NH_4Cl solution is (given pK_b=4.74)

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To 1L solution containing 0.1 mol each of $N H_{3}$ and $N H_{4} C l, 0.05$ mol of NaOH is added. The change in pH will be $(p K_{b} f o r N H_{3} = 4.74)$

Q. Solution of 0.1 N

N H_{4} O H

and 0.1 N

N H_{4} C l

has pH 9.25.

p K_{b}

N H_{4} O H

is :

Q. One litre of a buffer solution contains 0.01M

N H_{4} C l

and 0.1 M

N H_{4} O H

. The

p^{k b}

of base is 5.

p^{H}

value of the solution is:

p K_{b}

N H_{3}

is 4.74. The

p H

when 100 mL of 0.01 M

N H_{3}

solution is 50% neutralised by 0.01 M HCl is,

p K_{b}

N H_{4} O H

4.74

. If the ratio of the buffer mixture

[N H_{4} C l] : [N H_{4} O H]

1 : 10

, then the

p H

of that buffer is:

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