25.2.5ml of 2/5M weak monoacidic base (kb=10 to the power -12 at 25 degree Celsius) is titrated with 2/15M Hcl in water at 25 degree Celsius. Find the concentration of H plus ions at equivalence point. (kw=10 to the power -14 at 25 degree Celsius)

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Q. 2.5 mL of

\frac{2}{5} M

weak monoacidic base

(K_{b} = 1 \times 10^{- 12} a t 25^{\circ} C)

is titrated with

\frac{2}{15} M H C l

in water at

25^{\circ} C

. The

p H

at equivalence point is

(K_{w} = 1 \times 10^{- 14} a t 25^{\circ} C)

2.5 m L

\frac{2}{5} M

weak monoacidic base

(K_{b} = 1 \times 10^{- 12}

25^{\circ} C)

is titrated with

\frac{2}{15} M H C l

in water at

25^{\circ} C

. The concentration of

H^{+}

at equivalence point is:
[Note : use

K_{w} = 1 \times 10^{- 14}

25^{\circ} C

2.5 mL of $\frac{2}{5} M$ weak monoacidic base ( $K_{b} = 1 \times 10^{- 12}$ ) at $25^{o} C$ is titrated with $\frac{2}{15} M$ HCl in water at $25^{o} C .$ The concentration of $H^{+}$ at equivalence point is $(K_{w} = 1 \times 10^{- 14} a t 25^{o} C)$