The Ka of C6H5OH is 1-0-10-10-What is the pH of a 0-10 M C6H5O- solution-

The correct option is C 11.50 K_b=K_wK_a=1 × 10^ 141.0 × 10^ 10=1.0 × 10^ 4 For a base phenoxide ion, the expression for the pOH of the solution is gi ...

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Standard XII

Chemistry

Salt of Strong Acid and Weak Base

The Ka of ...

Question

The $K_{a}$ of $C_{6} H_{5} O H$ is $1.0 \times 10^{- 10}$ .What is the $p H$ of a $0.10 M C_{6} H_{5} O^{-}$ solution?

10.51

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11.04

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11.50

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12

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Solution

The correct option is C $11.50$
$K_{b} = \frac{K_{w}}{K_{a}} = \frac{1 \times 10^{- 14}}{1.0 \times 10^{- 10}} = 1.0 \times 10^{- 4}$

For a base phenoxide ion, the expression for the pOH of the solution is given by the expression $p O H = - l o g \sqrt{K_{b} C}$

Substitute values in the above expression:

$p O H = - l o g \sqrt{(1.0 \times 10^{- 4} \times 0.10)} = 2.5$

$p H = 14 - p O H = 14 - 2.5 = 11.50$

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The Ka of C6H5OH is 1.0×10−10.What is the pH of a 0.10 M C6H5O− solution?

The correct option is C 11.50Kb=KwKa=1×10−141.0×10−10=1.0×10−4For a base phenoxide ion, the expression for the pOH of the solution is given by the expression pOH=−log√KbCSubstitute values in the above expression:pOH=−log√(1.0×10−4×0.10)=2.5pH=14−pOH=14−2.5=11.50

The $K_{a}$ of $C_{6} H_{5} O H$ is $1.0 \times 10^{- 10}$ .What is the $p H$ of a $0.10 M C_{6} H_{5} O^{-}$ solution?