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Bronsted Lowry Theory

A buffer is a...

Question

A buffer is a solution of weak acid and its conjugate base or a weak base and its conjugate acid. It resists the change in $p H$ , when small amount of strong acid or base is added to it. Buffer solutions have wide applications.
$H C l$ gas is passed through an aqueous solution of 0.1M 1-aminopropane $(P r N H_{2})$ till the $p H$ reaches 9.71. Calculate the ratio of $[P r N H_{2}] / [P r N H_{3}^{+}]$ in this solution.
$[K_{a} (P r N H_{3}^{+}) = 1.96 \times 10^{- 11}$

0.1

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Solution

The correct option is A 0.1
$p H = p K_{a} + l o g S a l t / a c i d$

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Similar questions

H C l

(P r N H_{2})

[P r N H_{2}] / [P r N H_{3}^{+}]

[K_{a} (P r N H_{3}^{+}) = 1.96 \times 10^{- 11}]

l o g (1.96) = 0.292, l o g (0.1) = - 1

p H

20.0 m L

0.10 M

0.10 M

H C l

p H

p ≃ 6

H C l

0.1 M

1 - a m i n o r p o p a n e

(P r N H_{2})

p H

9.71

[P r N H_{2}] / [P r N H_{3}]^{+}

Given: K_{a} (P r N H_{3}^{+}) = 1.96 \times 10^{- 11} log (- 9.71) = 1.95 \times 10^{- 10}

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