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A buffer solution is prepared in which the concentration of {N

Question

A buffer solution is prepared in which the concentration of $N H_{3}$ is $0.30 M$ and the concentration of $N H_{4}^{+}$ is $0.20 M$ . If the equilibrium constant, $K_{b}$ for $N H_{3}$ equals $1.8 \times 10^{- 5}$ , what is the $p H$ of this solution? ( $lo g 2.7 = 0.43$ )

9.43

11.72

8.73

9.08

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Elijah Discussed

A buffer solution is prepared in which the concentration of

N H_{3}

0.30 M

and the concentration of

N H_{4}^{+}

0.20 M

. If the equilibrium constant,

K_{b}

for

N H_{3}

equals

1.8 \times 10^{- 5}

, what is the

p H

of this solution? (

lo g 2.7 = 0.43

)

12 mins ago

Discuss this question LIVE

12 mins ago

Text solutionVerified

p O H = p K_{b} + lo g . \frac{[ salt ]}{[ base ]}

= - lo g 1.8 \times 10^{- 5} + lo g . \frac{0.2}{0.30}

= 5 - 0.25 + (- 0.176)

= 4.75 - 0.176 = 4.57

∴ p H = 14 - 4.57 = 9.43

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Question Text	A buffer solution is prepared in which the concentration of $N H_{3}$ is $0.30 M$ and the concentration of $N H_{4}^{+}$ is $0.20 M$ . If the equilibrium constant, $K_{b}$ for $N H_{3}$ equals $1.8 \times 10^{- 5}$ , what is the $p H$ of this solution? ( $lo g 2.7 = 0.43$ )
Answer Type	Text solution:1
Upvotes	150