Go To Your Study Dashboard

Get Answers to all your Questions

header-bg

A buffer solution is prepared in which the concentration of $NH_3$ is $0.30M$ and the concentration of $NH_4^{+}$ is $0.20M$ . If the equilibrium constant, $K_b$ for $NH_3$ equals $1.8\times 10^{-5}$ , what is the pH of this solution? $(log2.7=0.433)$
Option: 1
$9.08$

Option: 2
$9.43$

Option: 3
$11.72$

Option: 4
$8.73$

Answers (1)

best_answer

$\left [ NH_{3} \right ]= 0.30 M, \ K_b = 1.8\times 10^{-5}$

$\left [ NH_{4}^{+} \right ]= 0.20 M$

From Henderson - Hasselbach equation

$p\left ( OH \right ) = pK_b +\log \frac{\left [ Salt \right ]}{\left [ Base \right ]} = 4.74+\log \frac{0.2}{0.3}$

$p\left ( OH \right ) = 4.56$

$\Rightarrow p\left ( H \right ) = 14 - p\left ( OH \right ) = 9.43$

The Correct answer is option 2.

Posted by

Deependra Verma

View full answer

NEET 2024 Most scoring concepts

Just Study 32% of the NEET syllabus and Score up to 100% marks

Similar Questions

Trending Articles/News

anam-khan

Fraudsters beware! For NEET UG 2025, NTA launches platform to report suspicious activity

anam-khan

NEET aspirant from Delhi found dead in Kota refused to sit for May 4 exam, wanted 1 more year

anam-khan

Bihar Police arrests 2024 NEET paper leak case mastermind from Patna

Latest Question