The pH of a 0.05 M ammonia solution is 10.97. Find the ionisation constant the conjugate acid of ammonia, N H4+. Given, p Kw=14.0 Kb for ammonia, =1.77 × 10-5

Question

The pH of a 0.05 M ammonia solution is 10.97. Find the ionisation constant the conjugate acid of ammonia, N H4+. Given, p Kw=14.0 Kb for ammonia, =1.77 × 10-5 (A)  4.77× 10-5  (B)  9.77× 10-5  (C)  4.99× 10-10  (D)  5.64× 10-10

Tardigrade Admin · Accepted Answer

Ka=(Kw/Kb) =(10-14/1.77 × 10-5) =5.64 × 10-10

Q. The $p H$ of a $0.05 M$ ammonia solution is $10.97$ . Find the ionisation constant the conjugate acid of ammonia, $N H_{4}^{+}$ . Given, $p K_{w} = 14.0 K_{b}$ for ammonia, $= 1.77 \times 1 0^{- 5}$

$4.77 \times 1 0^{- 5}$

$9.77 \times 1 0^{- 5}$

$4.99 \times 1 0^{- 10}$

$5.64 \times 1 0^{- 10}$

$K_{a} = \frac{K _{w}}{K _{b}}$
$= \frac{1 0 ^{- 14}}{1.77 \times 1 0 ^{- 5}}$
$= 5.64 \times 1 0^{- 10}$

Q. The pH of a 0.05M ammonia solution is 10.97. Find the ionisation constant the conjugate acid of ammonia, NH4+​. Given, pKw​=14.0Kb​ for ammonia, =1.77×10−5

4.77×10−5

9.77×10−5

4.99×10−10

5.64×10−10