PH of two equimolar weak acids are 3.0 and 5.0 respectively. Their relative strength is

English

Gujarati

Hindi

6-2.Equilibrium-II (Ionic Equilibrium)

medium

The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

A

$3:5$

B

$5:3$

C

$100:1$

D

$1:100$

Solution

The relative strength of acids $=$ ratio of hydrogen ion concentration

When $pH =3.0,\left[ H ^{+}\right]=10^{-3.0}\, M$

When $pH =5.0,\left[ H ^{+}\right]=10^{-5.0}\, M$

The ratio of hydrogen ion concentration $=\frac{10^{-3.0} \,M }{10^{-5.0} \,M }=100: 1$

The relative strength of acids is $100: 1$

Standard 11

Chemistry

Share

Similar Questions

At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be

medium

What is the $pH$ of solution of $7$ $gm$ $N{H_4}OH$ per $500$ $mL$ ? ( ${K_b}$ of $N{H_4}OH 1.8 \times {10^{ – 5}}$, Molecular moles of $N{H_4}OH$ is $35\,g\,mo{l^{ – 1}}$ )

medium

A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ – }$ would be

medium

A weak acid is $ 0.1\% $ ionised in $0.1\, M $ solution. Its $pH$ is

medium

In aqueous solution the ionization constants for carbonic acid are

$K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$

Select the correct statement for a saturated $0.034\, M$ solution of the carbonic acid.

normal

(AIEEE-2010)