Home
Class 11
CHEMISTRY
Approximate pH of 0.01 M NaHA is calcula...

Approximate pH of 0.01 M NaHA is calculated by :
`(K_(a1)=10^(-6)` and `K_(a2)=10^(-8)` are ionization constants of `H_(2)A)`

A

`pH=7+(pK_(a1))/2+(logC)/2`

B

`pH=7-(pK_(a1))/2-(logC)/2`

C

`pH=(pK_(a1)+pK_(a2))/2`

D

None of these

Text Solution

Verified by Experts

Promotional Banner

Topper's Solved these Questions

  • IONIC EEQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level- 1|1 Videos

  • IONIC EEQUILIBRIUM

    NARENDRA AWASTHI|Exercise Level- 2|11 Videos

  • GASEOUS STATE

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|1 Videos

  • SOLID STATE

    NARENDRA AWASTHI|Exercise Level 3 - Subjective Problems|1 Videos

Similar Questions

Explore conceptually related problems

The pH of 0.05 M acetic acid is (K_(a) = 2 xx 10^(-5))

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)

K_(a) of 0.02M CH^(3)COOH is 1.8xx10^(-5) Calculate a. [H_(3)O^(+)] b. % ionization c. pH

The ionization constants of HF, H COOH and HCN at 298 K are 6.8x10^(-4), 1.8xx10^(-4) and 4.7xx10^(-9) respectively. Calculate the ionization constants of the corresponding conjugate base.

An aqueous solution of metal bromide MBr_2 (0.05 M) is saturated with H_2 S . For saturated H_2 S of 0.1 M, K_1 = 10^(-7) and K_2 = 1.3 xx 10^(-13) . What is the minimum pH at which MS will precipitate? K_(sp) . for M S is 6 xx 10^(-21)

What is the minimum pH required to prevent the precipitation of Zn^(+2) in a solution that is 0.01 M ZnCl_(2) and saturated with 0.1 M H_(2) S (Given : K_(sp) ZnS = 10^(-21) and Ka_(1) xx Ka_(2) of H_(2)S = 10^(-20) )