Home
Class 11
CHEMISTRY
What will be the pH of an aqueous soluti...

What will be the pH of an aqueous solution of 1.0 M ammonium formate?
Given :`pK_(a)=3.8 and pK_(b)=4.8`

A

`7.5`

B

`3.4`

C

`6.5`

D

`10.2`

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 a 0.001 M aqueous solution of sodium hydroxide will be

The pH and pOH of 0.1 M aqueous solution of HNO_3 , are

What is the K_(w) value in the aqueous solution of pK_(w)=13.725 ?

Calculate the pH of one molar ammonium formate solution. Given that pK_a for HCOOH = 3.8, PK_b for NH_3 = 4.8.

Calculate pH of a 1.0xx10^(-8) M solution of HCl.

The pH of 1.2 % (w/v) aqueous solution of CH_(3) COOH at 25^(@) C is (pK_(a) = 4.7)

The pH of 0.004M hydrazine solution is 9.7 . Calculate its ionization constant K_(b) and pK_(b) .