Home
Class 11
CHEMISTRY
a. Calculate the ratio of pH of a soluti...

a. Calculate the ratio of `pH` of a solution continaing `1mol`. Of `CH_(3)COONa +1 mol` of `HC1` per litre and of other solution containing `1mol` of `CH_(3)COONa + 1mol` of `CH_(3)COOH` per litre.
b. A `0.1M `solution of weak acid `HA` is `1%` dissociated at `298k`. what is its `K_(a)`? what will be the new degree of dissociation of `HA` and `pH` when `0.2M` of `NaA` is added to it.

Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the ratio of pH of a solution containing 1 mole CH_3COONa + 1 mole of HCI per litre and of the other solution containing 1 mole of CH_3COONa + 1 mole of CH_3COOH per litre

The ratio of the pH of solution (I) containing 1 mol of CH_(3)COONa and 1 mol of HCl in 1L, and solution (II) containing 1 mol of CH_(3)COONa and 1 mol of CH_(3)COOH in 1L is

The ratio of pH of solution (1) containing 1 mole of CH_(3)COONa and 1 mole of HCl and solution (II) containing 1 mole of CH_(3)COONa and 1 mole of acetic acid in one litre is :

The ratio of pH of solution (1) containing 1 mole of CH_(3)COONa and 1 mole of HCl and solution (II) containing 1 mole of CH_(3)COONa and 1 mole of acetic acid in one litre is :

A 0.1 M solution of weak acid HA is 1% dissociated at 25^@C. What is the Ka ? If this solution is with respect to NaA 0.2M, what will be new degree of dissociation of HA and pH?

The pH of a solution containing 0.1mol of CH_(3)COOH, 0.2 mol of CH_(3)COONa ,and 0.05 mol of NaOH in 1L. (pK_(a) of CH_(3)COOH = 4.74) is:

The pH of a solution containing 0.1mol of CH_(3)COOH, 0.2 mol of CH_(3)COONa ,and 0.05 mol of NaOH in 1L. (pK_(a) of CH_(3)COOH = 4.74) is: