A `0.1molar` solution of weak base `BOH` is `1%` dissociated. If `0.2mol` of `BCI` is added in `1L` solution of `BOH`. The degree of dissociation of `BOH` will become

A 0.1molar solution of weak base BOH is 1% dissociated. If 0.2mol of BCl is added in 1L solution of BOH . The degree of dissociation of BOH will become

1.0 M solution of a weak base , BOH is only 0.5 % ionized . If 2 mL 1 M solution of BOH is mixed with 30 mL water , the degree of dissociation of the base in the resulting solution and H^(+) ion concentration of the solution will bee respectively

1.0 M solution of a weak base , BOH is only 0.5 % ionized . If 2 mL 1 M solution of BOH is mixed with 30 mL water , the degree of dissociation of the base in the resulting solution and H^(+) ion concentration of the solution will bee respectively

A 0.1 M solution of weak acid HA is 1% dissociated at 25^(@) C To this solution NaA is added till [NaA] = 0.2 M, if the new degree of dissociation of HA = yxx 10^(-5) then what is 'y'?

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?

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.

A 0.1 M solution of a weak acid HA is 1% dissociated. The approximate value of dissociation constant is :

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.

Calculate the OH^(-) ion concentration of 0.005 M solution of a weak base BOH if the degree of dissociation is 0.02.