`25 mL` of `0.4 M` of a weak base and `75 mL` of `0.2` M of its salt forms a buffer solution. The dissocation constant of base is `2 xx 10^(-5)` the `(log 1.5 = 0.176)`

A weak base BOH is 2.22 percent dissociated in its 0.1 M solution. Calculate the dissociation constant of the base.

A buffer solution is prepared by mixing 50 mL of 0.2 M of acetic acid with .x. mL of 0.2 M of NaOH solutions. If pH of the resulting buffer solutions is 4. 7 then value of .x. is (Ka= 2xx10 ^(-5))

A solution containing 75 mL of 0.2M HCI and 25 mL of 0.2M NaOH. Calculate the pH of solution.

To 50 mL of 0.5 M H_(2)SO_4 75 mL of 0.25 M H_2SO_4 is added. What is the concentration of the final solution if its volume is 125 mL?

If 50 ml of 0.2M KOH is added to 40 ml of 0.5 M HCOOH. the pH of the resulting solutions is (Ka = 1.8 xx 10^(-4) log 18= 1.26)

50 ml of 0.2 M NH_(4)OH and 50 ml of 0.2 M HCl solutions are Mixed. pH of the resulting solution is (Given Kb of NH_(4)OH=1 times 10^(-5) )

The pH of a buffer containing equal molar concentration of a weak base and its chloride (K_(b) weak base =2 xx 10^(-5) , log 2 =0.3 ) is