Calculate the `pH` of `0.005M` `Ba(OH)_(2)` in aq. solution.

The P^(H) of 0.005 M Ba (OH)_(2) is

Calculate the pH of 0.10M ammonia solution. Calcualte the pH after 50.0mL of this solution is treated with 25.0mL of 0.10M HCl . The dissociation constant of ammonia, K_(b)=1.77xx10^(-5) .

Calculate the pH of 0.001 M aqueous solution of ZnCl_2, K_a for the equilibrium, Zn^(2+) +H_(2) O hArr Zn (OH)^(+) +H^(+) is 1 xx 10^(-9)

20 gm of sample Ba(OH)_(2) is dissolved in 10 ml of 0.5 N HCl solution, The excess of HCl was titrated with 0.2 NaOH. The volume of NaOh used was 10 mol. Calculate the % of Ba(OH)_(2) in the sample.

Calculate the pH for a. 0.001 M NaOH b. 0.01 M Ca(OH)_(2) c. 0.0008M Ba(OH)_(2) d. 0.004 M NaOH