150 mL of 0.0008 M ammonium sulphate is mixed with 50 mL of 0.04 M calcium nitrate. The ionic product of `CaSO_(4)` will be : `(K_(sp)=2.4xx10^(-5) for CaSO_(4))`
50 mL of 0.2 M ammonia solution is treated with 25mL of 0.2 M HCl . If pK_(b) of ammonia solution is 4.75 , the pH of the mixture will be
50 ml of 0.2 M HCl is added to 30 ml of 0.1 MKOH solution. Find the pH of the solution.
When 100 ml of 0.4 M CH_3 COOH is mixed with 100 ml of 0.2 M NaOH , the [H_3O]^(+) in the solution is approximately : [K_a (CH_3COOH)= 1.8 xx 10 ^(-5) ]
60 mL of 0.3 M KOH and 40 mL of 0.2 M HCl are mixed. What is the pH of the mixture ?
if 500 mL of 0.4 M AgNO_3 is mixed with 500 mL of 2M NH_3 solution the what is the concentration of Ag (NH_3 ) ^(+) in solution? [Given : K_(f_1) [Ag (NH_3) ^(+)] =10 ^(3) , K _(f_2) [Ag (NH_3)_2^(+) ]= 10^(4) ]
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) .
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))
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
