`25.0`mL of `0.050 M Ba(NO_3)_2` is mixed with `25.0` mL of `0.020 MNaF. K_sp` of `BaF_2` is `0.5times 10^(-6)` at `298 K` . The ratio of `[Ba^(2+)][F^(-2)` and `K_(sp)` is ____.(Nearest interger)

If 25.0 cm^(3) of 0.05 M Ba(NO_(3))_(2) solution is mixed with 25.0 cm^(3) of 0.02 M NaF solution. Will any BaF_(2) precipitated ? (K_(sp) " for " BaF_(2) =1.7 xx 10^(-6))

100ml of 0.75 N NH_(4)OH is mixed with 100ml of 0.25 N HCl. The K_(b) of NH_(4) OH = 2 xx 10^(-5) . Hence pH of solution is .

250 ml of 0.10 M K_2 SO_4 solution is mixed with 250 ml of 0.20 M KCI solution. The concentration of K^(+) ions in the resulting solution will be:

When 15mL of 0.05M AgNO_(3) is mixed with 45.0mL of 0.03M K_(2)CrO_(4) , predict whether precipitation of Ag_(2)CrO_(4) occurs or not? K_(sp) of Ag_(2)CrO_(4) = 1.9 xx 10^(-12)

50.0 mL of 0.10 M ammonia solution is treated with 25.0 mL of 0.10M HCI . If K_(b)(NH_(3))=1.77xx10^(-5) , the pH of the resulting solution will be

500 ml of 0.2( M ) H_(2) SO_(4) are mixed with 250 ml of 0.1 ( M ) Ba( OH)_(2) , the normality of resulting solution is -

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))

10mL of 0.3M Na_(2)SO_(4) are mixed with 20mL solution having initially 0.1M Ca^(2+) and 0.1M Sr^(2+) in it. Calculate the final [Ca^(2+)], [Sr^(2+)] and [SO_(4)^(2-)] in solution? Given K_(sp) SrSO_(4) = 7.6 xx 10^(-7) and K_(sp) CaSO_(4) = 2.4 xx 10^(-5) .

100 ml of 0.2"M H"_(2)SO_(4) solution is mixed with 400ml of 0.05"M Ba"_(3)(PO_(4))_(2) . Calculate the concentration of [Ba^(+2)] ion in resulting solution.