50 litre of a solution containing `10^(-5)" mole of "Ag^(+)` is mixed with 50 litre of a `2xx 10^(-7)` M HBr solution. `[Ag^+]` in resultant solution is: `["Given : "K_(sp)(AgBr)= 5xx 10^(-13)] `

50mL of a solution containing 10^(-3) mole of Ag^(+) is mixed with 50 mL of a 0.1M HCl solution. How much Ag^(+) remains in solution ? (K_(sp) of AgCl=1.0xx10^(-10))

50mL of a solution containing 10^(-3) mole of Ag^(+) is mixed with 50 mL of a 0.1M HCl solution. How much Ag^(+) remains in solution ? (K_(sp) of AgCl=1.0xx10^(-10))

50mL of a solution containing 10^(-3) mole of Ag^(+) is mixed with 50 mL of a 0.1M HCl solution. How much Ag^(+) remains in solution ? (K_(sp) of AgCl=1.0xx10^(-10))

50 ml of 0.05 M sodium hydroxide is mixed with 50 ml 0.1 of M acetic acid solution. What will be the pH resulting solution if K_(a) (CH_(3)COOH) = 2 xx 10^(-5)

50 ml of 0.05 M sodium hydroxide is mixed with 50 ml 0.1 of M acetic acid solution. What will be the pH resulting solution if K_(a) (CH_(3)COOH) = 2 xx 10^(-5)

A saturated solution of calcium fluoride contains 2xx10^(-4) mole of the salt per litre of the solution its K_sp is :

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) )

2.5 litre of 1M NaOH solution is mixed with another 3 litre solution of 0.5M NaOH solution. Then the molarity of the resulting solution is

A solution of Na_(2)CO_(3) is added drop by drop to 1 litre of a solution containing 10^(-4) mole of Ba^(2+) and 10^(-5) mole of Ag^(+) , if K_(sp) for BaCO_(3) is 8.1xx10^(-9) and K_(sp) for AgCO_(3) is 6.9xx10^(-12) then which is not true?

A solution containing 0.2 mole of dicholoracetice acid (K_(a)=5xx10^(-2)) and0.1 mole sodium dicholoroacetate in one litre solution has [H^(+)] :