`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 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)]

What will be present in th solution when 50 of ml 0.1 M HCl is mixed with 50 ml of 0.1 M NaOH soltion?

What will be present in th solution when 50 of ml 0.1 M HCl is mixed with 50 ml of 0.1 M NaOH soltion?

A 50mL10^(-3) MHCl solutions is mixed with 50mL8xx10^(-4)M NaOH solution. What would be the pH of resulting solution?

Calculate the pH of a solution obtained by mixing 50ml of 0.2 M HCl with 49.9 mL of 0.2 m NaOH solution.

40 ml of 0.1 M CaCl_2 solution is mixed with 50 ml of 0.2 M AgNO_3 solution. Mole of AgCl formed in the reaction is

40 ml of 0.1 M CaCl_2 solution is mixed with 50 ml of 0.2 M AgNO_3 solution. Mole of AgCl formed in the reaction is

The PH of a solution obtained by mixing 50 ml of 0.4 M HCl and 50 ml of 0.2 M NaoH IS :