A solution containing a mixture of 0.05M NaCl and 0.05M NaI is taken `(K_(sp)` of `AgCl=10^(-10)` and `K_(sp)` of `AgI=4xx410^(-18))` . When `AgNO_(3)` is added to such a solution:

A solution containing a mixture of 0.05M NaCI and 0.05M Nal is taken. (K_(sp) of AgCI = 10^(-10) and K_(sp) of AgI = 4 xx 10^(-16)) . When AgNO_(3) is added to such a solution:

A solution containing a mixture of 0.05M NaCI and 0.05M Nal is taken. (K_(sp) of AgCI = 10^(-10) and K_(sp) of AgI = 4 xx 10^(-16)) . When AgNO_(3) is added to such a solution:

The solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))

The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))

If the solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

The following solutions are mixed: 500mL of 0.01 M AgNO_(3) and 500mL solution that was both 0.01M in NaCI and 0.01M in NaBr . Given K_(sp) AGCI = 10^(-10), K_(sp) AgBr = 5 xx 10^(-13) . Calculate the [Ag^(o+)] in the equilibrium solution.

The following solutions are mixed: 500mL of 0.01 M AgNO_(3) and 500mL solution that was both 0.01M in NaCI and 0.01M in NaBr . Given K_(sp) AGCI = 10^(-10), K_(sp) AgBr = 5 xx 10^(-13) . Calculate the [Ag^(o+)] in the equilibrium solution.

The solubility of AgCl in 0.2 M NaCl is [K_(sp) AgCl =1.8 xx 10^(-10)]