A solution contains `2.3 xx 10^(-3) M Ag NO_(3)`. What concentration of NaCl will be required to initiate the precipitation of AgCl.
The solubility product of AgCl is `2.8 xx 10^(-10)` ?

A solution contains 1.4 xx 10^(-3)M AgNO_(3) . What concentration of KC1 will be required to initiate the precipitation of AgC1 ? K_(sp) AgC1 = 2.8 xx 10^(-10)

A solution contains 1.4 xx 10^(-3)M AgNO_(3) . What concentration of KC1 will be required to initiate the precipitation of AgC1 ? K_(sp) AgC1 = 2.8 xx 10^(-10)

What will be the solubility of AgCl in 0.05 M NaCl aqueous solution if solubility product of AgCl is 1.5xx10^(-10) ?

What will be the solubility of AgCl in 0.05 M NaCl aqueous solution if solubility product of AgCl is 1.5xx10^(-10) ?

AgCl is dissolved separately in pure water and in 0.025(M) NaCl solution. Find the ratio of concentrations of Ag^(+) ion in pure water and in the NaCl solution. The solubility product of AgCl is 1.75xx10^(-10) .

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

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

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

The molar solubility of AgCl in 1.8 M AgNO_(3) solution is ( K_(sp) of AgCl = 1.8 xx 10^(-10) )