A solution is 0.01 M Kl and 0.1 M KCl. If solid `AgNO_(3)` is added to the solution, what is the `[l^(-)]` when AgCl begins to precipitate?
`[K_(SP)(Agl)=1.5xx10^(-16),K_(SP)(AgCl)=1.8xx10^(-10)]`

A solution is 0.01 M Kl and 0.1 M KCl. If solid AgNO_(3) is added to the solution, what is the [I^(-)] when AgCl begins to precipitate? [K_(SP)(Agl)=1.5xx10^(-16),K_(SP)(AgCl)=1.8xx10^(-10)]

A solution is 0.01 M Kl and 0. 1 M KCl . If solid AgNO_3 is added to the solution, what is the [1^(-) ] when AgCl begins to precipitate [K_(sp) (Agl) =1.5 xx 10^(-16) , K_(sp) (AgCl) =1.8 xx 10^(-10)]

A solution of 0.1 M in Cl^(-) and 10^(-4) M CrO_(4)^(-2) . If solid AgNO_(3) is gradually added to this solution, what will be the concentration of Cl^(-) when Ag_(2)CrO_(4) begins to precipitate? [K_(sp)(AgCl)=10^(-10)M^(2),K_(sp)(Ag_(2)CrO_(4))=10^(-12) M^(3)]

A solution is a mixture of 0.05 M NaCl and 0.05 M AgI. The concentration of iodide in the solution when AgCl just starts precipitating is equal to: (K_(sp)AgCl=1xx10^(-10)M^(2), K_(sp)AgI=4xx10^(-16)M^(2))

A solution is a mixture of 0.05 M NaCl and 0.05 M NaI. The concentration of iodide in the solution when AgCl just starts precipitating is equal to: (K_(sp)AgCl=1xx10^(-10)M^(2), K_(sp)AgI=4xx10^(-16)M^(2))

A solution is a mixture of 0.06M KCl and 0.06 M Kl. AgNO_(3) solution is being added drop by drop till AgCl starts precipitating (K_(sp)AgCl=1xx10^(-10) and K_(sp)Agl=4xx10^(-16)) . The concentration of iodide ion at this instant will be nearly equal to :

On addition of increasing amount of AgNO_3 to 0.1 M each of NaCl and NaBr in a solution, what % of Br^- ion gets precipitated when Cl^- ion starts precipitating? K_(sp)(AgCl)= 1.0 xx 10^(-10), K_(sp)(AgBr)=1xx10^(-13)