[" A solution contains "0.1MBa(NO_(3))_(2)" and "0.1MSr(NO_(3))_(2)" .If solid "Na_(2)CrO_(6)" is added to the "],[" soluton,the [ textrmBa ^ 2- ] " concentration when " SrC _ 10 ," begins to precipitate is " "],[" (Given "K_(rp)BaCrO_(4)=1.4times10^(-10);K_(p)SrCrO_(4)=3.5times10^(-5))]

A solution is 0.10 M Ba(NO_(3))_(2) and 0.10 M Sr(NO_(3))_(2.) If solid Na_(2)CrO_(4) is added to the solution, what is [Ba^(2+)] when SrCrO_(4) begins to precipitate? [K_(sp)(BaCrO_(4))=1.2xx10^(-10),K_(sp)(SrCrO_(4))=3.5xx10^(-5)]

A solution is 0.10 M Ba(NO_(3))_(2) and 0.10 M Sr(NO_(3))_(2.) If solid Na_(2)CrO_(4) is added to the solution, what is [Ba^(2+)] when SrCrO_(4) begins to precipitate? [K_(sp)(BaCrO_(4))=1.2xx10^(-10),K_(sp)(SrCrO_(4))=3.5xx10^(-5)]

A solution is 0.10 M Ba(NO_(3))_(2) and 0.10 M Sr(NO_(3))_(2.) If solid Na_(2)CrO_(4) is added to the solution, what is [Ba^(2+)] when SrCrO_(4) begins to precipitate? [K_(sp)(BaCrO_(4))=1.2xx10^(-10),K_(sp)(SrCrO_(4))=3.5xx10^(-5)]

A solution contains 0.1 M is 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? (Ksp (AgCl) = 10^(-10) M^(2) , K_(sp) (Ag_(2)CrO_(4)) = 10^(-12)M^(3))

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 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)]

Solid Na_(2)SO_(4) is slowly added to a solution which is 0.020 M in Ba(NO_(3))_(2) and 0.020 M is Pb(NO_(3))_(2) . Assume that there is no increase in volume on adding Na_(2)SO_(4) . There preferential precipitation takes place. What is the concentration of Ba^(2+) when PbSO_(4) starts to precipitate? [K_(sp)(BaSO_(4))=1.0xx10^(-10) and K_(sp)(PbSO_(4))=1.6xx10^(-8)]

Solid Na_(2)SO_(4) is slowly added to a solution which is 0.020 M in Ba(NO_(3))_(2) and 0.020 M is Pb(NO_(3))_(2) . Assume that there is no increase in volume on adding Na_(2)SO_(4) . There preferential precipitation takes place. What is the concentration of Ba^(2+) when PbSO_(4) starts to precipitate? [K_(sp)(BaSO_(4))=1.0xx10^(-10) and K_(sp)(PbSO_(4))=1.6xx10^(-8)]