What is minimum concentration of `SO_(4)^(2-)` required to precipitate `BaSO_(4)` in solution containing `1 xx 10^(-4)` mole of `Ba^(2+)` ? (`K_(sp)` of `BaSO_(4) = 4 xx 10^(-10)`)

What is the minimum concentration of sulphuric acid required to initiate the precipitation of BaSO_4 from a solution containing 7xx10^(-8) mol L^(-1) of BaCl_2 ? [K_(sp)(BaSO_4)=1.4xx10^(-10)]

What is the minimum concentration of Ba^(+2) ions required in order to initiate the precipitation of BaSO_(4) from a solution containing 0.002 mole L^(-1) of SO_(4)^(-2) ions? (Given K_(sp) for BaSO_(4)=1.4xx10^(-10))

What is the minimum concentration of Ba^(+2) ions required in order to initiate the precipitation of BaSO_(4) from a solution containing 0.002 mole L^(-1) of So_(4)^(-2) ions? (Given K_(sp) for BaSO_(4)=1.4xx10^(-10))

What is the minimum concentration of Ba^(+2) ions required in order to initiate the precipitation of BaSO_(4) from a solution containing 0.002 mole L^(-1) of So_(4)^(-2) ions? (Given K_(sp) for BaSO_(4)=1.4xx10^(-10))

Calculate the concentration of SO_4^(2-) ions necessary to cause the precipitation of BaSO_4 (K_(sp)=1.5xx10^(-9)) from solution of BaCl_2 (0.5 M)

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)]