What is the concentration of `Pb^(2+)` when `PbSO_(4)` `(K_(sp)=1.8xx10^(-8))` begins to precipitate from a solution that is 0.0045 M in `SO_(4)^(2-)`?
What is the concentration of Ba^(2+) when BaF_(2) (K_(sp)=1.0xx10^(-6)) begins to precipitate from a solution that is 0.30 M F^(-) ?
What is the hydronium ion concentration of a 0.25 M HA solution? (K_(a)=4xx10^(-8))
What is the molarity of a saturated solution of CaCO_(3) ? (K_(sp)=2.8xx10^(-9))
The solubility product of BaSO_(4)" at " 25^(@) C " is " 1.0 xx 10^(-9) . What would be the concentration of H_(2)SO_(4) necessary to precipitate BaSO_(4) from a solution of 0.01" M Ba"^(+2) ions
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)]
Calculate pH at which Mg(OH)_(2) begins to precipitate from a solution containing 0.10M Mg^(2+) ions. (K_(SP)of Mg(OH)_(2)=1xx10^(-11))
What is the pH value at which Mg(OH)_(2) begins to precipitate from a solution containing 0.2 M Mg^(+2) ions ? K_(SP) of Mg(OH)_(2) is 2 xx 10^(-13) M^(2) ?
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 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) )
