Solid `Ba(NO_(3))_(2)` is gradually dissolved in a `1.0xx10^(-4)M" "Na_(2)CO_(3)` solution. At what concentration of `Ba^(2+)` will a precipitate begin to form ? (`K_(sp)` for `BaCO_(3)=5.1xx10^(-9)`).

At 25^(@)C , equal volumes of 0.04 (M) CaCl_(2) and 0.01(M) Na_(2)SO_(4) solution are mixed. Will CaSO_(4) be precipitated in the resulting solution? K_(sp)(CaSO_(4))=2.4xx10^(-5)(25^(@)C) .

10^(-4) mol Pb(NO_3)_2,10^(-4) mol Ca(NO_3)_2 and 10^(-3) mol Na_2CO_3 are added to 500 mL of water. Will there be any precipitation? If so, which will be precipitated? [Given: K_(sp)(PbCO_3)=7.4xx10^(-14) and K_(sp)(CaCO_3)=6.0xx10^(-9) ]

If equal volumes of 0.02(M) CaCl_2 and 0.0003(M) Na_2SO_4 solutions are mixed, will CaSO_4 be precipitated ? [Given : K_(sp)(CaSO_4)=2.4xx10^(-15) ]

Calculate the concentrations of Ca^(2+) and PO_4^(3-) ions in a saturated [Ca_3(PO_4)_2] solution. Given: K_(sp)[Ca_3(PO_4)_2]=2.0xx10^(-29) (at 25^(@)C )

At 25^(@)C what is the concentration of H_(3)O^(+) ions in an aqueous solution in which the concentration of OH^(-) ions is 2xx10^(-5)(M) ?

pH of human blood is maintained by the balance in concentrations of H_(2)CO_(3) & NaHCO_(3) . What volume of 5(M) NaHCO_(3) solution is to be added to 10 mL of a blood sample containing 2(M) H_(2)CO_(3) in order to maintain the pH at 7.4 ? [K_(a)(H_(2)CO_(3))=7.8xx10^(-7) ]

At what concentration of PO_(4)^(3-) ions in 0.1(M) aqueous solution of AgNO_(3), will Ag_(3)PO_(4) start to precipitate?Given: K_(sp)(Ag_(3)PO_(4))=1.3xx10^(-20) .

Determine the pH of an aqueous solution of ammonia if the concentration of the solution is 3(M). K_(b) (ammonia) =1.8xx10^(-5) .

If equal volumes of the given solutions are mixed, precipitation of AgCl(K_(sp)=1.8xx10^(-11)) will occur only with -

At what value of pH of 0.1 (M) aqueous FeCl_(3) solution, will Fe(OH)_(3) start to precipitate? Given: Solublity product of Fe(OH)_(3)=2.0xx10^(-39) .