Find the concentration of Ba2+ in a 0.100 M (CH 3 ) 4 NIO3 solution saturated with Ba(IO3 ) 2 . Thesolubility product constant for barium iodate is 1.5 x 10–9 . (CH 3 ) 4 N + is a derivative ofammonium. What would be the concentration of Ba2+ if the (CH 3 ) 4 NIO3 were replaced with(CH 3 ) 4 NCl show the work

A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?

You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is reported to have a Ksp value of zero in water at 25C. What does this mean?

A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.

Sodium carbonate is added to a solution in which the concentration of Ni2+ ion is 0.0024 M. Will precipitation of NiCO3 occur (a) when the concentration of the carbonate ion is 1.0 106 M or (b) when it is 100 times greater (1.0 104 M)?

Cadmium(ll) chloride is added to a solution of potassium hydroxide with a pH of 9.62. (KspCd(OH)2=2.51014) (a) At what concentration of Cd2+ does a precipitate first start to form? (b) Enough cadmium(II) chloride is added to make [ Ca2+ ]=0.0013 M. What is the pH of the resulting solution? (c) What percentage of the original hydroxide ion is left in solution?

Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl. After the solution has come to equilibrium it is saturated with H2S ( H2S[H2S]=0.10M). What concentrations of Pb2+ and Fe2+ remain in the solution? For a saturated solution of H2S we can use the equilibrium: H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026 (Hint: The [H3O+] changes as metal sulfides precipitate.)

What mass of Ca(NO3O)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 1011 and Ka, for HF = 7.2 104. Assume no volume change on addition of Ca(NO3)2(s).

. Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.