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41 solutions

Selective Precipitation

Q. The Ksp of Al(OH)3 is 2 ✕ 10−32. At what pH will a 0.48 M Al3+ solution begin to show precipitation of Al(OH)3? (Assume Kw = 1.00 ✕ 10−14.)

Solved • Dec 3, 2019

Selective Precipitation

Q. The concentration of Mg2+ in seawater is 0.046 M. At what pH will 99% of the Mg2+ be precipitated as the hydroxide salt? (Ksp for Mg(OH)2 = 8.9 ✕ 10−12. Assume that all solutions are at 25°C.)

Solved • Dec 3, 2019

Selective Precipitation

Q. Consider a solution containing the following cations: Na+, Hg2+, Mn2+, Al3+, Ag+. Treatment of the solution with dilute HCl followed by saturation results in the formation of precipitate(s). Which ions still remain in solution (i.e. did not precipitate)?

Solved • Nov 15, 2019

Selective Precipitation

Q. Which, if any of the following mixtures will result in a precipitate. You might need to know that the Ksp for AgCN is 2.2 x 10^-16 and that for PbI2 is 7.9 x 10^-19 I. A mixture that is 1.2 x 10^-6 M AgNO3 and 2.4 x 10^-10 M NaCN II. A mixture that is 2.3 x 10^-4 M Pb(ClO4)2 and 4.6 x 10^-3 KI

Solved • Nov 15, 2019

Selective Precipitation

Q. 7. A solution contains 0.80 M iron (II) ions and 0.80 M iron (III) ions. What amount in moles of sodium hydroxide must be added to completely precipitate the Fe (II) ions? Fe(OH)2 Ksp=1.6x10^-14 Fe(OH)3 Ksp=1.1x10^-36

Solved • Oct 2, 2019

Selective Precipitation

Q. Solid AgCl has been placed in a beaker of water. After some time, the concentrations of Ag^+ and Cl^- are each 1.0x10^-5 mol/L. Has the system reached equilibrium? If not, will more AgCl dissolve? Ksp (AgCl) = 1.8x10^-10

Solved • Nov 5, 2019

Selective Precipitation

Q. Assume the solubility product of Mg(OH)2 is 1.5 x 10^-11 at a certain temperature. What minimum OH- concentration must be attained (for example, by adding NaOH) to decrease the Mg2+ concentration in a solution of Mg(NO3)3 to less than 1.5 x 10^-10 M. ___ M (Enter your answer in scientific notation.)

Solved • Nov 2, 2019