Solid sodium carbonate is slowly addedto 150 mL of a 0.0426 M nickel(II)acetate solution. The concentration ofcarbonate ion required to just initiateprecipitation isМ. Solid sodium carbonate is slowly addedto 50.0 mL of a nickel(II) iodide solutionuntil the concentration of carbonate ionis 0.0518 M. The maximum amount ofnickel ion remaining in solution isМ.

The Ksp is also known as the solubility product constant refers to the equilibrium which is present…

Answered: Solid sodium carbonate is slowly added…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section15.4: Solubility Equilibria And The Solubility Product Constant, Ksp

Problem 15.9CE

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Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
A 45.0-mL sample of 0.0015 M BaCl2 was added to a beaker containing 75.0 mL of 0.0025 M KF. Will a precipitate form?
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?
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?
Will a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?
Solid barium acetate is slowly added to 50.0mL of a 0.0573M potassium carbonate solution. The concentration of barium ion required to just initiate precipitaion is?
Solid Lead Nitrate is slowloy added to 150mL of a 0.0386 M sodium sulfate solution. The concentration of lead ion required to just initiate precipitation is M?
The Solubility Product Constant for barium phosphate is 1.3 x 10^-29 . Solid sodium phosphate is slowly added to 125 mL of a 0.0382 M barium acetate solution. The concentration of phosphate ion required to just initiate precipitation is M.
The Solubility Product Constant for lead phosphate is 3.0 x 10^-44. Solid potassium phosphate is slowly added to 150 mL of a 0.0680 M lead acetate solution. The concentration of phosphate ion required to just initiate precipitation is ____ M.
Solid sodium hydroxide is slowly added to 125 mL of a 0.0449 M chromium(III) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is M.
25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?

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