Tutored Practice Problem 18.2.3 COUNTS TOWARDS GRADE Use the reaction quotient to predict whether a precipitate will form. Close Problem If 12.0 mL of 1.10x10-4 M Ba(OH)₂ are added to 25.0 mL of 7.60x10-5 M Na₂CO3, will solid BaCO3 (Ksp = 8.1x109) precipitate? If a precipitate will not form, what carbonate ion concentration will cause a precipitate of barium carbonate to form? If a precipitate will form, what is the minimum [CO32-] that could have been present without initiating precipitation? Assume the total volume used in the above example. M

Tutored Practice Problem 18.2.3 COUNTS TOWARDS GRADE Use the reaction quotient to predict whether a precipitate will form. Close Problem If 12.0 mL of 1.10x10-4 M Ba(OH)₂ are added to 25.0 mL of 7.60x10-5 M Na₂CO3, will solid BaCO3 (Ksp = 8.1x109) precipitate? If a precipitate will not form, what carbonate ion concentration will cause a precipitate of barium carbonate to form? If a precipitate will form, what is the minimum [CO32-] that could have been present without initiating precipitation? Assume the total volume used in the above example. M

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 37P

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Solid silver chromate is added to pure water at 25 °C, and some of the solid remains undissolved. The mixture is stirred forseveral days to ensure that equilibrium is achieved between the undissolved Ag2CrO4(s) and the solution. Analysis of theequilibrated solution shows that its silver ion concentration is 1.3 x 10-4 M. Assuming that the Ag2CrO4 solution is saturatedand that there are no other important equilibria involving Ag+ or CrO42 - ions in the solution, calculate Ksp for this compound.
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When 18.0 mL of a 6.86 x 10^-4 M lead acetate solution is combined with 12.0 mL of a 2.28 X10^-4 M potassium chloride solution does a precipitate form? (ksp PbCl2 =1.7 X10^-5) Yes, the precipitate forms. No, the precipitate doesn't form . For these conditions the Reaction Quotient, is equal to .....M
(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?Ksp = __________(b) It is found that 8.90e-06 g of Y2(CO3)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Y2(CO3)3.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3? solubility = ________mol/L
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When 22.0 mL of a 7.86X 10^-4 M ammonium carbonate solution is combined with 25.0 mL of a 1.44 X10^-4 M zinc acetate solution does a precipitate form? (Ksp of ZnCO3 = 1.5 X10^-11) a)Yes, the precipitate forms. b)No, the precipitate doesn't form. For these conditions what is the Reaction Quotient Q .
The molar solubility of magnesium carbonate in a water solution is _______________ M Ksp = 4.0 × 10-5
A saturated solution of BaF2 at 25°C is prepared by equilibrating solid BaF2 with water. Powdered NaF is then dissolved in the solution until the solubility of BaF2 is 1.0% of that in H2O alone. The solubility product Ksp of BaF2 is1.7 × 10-6 at 25°C. Calculate the concentration of fluoride ion in the solution after addition of the powdered NaF.
1. Write the dissociation reaction and solubility product constant expression for the following sparingly soluble salt. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 2. Determine the Molar Solubility of the following sparingly soluble salt in water. a. AgBr Ksp = 5.2 x 10-13 b. PbCl2 Ksp = 1.7 x 10-5 3. Express the solubility (S) in question #2 in g/L. 4. Calculate Ksp for the ff. substances, given the molar concentration of their saturated solution. a. Ag2C2O4 ( S= 2.06 x 10-4 ) b. Al(OH)3 ( S = 1.82 x 10-9 ) 5. Calculate the molar solubility of the salts in problem #2 for the solution in which the cation concentration is 0.050 M.
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