10. The molar solubility of silver chromate, [Ag2CrO4] is 8.80 x 10-5 mol/L.Calculate Ksp for this compound. [HINT: Ag ion is +1].a 3.21 x 10-8b) 6.34 x 10-23.27 x 10-7d)) 2.73 x 10-12e) 4.06 x 10-14f) 5.07 x 10-13g) 2.96 x 10-10As a GoyKSP

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Answered: 10. The molar solubility of silver…

Chemistry for Engineering Students

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Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.109PAE: 12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar...

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Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) KHC4H4O6. (b) PbI2. (c) Ag4[Fe(CN)6], a salt containing the Fe(CN)4- ion. (d) Hg2I2
12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its Ksp.
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product: (a) Ag2SO4. (b) PbBr2. (c) AgI. (d) CaC2O4H2O
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?
A solution contains 0.0150 M lead(II) ion. A concentrated sodium iodide solution is added dropwise to precipitate lead iodide (assume no volume change). a At what concentration of I does precipitate start to form? b When [I] = 2.0 103 M, what is the lead-ion concentration? What percentage of the lead(II) originally present remains in solution?
Consider the insoluble salts JQ, K2R, L2S3, MT2, and NU3. They are formed from the metal ions J+, K+, L3+, M2+, and N3+ and the nonmetal ions Q-, R2-, S2-, T-, and U-. All the salts have the same Ksp, 11010 at 25C. (a) Which salt has the highest molar solubility? (b) Does the salt with the highest molar solubility have the highest solubility in g salt/100 g water? (c) Can the solubility of each salt in g/ 100 g water be determined from the information given? If yes, calculate the solubility of each salt in g/100 g water. If no, why not?
How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?
. 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.
Consider the equilibrium curve for AgCl shown below. Which of the following statements about a solution at point A on the curve are true? (a) The solution is saturated and at equilibrium. (b) Addition of NaCl increases the concentration of Cl- in solution. (c) Addition of NaCl increases the concentration of in solution. (d) Addition of Ag+ results in the precipitation of AgCl. (e) Addition of solid NaNO3 to the solution without change in volume does not change [Ag+] or [Cl-].
The Ksp value for radium sulfate, RaSO4, is 4.2 1011. If 25 mg of radium sulfate is placed in 1.00 102 mL of water, does all of it dissolve? If not, how much dissolves?

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10. The molar solubility of silver chromate, [Ag2CrO4] is 8.80 x 10-5 mol/L. Calculate Ksp for this compound. [HINT: Ag ion is +1]. a 3.21 x 10-8 b) 6.34 x 10-2 3.27 x 10-7 d)) 2.73 x 10-12 e) 4.06 x 10-14 f) 5.07 x 10-13 g) 2.96 x 10-10 As a Goy KSP