The solubility of Caso4 (MM=132.6) is 0.191 g per 100 mL. Find the solubility product constant. 2.07 x 10-6 2.07 x 10-4 1.44 x 10-4 1.44 x 10-2
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- Which of the following is more likely to precipitate the hydroxide ion? Cu(OH)2(s) *=» Ctr+(aq) + 2 OH’(aq) K = 1.6 X IO-19 Ca(OH)2(s) *=» Ca2+(aq) + 2 OH’(aq) K = 7.9 X 10"6Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3(Ksp=1.36107). (b) If the NiCO3 were a contaminant in a sample of COCO3(Ksp=1.01012), what mass of COCO3 would have been lost? Keep in mind that both NiCO3 and COCO3 dissolve in the same solution.The solubility-product constant for Ce(IO3)3 is 3.2x10-10 . What is the Ce3+ concentration in a solution prepared by mixing 40.00 mL of 0.0420 M Ce3+ with 40.00 mL of water? M 0.0420 M IO3-? M 0.260 M IO3-? M 0.0470 M IO3-? M
- Consider a solution containing 0.181 M lead ions and 0.174 M mercury(II) ions. The Ksp for lead sulfide is 3.4 x 10-28 and that for mercury(II) sulfide is 4.0 x 10-53. Calculate the maximum concentration of sulfide ions that can be in solution without precipitating any lead ions. The answer is 1.4 x 10-27How much potassium oxalate can be added to 156.0 mL of 0.5 M [Cu(NH3)4]Cl2 before a precipitate of CuC2O4 begins to form? Ksp(CuC2O4)=2.9x10-8 and Kf(Cu(NH3)42+)=1.1x1012Include at least 3 significant figures in your answer.The solubility of CaSO4 (MM=132.6) is 0.191 g per 100 mL. Find the solubility product constant. 2.07 x 10-6 2.07 x 10-4 1.44 x 10-2 1.44 x 10-4
- What is the solubility of Sr3SO₄ in a solution that contains 0.090 M Sr3+ ions? (Ksp of SrSO₄ is 3.44×10⁻⁷)The solubility of lead iodide (PbI2) at 0 °C is 0.044 g in 100 mL of water. Calculate the solubility product of PbI2 at this temperature. a. 3.5 x 10-10 b. 8.7 x 10-10 c. 3.5 x 10-9 d. 7.9 x 10-9 e. 9.5 x 10-4The maximum amount of copper(II) sulfide that will dissolve in a 0.124 M potassium sulfide solution is ______ M. Ksp = 7.9 x 10-37
- One way to reduce the presence of lead in water is to add a phosphate corrosion inhibitor, which forms an insoluble saltwith lead, coating the pipes with a protective mineral later: Pb3(PO4)2(s) ⇌ 3Pb2+(aq) + 2PO43-(aq) Kc=9.9 x 10-55 a.) Calculate the solubility of lead (Pb2+) in g/L when Pb3(PO4)2 is dissolved in water. b.) The acceptable level of lead in water is less than 1x10-6g/L. If phosphate is added to drinking water, does it keep the lead levels below the allowed limit? c.) In 2014, the city of Flint, MI, changed water sources to a system that didn’t include phosphate. Instead, it used chlorine to treat water. The Ksp of lead chloride is 1.5x10-5. The switch increased the levels of lead in the drinking water and significantly affected the community. Explain why switching water sources increased the lead levels in Flint’s drinking water.Consider a slightly soluble salt with a general form of MX(s) --> M+(aq) + X-(aq). If Ksp = 6.7 x 10-4 for a salt with a molar mass of 142 g/mol and there is 800 mg of this salt dissolved in 1 L, which of the following is true?Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver? Question 4 options: a) 6.37 × 10-5 b) 0.0637 c) 3.73 × 10-3 d) 0.218