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Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0080M BaCl2 solution.
Ksp is
BaCrO4
|
1.17×10-10
|
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Solved in 2 steps
- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLThe Ksp of Ba(IO3)2 at 25 °C is 6.0 * 10-10. What is the molar solubility of Ba(IO3)2?What is the molar solubility (in mol L-1¹) of a salt with general molecular formula MX₂ (where M is a cation and X is an anion) in a solution already containing 0.513 mol L-¹ X-? The Ksp of MX₂ = 2.01 x 10-8
- The solubility-product constants, Kp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Кар FeCO3 2.10 x 10-11 CdCO3 1.80 x 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.03x10-2 M Fe2+ and 1.52x10-2 MCd2+. What concentration of CO² is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ▸ View Available Hint(s) [CO32] = Value Units Submit Part B Complete previous part(s) Part C Complete previous part(s) Provide Feedback ? Next >What is the solubility of barium sulfate in a solution containing 0.050 M sodium sulfate? The Ksp value for barium sulfate is 1.1 x10-10.2) 3) Using equilibrium table, calculate the molar solubility of PbF2 [Ksp - 4x10"] in 0.035 M NaF aq. solution. mL. Using equilibrium table, calculate the Ksp of CaCO3 at this temperature. [Molar The solubility of CaCO3 in water at a certain temperature is 3.5x102 g/50 mass of CaCO3 is 100 g/mol] 4) Calculate the moles of acetic acid CH3COOH that should be added to 2.5 L of 0.35 M sodium acetatc CH3COONa aq. solution to prepare a buffer solution with pH of 4.8. [Ka acetic acid = 1.8x10-]
- What is the molar solubility of barium Florida in water? The Ksp is 1.7 x 10-6.The solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10 x 10-11 CdCO3 1.80 × 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.02x10-2 MFe²+ and 1.48x10-2 M Cd²+. What concentration of CO3²- is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ► View Available Hint(s) [CO3²- ] = Submit μA Value Part B Complete previous part(s) Part C Complete previous part(s) Units ?Oxalic acid forms a precipitate with calcium ion Ca2+ (aq) + C2H204(ag) + H20(1) -> CaC2O4*H20 (s) + 2 H* (ag). The Ksp for calcium oxalate is 1.3 x 10^-8. A solution is prepared that initially contains 0.04 moles of Ca2+ and 0.04 moles of oxalic acid in 0.100 L of water. Based only on the Ksp value, how many moles of Ca2+ are in solution when equilibrium is reached? Using Le Chatelier's principle, suggest two things you could do, that would reduce the amount of Ca2+ remaining in solution.