Determine the molar solubility for Cr(OH)3 (Ksp 6.3 x 1 31) in an aqueous solution that has a pH of 11.90 at 25 °C. %3D PREV 2 NEXT Based on your ICE table, set up the expression for Ksp in order to determine the unknown. Do not combine or simplify terms. Ksp [x] [3x]" = 6.3 x 10-31 %3D
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- The Ksp of barium chromate is given below. What is the molar solubility, in g/L? Include units in your answer. Ksp=1.2x10^-10Ammonium acetate buffer is used as an important reagent for studying molecular biology, biological buffers, reagents and DNA and RNA purification. Ammonium acetate (0.24M) in combination with cold 66% (v/v) ethanol quantitatively precipitated RNA from very dilute solutions (greater than or equal to μg/ml) after centrifugation. Ammonium acetate (CH3COONH4) is also a salt of weak acid (CH3COOH) and weak base (NH4OH). The Ka and Kb are equal to 1.8 x10-5. The pH of this salt solution will be, a. pH > 7 b. pH ≈ 7 c. pH < 7 d. both cation and anion don’t hydrolyze. e. none of the above.Calculate the molar solubility and solubility in g/L of lithium fluoride (LiF, 25.939 g/mol) in pure water. Ksp = 1.7 x 10-3 Calculate the molar solubility and solubility in g/L of gold(III) chloride (AuCl3, 303.33 g/mol) in pure water. Ksp = 3.2 x 10-25 Calculate the molar solubility and solubility in g/L of gold(III) chloride in a solution that is 0.010 M in MgCl2. Ksp = 3.2 x 10-25
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- Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is 8 mL consumption, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) What is the solubility of benzoic acid at 27 ° C? b) What is the solubility of benzoic acid at different temperatures? c) What is the second test temperature? (M (benzoic acid): 122.12 g / mol)A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state. Ba2+ (aq) -560.77 kJ/mol Delta Gfo Cl- (aq) -131.228 kJ/mol Delta Gfo BaCl2 -1296.32 kJ/mol Delta GfoConsider a solution that is made from mixing 122.3ml of 0.333M ZnCl2 and 83.57ml of 0.654M Na2CO3 a. What is the concentration of cations and anions at equilibrium(in molarity)? Use x-is-small approximation. b. What is the ‘net’ amount of precipitate produced(in moles)? ksp (ZNCO3) = 1 x 10^-10