Which of the following salts would have the greatest solubility in water? Formula Ksp A) AGCI AgCI 1.8 x 10-10 B) LaFs LaF3 2 x 10-19 C) CuBr CuBr 5.3 x 10-9 D) CaF: CaF2 3.5 x 10-11
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Which of the following salts would have the greatest solubility in water?
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- The Henry’s law constant for CO2 in water at 25 °C is3.1x 10-2 M atm-1. (a) What is the solubility of CO2 inwater at this temperature if the solution is in contact withair at normal atmospheric pressure? (b) Assume that all ofthis CO2 is in the form of H2CO3 produced by the reactionbetween CO2 and H2O:CO2(aq) + H2O(l)------>H2CO3(aq)What is the pH of this solution?A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal places
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)What is the boiling point rise in oF of a 15% solution of nitric acid in water boiling at 200oF? Need asap
- 1. Calculate the solubility of calcium carbonate water temperature of 5 °C; at that temperature, Ksp = 8.1 x 10-9 for CaCO3, Ka = 2.8 x 10-11 for HCO3-, and Kw = 2.0 x 10-15An aqueous chloric acid solution has a sp. gr. of 1.124 and contains 26.02% by mass. Calculate M, N, m, mole fraction of solute, BP, FP, and osmotic pressure at 25.0°C assuming 100% effective ionization.KNO3 (aq) added to CaC2O4 (Ksp = 1.3 x 10-8) in solution will lead to __________ in solubility of the solid no effect then decrease increase no effect
- 23. The Ksp of CuCO3ls) (copper carbonate, a salt) is reported as 2.21x10-11. Determine the solubility (in mg/L) of 1this salt in pure water Constants: The molecular mass (M) of copper carbonate (CuCOg) is 123.554 g mol-12.3 - At temperature of 18°C was 4,7 g of silver molybdate (M = 376 g mol–1) mixed with 500 cm3 of a) distilled water b) solution of AgNO3 with concentration of 0,02 mol dm–3 c) solution of Na2MoO4 with concentration of 0,02 mol dm–3 Determine, how many percent of Ag2MoO4 will dissolve in each case. Solubility equilibrium of Ag2MoO4 is 3,1.10-11.A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.