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Q: What is the solubility of PbF₂ in a solution that contains 0.0800 M F⁻ ions? (Ksp of PbF₂ is 3.60 ×…
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- The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mLA 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)Estimate the aqueous gram-solubility in g/L of mercury(I) chloride: Hg2Cl2(s) ↔ 2Hg+ (aq) + 2Cl– (aq), Ksp = 1.43×10–18 The molar mass of Hg2Cl2 is 472.06 g/mol.
- If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte.found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs:CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac)and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.
- Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte. found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs: CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac) and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.Calculate the solubility at 25°C of CoOH2 in pure water and in a 0.0100M CoCl2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0100 M CoCl2 solution: gLSolid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.