I. heating III. adding a non-electrolyte solution A. I only II. stirring IV. adding cold distilled water В. П only С. Ш only D. I & Π Е. I & II
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- Figure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If 255 g of AgNO3 is added to 100 g of water at 95°C and cooledslowly, at what temperature will the solution becomesaturated?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)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 mL
- The mass of magnesium fluoride that is dissolved in 150 mL of a saturated solution is _______ grams. The volume of water needed to dissolve 0.0671 grams of calcium hydroxide is ______ L.Assume no volume change upon addition of the solid.The Ksp of Pbl2 is 8.4 x 10^-9. The molar mass of Pbl2 is 461.03 g/mol. The mass solubility (g/L) of Pbl2 in 0.015 M Pb(NO3)2 is?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.
- The colloidal particles has tenth ofmm diameter and easily filtered tru or false(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?The following data table indicates the solubility of a substance. By examining the data presented, predict the solubility of the substance at 50 oC. Temperature (oC) Solubility (mM) 5 5.00 15 4.35 25 3.70 35 3.05 45 2.40
