2. Salt-in effect implies that solubility: a. Remains constant with increase in ionic strength b. Increases with increase in ionic strength c. Decreases with increase in ionic strength In boiling point elevation experiment, Beckman thermometer is used to measure temperature variations because: 3 O a. It can withstand high temperature O b. It is more accurate than digital thermometers O c. It has an accuracy of 0.01°C d It is easier to read than digital

2. Salt-in effect implies that solubility: a. Remains constant with increase in ionic strength b. Increases with increase in ionic strength c. Decreases with increase in ionic strength In boiling point elevation experiment, Beckman thermometer is used to measure temperature variations because: 3 O a. It can withstand high temperature O b. It is more accurate than digital thermometers O c. It has an accuracy of 0.01°C d It is easier to read than digital

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter31: An Oxidation–reduction Scheme: Borneol, Camphor, Isoborneol

Section: Chapter Questions

Problem 4Q

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Sodium chloride (NaCl) was isolated from SiO2 and CaCO3 by dissolving it in distilled water. Unmentioned is that CaCO3 is slightly soluble in water (0.001 g/100 mL). Describe the effect this fact will have on each component of the mixture: will the “isolated“ mass of each be greater than, equal to, or less than that in the sample?
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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 vapor pressure of the solution to 3 decimal places in atm.
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