B identify wnat is correCtIT not, wIne2. Use the following information to answer the questions below:Density of carbon tetrachloride is 1.584 g/cm3Boiling point elevation constant of carbon tetrachloride is 4.95 °C/mNormal boiling point of carbon tetrachloride is 76.8 °Ca. Calculate the boiling point of a solution made by mixing 25.56 grams of solidiodine with 250 ml carbon tetrachloride. (Show all work)b. Calculate the boiling point of a solution made by mixing 25.56 grams of solidnaphthalene (C10H8) with 250 ml carbon tetrachloride. (Show all work).thio ooloulation supnort or refute the

Given: Mass of C10H8 dissolved = 25.56 g. Volume of CCl4 = 250 mL.

Answered: b. Calculate the boiling point of a…

b. Calculate the boiling point of a solution made by mixing 25.56 grams of solid naphthalene (C10H8) with 250 ml carbon tetrachloride. (Show all work). thie ooloulotion supnort or refute the

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 73QAP: Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol,...

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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Specifications for lactated Ringers solution, which is used for intravenous (IV) injections, are as follows to reach 100. mL of solution: 285315 mg Na+ 14.117.3 mg K+ 4.9Q.O mg Ca2+ 368408 mg Cl 231261 mg lactate, C3H5O3 a. Specify the amount of NaCl, KCl, CaCl2 2H2O, and NaC3H5O3 needed to prepare 100. mL lactated Ringers solution. b. What is the range of the osmotic pressure of the solution at 37C, given the preceding specifications?
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of 5.20C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
Analysis of a compound gave 39.50% C, 2.21% H, and 58.30% Cl. When 0.855 g of this solid was dissolved in 7.50 g of naphthalene, the solution had a freezing point of 78.0C. The pure solvent freezes at 80.0C; its molal freezing point constant is 6.8C/m. a What is the molecular formula of the compound? b What is its molecular weight to the nearest 0.1 g?
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
The Henry's law constant for the solubility of argon gas in water is 1.0103M/atm at 30C. (a) Express the constant in M/mm Hg. (b) If the partial pressure of argon gas at 30C is 693 mm Hg, what is the concentration (in M) of the dissolved argon gas at 30C? (c) How many grams of argon gas can be dissolved in 29 L of water at 693 mm Hg and 30C? (Ignore the partial pressure of water.)
Calculate the percent by mass of solute in each of the following solutions. 5.00 g of calcium chloride dissolved in 95.0 g of water 1.00 g of calcium chloride dissolved in 19.0 g of water 15.0 g of calcium chloride dissolved in 285 g of water 2.00 mg of calcium chloride dissolved in 0.0380 g of water