Answered: Determine the concentration in μg/m³ of…

Determine the concentration in μg/m³ of 10 ppm, (by volume) of trichloroethylene (TCE) (C₂HCl) at standard conditions (0°C and 1 atm).

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter1: Basic Concepts Of Chemistry

Section: Chapter Questions

Problem 49RGQ: Fluoridation of city water supplies has been practiced in the United States for several decades. It...

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6-20 Give a familiar example of solutions of each of these types: (a) Liquid in liquid (b) Solid in liquid (c) Gas in liquid (d) Gas in gas
6-19 In each of the following, tell whether the solutes and solvents are gases, liquids, or solids. (a) Bronze (see Chemical Connections 2E) (b) Cup of coffee (c) Car exhaust (d) Champagne
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Oxygen gas in water with P = 1 atm and T = 10C Oxygen gas in water with P = 1 atm and T = 20C b. Nitrogen gas in water with P = 2 atm and T = 50C Nitrogen gas in water with P = 1 atm and T = 70C c. Table salt in water with P = 1 atm and T = 40C Table salt in water with P = 1 atm and T = 70C d. Table sugar in water with P = 3 atm and T = 30C Table sugar in water with P = 1 atm and T = 80C
Insulin is a hormone responsible for the regulation of glucose levels in the blood. An aqueous solution of insulin has an osmotic pressure of 2.5 mm Hg at 25C. It is prepared by dissolving 0.100 g of insulin in enough water to make 125 mL of solution. What is the molar mass of insulin?
6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.
6-60 Predict which of these covalent compounds is soluble in water. (a) C2H6 (b) CH3OH (c) HF (d) NH3 (e) CCI4
Calculate what volume of concentrated hydrochloric acid, 37.2 % (w/w), that you would need to produce a 3.00 L stock of 2.00 mol dm–3 HCl. [Mr (HCl) = 36.5 g mol–1; density of 37.2% HCl = 1.19 g mL–1]
Seawater consists of many important elements in the form of salts dissolved in the water. At 25°C the mass percentage of salts in seawater will total 3.5% m/m. The density of seawater at this temperature and salt percentage is 1.024 kg/L. Study the chart and answer the questions below: 1. The chart assumes 1000.0 g of seawater. What volume, Vsoln (L), does this correspond to at 25 °C? 2. The diagram claims that chloride ions make up 55% m/m of all salt ions. Confirm this number. if possible, I would like handwritten answers with calculations. Thanks :)
At 20 °C, an aqueous solution of NaCl was prepared by dissolving 11.44 g NaCl (Molar Mass = 58.44) in 45.76 g H20 (Molar Mass 18.02). The density of the NaCl solution (at 20 °C) is 1.1478 g/mL. Which of the following statements is consistent with the data given? %3D The volume of the solution is 57.20 mL. The solution contains 25.00% NaCl by mass. C The molality of the solution is 3.423 molal. The molarity of the solution is 3.929 M NaCl.
A mystery liquid with a density of 1.22 g/mL has a boiling point of 132.5 oC. (a) A sample of 37.8 grams of NaCl is dissolved in a 420. mL of this liquid. The boiling point of the solution is 134.7 oC. What is the boiling point elevation, DTb? What is the boiling point elevation constant of this liquid? DTb = Kb = A sample of 19.54 g of glucose (180.16 g/mol) is dissolved in 150. mL of this same liquid. What is its boiling point of this solution?
Wastewater from a cement factory contains 0.25 g of Ca²⁺ ion and 0.056 g of Mg²⁺ ion per 100.0 L of solution. The solu-tion density is 1.001 g/mL. Calculate the Ca²⁺ and Mg²⁺ con-centrations in ppm (by mass).