General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 11, Problem 11.119CHP
Interpretation Introduction
Interpretation:
The Kelvin temperature of given solution has to be calculated.
Concept introduction:
Osmotic pressure
The additional pressure that has to be given to solution in order to stop osmosis is called as osmotic pressure. Osmosis is the run of solvent into a solution by means of semipermeable membrane.
Osmotic pressure can be calculated by the equation,
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Northern cod produce proteins that protect their cells from damage caused by subzero temperatures. Measurements of the osmotic pressure for two
"antifreeze" proteins at 18°C yielded the data listed below. Use this information to calculate the molar mass for each of the proteins. Assume these
proteins are nonelectrolytes and use the value i = 1.
Please provide detailed solution and give the explanation of the concept
Calculate the osmotic pressure of a solution containing 19.25 mg of hemoglobin in 14.7 mL of solution at 35 °C. The molar mass of hemoglobin is 6.5 x 10^4 g/mol. Express your answer in atmospheres.
When 3.14 g of a nonelectrolyte solute is dissolved in water to make 325 mL of solution at 22 °C, the solution exerts an osmotic pressure of 849 torr.
What is the molar concentration of the solution? Moles of a solute? Molar mass of solute?
Chapter 11 Solutions
General Chemistry: Atoms First
Ch. 11.2 - Arrange the following compounds in order of their...Ch. 11.2 - Which would you expect to have the larger (more...Ch. 11.3 - Prob. 11.3PCh. 11.3 - Prob. 11.4PCh. 11.3 - Prob. 11.5PCh. 11.3 - Prob. 11.6PCh. 11.3 - Prob. 11.7PCh. 11.3 - Prob. 11.8PCh. 11.3 - Prob. 11.9PCh. 11.3 - Prob. 11.10P
Ch. 11.4 - Prob. 11.11PCh. 11.4 - Prob. 11.12PCh. 11.6 - Prob. 11.13PCh. 11.6 - How many grams of NaBr must be added to 250 g of...Ch. 11.6 - The following diagram shows a close-up view of...Ch. 11.6 - (a) What is the vapor pressure in mm Hg of a...Ch. 11.6 - The following phase diagram shows part of the...Ch. 11.7 - What is the normal boiling point in C of a...Ch. 11.7 - What is the freezing point in C of a solution...Ch. 11.7 - Assuming complete dissociation, what is the...Ch. 11.7 - When 9.12 g of HCl was dissolved in 190 g of...Ch. 11.7 - The following phase diagram shows a close-up view...Ch. 11.8 - What osmotic pressure in atmospheres would you...Ch. 11.8 - A solution of an unknown substance in water at 300...Ch. 11.9 - A solution of 0.250 g of naphthalene (mothballs)...Ch. 11.9 - What is the molar mass of sucrose (table sugar) if...Ch. 11.10 - What is the difference between a dialysis membrane...Ch. 11 - The following phase diagram shows part of the...Ch. 11 - Prob. 11.30CPCh. 11 - The following diagram shows a close-up view of...Ch. 11 - Prob. 11.32CPCh. 11 - Prob. 11.33CPCh. 11 - Prob. 11.34CPCh. 11 - A phase diagram of temperature versus composition...Ch. 11 - The following phase diagram shows a very small...Ch. 11 - Prob. 11.38SPCh. 11 - Prob. 11.39SPCh. 11 - Prob. 11.40SPCh. 11 - Prob. 11.41SPCh. 11 - Prob. 11.42SPCh. 11 - Prob. 11.43SPCh. 11 - Prob. 11.44SPCh. 11 - Prob. 11.45SPCh. 11 - Prob. 11.46SPCh. 11 - Prob. 11.47SPCh. 11 - Prob. 11.48SPCh. 11 - Prob. 11.49SPCh. 11 - Prob. 11.50SPCh. 11 - Prob. 11.51SPCh. 11 - Prob. 11.52SPCh. 11 - Which of the following solutions has the higher...Ch. 11 - What is the mass percent concentration of the...Ch. 11 - Prob. 11.55SPCh. 11 - Prob. 11.56SPCh. 11 - Prob. 11.57SPCh. 11 - Prob. 11.58SPCh. 11 - Prob. 11.59SPCh. 11 - Prob. 11.60SPCh. 11 - Prob. 11.61SPCh. 11 - Prob. 11.62SPCh. 11 - Prob. 11.63SPCh. 11 - Prob. 11.64SPCh. 11 - Prob. 11.65SPCh. 11 - Prob. 11.66SPCh. 11 - Prob. 11.67SPCh. 11 - Prob. 11.68SPCh. 11 - Look at the solubility graph in Figure 11.6, and...Ch. 11 - Vinyl chloride (H2CCHCl), the starting material...Ch. 11 - Prob. 11.71SPCh. 11 - Prob. 11.72SPCh. 11 - Prob. 11.73SPCh. 11 - Sulfur hexafluoride, which is used as a...Ch. 11 - Prob. 11.75SPCh. 11 - Prob. 11.76SPCh. 11 - Prob. 11.77SPCh. 11 - Draw a phase diagram showing how the phase...Ch. 11 - Prob. 11.79SPCh. 11 - Prob. 11.80SPCh. 11 - Prob. 11.81SPCh. 11 - What is the boiling point in C of each of the...Ch. 11 - Prob. 11.83SPCh. 11 - Prob. 11.84SPCh. 11 - The vant Hoff factor for KCl is i = 1.85. What is...Ch. 11 - Heptane (C7H16) and octane (C8H18) are...Ch. 11 - Prob. 11.87SPCh. 11 - Acetone, C3H6O, and ethyl acetate, C4H8O2, are...Ch. 11 - The industrial solvents chloroform, CHCl3, and...Ch. 11 - What is the mole fraction of each component in the...Ch. 11 - Prob. 11.91SPCh. 11 - Prob. 11.92SPCh. 11 - Prob. 11.93SPCh. 11 - A solution of citric acid, C6H8O7, in 50.0 g of...Ch. 11 - What is the normal boiling point in C of ethyl...Ch. 11 - Prob. 11.96SPCh. 11 - Prob. 11.97SPCh. 11 - Prob. 11.98SPCh. 11 - Prob. 11.99SPCh. 11 - When salt is spread on snow-covered roads at 2 C,...Ch. 11 - Prob. 11.101SPCh. 11 - Prob. 11.102SPCh. 11 - Prob. 11.103SPCh. 11 - Prob. 11.104SPCh. 11 - Prob. 11.105SPCh. 11 - Prob. 11.106SPCh. 11 - Prob. 11.107SPCh. 11 - Prob. 11.108CHPCh. 11 - Prob. 11.109CHPCh. 11 - Prob. 11.110CHPCh. 11 - Silver chloride has a solubility of 0.007 mg/mL in...Ch. 11 - Prob. 11.112CHPCh. 11 - Prob. 11.113CHPCh. 11 - Prob. 11.114CHPCh. 11 - Prob. 11.115CHPCh. 11 - Prob. 11.116CHPCh. 11 - Prob. 11.117CHPCh. 11 - Rubbing alcohol is a 90 mass % solution of...Ch. 11 - Prob. 11.119CHPCh. 11 - Prob. 11.120CHPCh. 11 - What is the vant Hoff factor for K2SO4 in an...Ch. 11 - If the vant Hoff factor for LiCl in a 0.62 m...Ch. 11 - Prob. 11.123CHPCh. 11 - Prob. 11.124CHPCh. 11 - Many acids are partially dissociated into ions in...Ch. 11 - Prob. 11.126CHPCh. 11 - Prob. 11.127CHPCh. 11 - A solution of LiCl in a mixture of water and...Ch. 11 - Prob. 11.129CHPCh. 11 - Prob. 11.130CHPCh. 11 - Prob. 11.131CHPCh. 11 - Prob. 11.132CHPCh. 11 - Prob. 11.133CHPCh. 11 - Prob. 11.134CHPCh. 11 - Prob. 11.135CHPCh. 11 - A solution prepared by dissolving 100.0 g of a...Ch. 11 - Treatment of 1.385 g of an unknown metal M with an...Ch. 11 - A compound that contains only C and H was burned...Ch. 11 - Prob. 11.139MPCh. 11 - When 8.900 g of a mixture of an alkali metal...Ch. 11 - Prob. 11.141MP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 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.arrow_forwardFor 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 = 70Carrow_forwardFor 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 = 80Carrow_forward
- Simple acids such as formic acid, HCOOH, and acetic acid, CH3COOH, are very soluble in water; however, fatty acids such as stearic acid, CH3(CH2)16COOH, and palmitic acid, CH3(CH2)14COOH, are water-insoluble. Based on what you know about the solubility of alcohols, explain the solubility of these organic acids.arrow_forwardStarch contains CC, CH, CO, and OH bonds. Hydrocarbons have only CC and CH bonds. Both starch and hydrocarbons can form colloidal dispersions in water. Which dispersion is classified as hydrophobic? Which is hydrophilic? Explain briefly.arrow_forwardCalculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.arrow_forward
- Fluoridation of city water supplies has been practiced in the United States for several decades. It is done by continuously adding sodium fluoride to water as it comes from a reservoir. Assume you live in a medium-sized city of 150,000 people and that 660 L (170 gal) of water is used per person per day. What mass of sodium fluoride (in kilograms) must be added to the water supply each year (365 days) to have the required fluoride concentration of 1 ppm (part per million)that is, 1 kilogram of fluoride per 1 million kilograms of water? (Sodium fluoride is 45.0% fluoride, and water has a density of 1.00 g/cm3.)arrow_forwardThe dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?arrow_forwardInsulin 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?arrow_forward
- A compound has a solubility in water of 250 mg/L at 25C. Should this compound be characterized as a soluble or insoluble compound at 25C?arrow_forwardIn the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.arrow_forwardWhat is the osmotic pressure of a 4.5 FL OZ solution containing 30.6 g of fructose (C6H12O6) at 40 °F. Osmotic pressure is 29.2 atm. Explain why.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY