Describe the difference between solvation of ionic compounds and solvation of covalent compounds, For each type of compound: describe what forces hold the compound together • describe how and why they dissociate (come apart) in water.

Describe the difference between solvation of ionic compounds and solvation of covalent compounds, For each type of compound: describe what forces hold the compound together • describe how and why they dissociate (come apart) in water.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 4ALQ

See similar textbooks

Similar questions

When KNO3 is dissolved in water, the resulting solution is significantly colder than the water was originally. (a) Is the dissolution of KNO3 an endothermic or an exothermic process? (b) What conclusions can you draw about the intermolecular attractions involved in the process? (c) Is the resulting solution an ideal solution?
Which of the following salts, Li2SO4 or Cs2SO4, is expected to have the more exothermic enthalpy of hydration?
Will red blood cells crenate, hemolyze, or remain unaffected when placed in each of the solutions in Problem 8-107?
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?
Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?
An aqueous solution of LiX is prepared by dissolving 3.58 g of the electrolyte in 283 mL of H2O(d=1.00g/mL). The solution freezes at -1.81C. What is X-? (Assume complete dissociation of LiX to Li+ and X-.
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?
In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
Acetylene can be made by reacting calcium carbide with water. CaC2(s) + 2 H2O() C2H2(g) + Ca(OH)2(aq) Assume that you place 2.65 g CaC2 in excess water and collect the acetylene over water. The volume of the acetylene and water vapor is 795 mL at 25.0 C and a barometric pressure of 735.2 mmHg. Calculate the percent yield of acetylene. The vapor pressure of water at 25 C is 23.8 mmHg.
An aqueous solution of M2O is prepared by dissolving 10.91 g of the electrolyte in 435 mL of H2O(d=1.00g/mL). The solution freezes at -4.68C. What is M+? (Assume complete dissociation of M2O to M+ and O2-.)
Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H2O. What is the mole fraction of HCl in concentrated hydrochloric acid? What is the molal concentration of HCl?
Caffeine is made up of 49.5% C, 5.2% H, 16.5% O, and 28.9% N. A solution made up of 8.25 g of caffeine and 100.0 mL of benzene (d=0.877g/mL) freezes at 3.03C. Pure benzene (k f =5.10C/m) freezes at 5.500C. What are the simplest and molecular formulas for caffeine?