30. Which of the following organic compounds is the least soluble in water? A. H,CH,COCH,CH, B. CH,CH,OH C. CH,COH D. CH,CH,NH, 31. Which of the following molecular characteristics will be expected to increase the solubility of a simple solute in an aqueous solution? |-A low melting point Il - A high molecular surface area III- The presence of a polar group IV-A high boiling point A. Option I and II B. Option II and IV C. Options I, Il and III D. Options I, II, III and IV

30. Which of the following organic compounds is the least soluble in water? A. H,CH,COCH,CH, B. CH,CH,OH C. CH,COH D. CH,CH,NH, 31. Which of the following molecular characteristics will be expected to increase the solubility of a simple solute in an aqueous solution? |-A low melting point Il - A high molecular surface area III- The presence of a polar group IV-A high boiling point A. Option I and II B. Option II and IV C. Options I, Il and III D. Options I, II, III and IV

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The solubility limit of a solute at 20. °C and 1.0 atm is 13.8 g of solute per 1 L of water. What will MOST likely happen when 12.0 g of solute are added to 1 L of pure water and the solution is mixed well (at the same conditions)?
The CO2 gas sealed inside a carbonated beverage bottle has a pressure of 1.9atm. At this pressure, the solubility of CO, in water is 0.065g CO2/100 g H20. When the bottle is opened,the CO2 in the space above the liquid escapes, and the partial pressure of the CO2 falls to 2.3 mmHg, the value in the surrounding atmosphere of the room. Calculate the solubility of CO2 in the beverage at this new pressure, assuming no changes in temperature occur. Give the result in 2 sig. figs. 2.6 x 10^ -4 g of CO2 in 100 g of water.
At a particular temperature, the solubility of Kr in water is 0.060 M when the partial pressure is 0.90 atm. What partial pressure (in atm) of Kr would give a solubility of 0.090 M?
1. A 0.735 g of a covalent organic compound is dissolved in 15.00 g cyclohexane (freezing point = 6.20 °C). This solution freezes at -7.56°C. The Ki of cyclohexane =20.0°C.kg/mole. What is the molar mass of the solute?
Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?
Biphenyl, C1„H10. is a nonvolatile, nonionizing solute that is soluble in benzene, C,H,. At 25 °C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 18.0 g of biphenyl in 30.9 g of benzene? Polution Torr ||
A small amount of acetonitrile (CH3CN) is dissolved in a large amount of water. Imagine separating this process into the four stages sketched below. (These sketches show only a portion of the substances, so you can see the density and distribution of atoms and molecules in them.) C B CH3 CN H₂O Use these sketches to answer the questions in the table below. soln The enthalpy of solution AH is negative when CH3CN dissolves in water. Use this information to list the stages in order of increasing enthalpy. Would heat be absorbed or released if the system moved from Stage C to D? What force would oppose or favor the system moving from Stage C to D? Check all that apply. 0 absorbed released neither absorbed nor released none ionic bonding force covalent bonding force metal bonding force hydrogen-bonding force dipole force ion-dipole force dispersion force 0,0,... solution Ś
Six solutions are made by dissolving a certain amount of each of the six substances in 500. g water. If the freezing point of the each aqueous solution is the same, which substance is added to water in the largest amount, in grams? Assume all ionic compounds dissociate 100% to form ions in solution. ΔT = iKbmsolute ΔT = –iKfmsolute Select one: A. (NH4)2CO3 B. KCl C. The largest mass (g) of substance added is the same for two of the solutions. D.NH4Cl E. Insufficient information is provided. F. NaCl G. CH3OH H. MgCl2 The correct answer should be "B" or KCl, but I don't understand why
8, Q6
20 A 2.34 L aqueous solution of KQH contains 185 g of KOH. The solution has a density of 1.29 g/mL. Calculate the molarity (M), molality (m), and mass percent concentration of the solution. O Macmillan molarity: molality: mass percent: M m %
Hydrochloric acid is usually obtained as a 36% hydrochloric acid solution. If it is 13.42 M, what is the density of this solution? What is its molality? Density = g/mL Molality :
The solubility in acetone of molecular compound M is measured and found to be 80.2 2 that would contain 490. mg of M at this temperature. Be sure your answer has the correct unit symbol and number of significant digits. 10 0.0 X DO at at 25. °C. Calculate the volume of a saturated solution of M in acetone ola Ar 8: