PLEASE SHOW WORK WHEN POSSIBLE FOR ALL QUANTITATIVE PROBLEMS 1. A solution is su

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PLEASE SHOW WORK WHEN POSSIBLE FOR ALL QUANTITATIVE PROBLEMS

1. A solution is supersaturated when A. it is in contact with solute not dissolved B. addition of a crystal of the solute starts crystallization of excess solute C. it is formed from two completely miscible liquids D. it is a homogeneous mixture of the solute and solvent E. all of the statements given are true

2. Two liquids are immiscible when A. one liquid forms a dilute solution in the other B. a homogeneous mixture of the two forms when they are mixed C. one liquid forms an unsaturated solution in the other D. one liquid is insoluble in the other E. none of the above

3. Solubility of a gas in solution A. decreases as the pressure of the gas increases B. decreases as the temperature of the gas increases C. increases as the pressure of the gas increases D. both A and B E. both B and C

4. When solute and solvent are mixed, and solute-solvent attractions are stronger than solute-solute and solvent-solvent attractions, A. the entropy change is minimal B. heat is released C. heat is absorbed D. dissolution will not occur E. none of the above

5. An ionic solid such a sodium chloride dissolves in water because A. molecules of NaCl react with water molecules to form ions B. a nonelectrolyte forms C. the disorder of the system decreases as the two components, NaCl and H2O, change to one component, the solution D. the water molecules are attracted to the sodium and chloride ions by ion-dipole attractions and form hydrated ions E. none of these

6. Calculate the molarity of a solution containing 63 g of H3PO4 in 275.0 mL of solution.

7. Determine the molality of a solution containing 0.255 g of HNO3 in 212 g of H2O.

8. Calculate the mole fraction of methyl alcohol in a solution containing 51.0 g of C6H6 and 12.0 g of CH3OH.

9. Calculate the number of grams of NaOH in 3.00 L of a 0.390 M solution. 1

0. How many moles of HCl are present in a solution that has a total mass of 1000.0 g and percent solute of 49.0?

11. As the number of solute particles in a given volume increases, the vapor pressure of the solvent A. decreases B. increases C. is not changed D. increases exponentially E. decreases exponentially 2

12. A liquid boils when A. its vapor pressure is lower than the external pressure on its surface. B. its vapor pressure is lower than the molal boiling point constant. C. its vapor pressure is equal to the external pressure on its surface. D. its vapor pressure is higher than the molal boiling point contstant. E. none of the above

13. A solution was prepared by dissolving glucose (molar mass = 180.0 g/mol) in 100.0 g of acetic acid. The solution's boiling point was found to be 119.81C. The boiling point of pure acetic acid is 118.10C and the molal boiling-point elevation constant is 3.07C/molal. How many grams of glucose were used?

14. When a concentrated solution is in contact, by means of a semipermeable membrane, with a dilute solution of the same solute, the volume of the more concentrated solution A. decreases B. remains constant C. increases D. depends on the concentration E. none of the above

15. How many grams of glucose (molar mass = 180.0 g) must be dissolved in 300.0 mL of water at 25C to give an osmotic pressure of 9.05 atm?

16. Which of the following types of compounds would most likely be the best candidate for a detergent? A. a highly polar compound with no nonpolar character B. a nonpolar compound with no polar character C. a compound with an ionic group and a long nonpolar hydrocarbon chain D. all of these E. none of these

17. Which of the following solutions has the highest boiling point? A. 0.05 m I2 (aq) B. 0.10 m NaOH(aq) C. 0.10 m CaCl2 (aq) D. 0.20 m glycerin(aq) E. All of these have the same boiling point, because boiling point elevation is a colligative property.

18. A solution is prepared by dissolving 12.36 g of CaCl2 (an electrolyte, molar mass = 111 g) in 135g of H2O (molar mass = 18.0 g). The resulting solution has a density of 1.10 g/mL. Calculate the molarity of CaCl2 in the solution.

19. For many ionic compounds that dissolve with the absorption of heat, what is the driving force? A. higher energy state achieved B. more disordered state achieved C. no driving force D. both A and B E. none of the above

20. A student needs 5.00 mol of NH3 to perform an experiment. The only available source is a concentrated solution of NH3 that has a density of 0.900 g/mL and is 29.0 % NH3 by mass. What volume of NH3 solution should the student use?

21. If 0.900 L of a 10.00 M solution of Pb(NO3)2 is diluted to a volume of 1.50 L by adding water, what is the molarity of the resulting diluted solution?

22. The greater the __________ , the better the substance is at forming a solution that can conduct an electrical current. A. molecular mass B. dielectric constant C. degree of ionization D. both a and b E. both b and c

23. Consider a 0.700 M Al2(SO4)3 solution. This solution has a sulfate ion concentration of _____ . 3

24. A solution is made up of 44.4 percent ethyl alcohol, C2H5OH, and 55.6 percent H2O by mass. Its density is 0.936 g/mL. What is the molality of the alcohol in this solution?

25. The most important factor in determining the solubility of a solute in a solvent is/are the A. similar intermolecular forces. B. melting point of solute. C. temperature of the solvent. D. melting point of solute and boiling point of the solvent.

26. Which of the following liquids would be expected to be immiscible with liquid ammonia? A. H2O B. CH3OH C. CS2 D. N2H4 E. HCONH2

27. When naphthalene (a solid) is dissolved in benzene it causes freezing point lowering. boiling point elevation. vapor pressure elevation. 1 2 3 A. 1 only B. 2 only C. 1 and 2 only D. 2 and 3 only E. 1, 2, and 3

28. How many grams of KBr dissolved in 125 g of water is needed to raise the boiling point of water to 103.2 C?

29. Which of the following is not a colloid? A. fog B. air C. mayonnaise D. a gel E. milk

30. When 0.200 g of a high-molar-mass compound is dissolved in water to form 12.5 mL of solution at 25C, the osmotic pressure of the solution is found to be 1.10 x 10-3 atm. What is the molar mass of the compound?

31. Which of the following pairs of liquids are miscible with each other? CCl4 and C6H6 CS2 and CH2Cl2 HOCH2CH2OH and C6H14 1 2 3 A. 1 only B. 2 only C. 3 only D. 1 and 2 only E. 1 and 3 only 4

PLEASE SHOW WORK WHEN POSSIBLE FOR ALL QUANTITATIVE PROBLEMS

Explanation / Answer

Chegg rules allow tutors to answer only 4 questions per post. The quantitative problems starts from the number 6, so i will answer from there.

6) Molarity= mol/volume(L)

mol H3PO4= 63g/97.97g/mol= 0.643mol

M=0.643mol/0.275L= 2.34M

7) molality= mol of solute/kg solvent

mol HNO3= 0.255g/63g/mol= 4.05x10-3mol

molality=4.05x10-3mol/0.212kg= 0.019m

8) mole fraction= mol of solute/total moles

total moles= 51g/78g/mol + 12g/32g/mol= 0.654 mol + 0.375mol= 1.029mol

mole fraction CH3OH= 0.375mol/1.029mol= 0.364

9) 0.390M x 3L= moles

moles= 1.17mol

mass= 1.17mol x 40g/mol= 46.8 g

I will answer one more:

10) %solute=49%

This means that in 100g of solution there are 49g of solute, so, in 1000g of solution there are 490g of solute.

mole HCl= 490g/36.453g/mol= 13.44 mol

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