ࡱ> npmy @bjbj 5F{{RFFFFFZZZ8$dZ\t(BBB[[[[[[[$^`~\9Fggg\FFBBV\gFBFB[g[U[BΝ^W8[l\0\W@aT@ap[@aF[PvTD+<\\I\gggg@a : Pretest 4 Chapters: 15, 16 and 17 Directions: Answer each of the following questions in complete sentences where appropriate. Be sure to show all of your work and report your answers to the correct number of significant figures. Question 1. A typical air sample in the lungs contains oxygen at 100 mm Hg, nitrogen at 573 mm Hg, carbon dioxide at 40 mm Hg, and water vapor at 47 mm Hg. What is the total pressure of air in the lungs? Question 2. A 35.20 g sample of metal is heated to 100.0 C and is then placed in a calorimeter containing 42.5 g of water at 19.2 C. If the final temperature of the metal and the water is 29.5 C, what is the specific heat of the solid? Assume no heat loss; the specific heat of water is 4.184 J/g C. Question 3. Calculate the amount of heat in calories required to vaporize 2.00 g of acetone, C3H6O, at 25 C. The heat of vaporization is 31.0 kJ/mol; the heat of fusion is 5.69 kJ/mol. Question 4. Identify each as an ionic, molecular, network or metallic solid. silicon dioxide, SiO2 ________________________ titanium tetrachloride, TiCl4 ________________________ cesium chloride ________________________ Question 5. Name the types of intermolecular forces for each molecule: ethanol, CH3CH2CH2OH ____________________________________ silicon dioxide, SiO2 ____________________________________ c. carbon monoxide, CO ____________________________________ Question 6. In hexane, C6H14, the intermolecular attraction is less than that in isopropyl alcohol, C3H7OH. Predict which liquid has the higher value for each of the following: vapor pressure ________________________ viscosity ________________________ boiling point ________________________ surface tension ________________________ Question 7. A tincture of iodine is prepared with 0.10 g I2 and 10.0 mL ethyl alcohol, density of ethyl alcohol solution is 1.064 g/mL. What is the solute, and what is the solvent? solute _________________ solvent ___________________ Question 8. Potassium nitrate has a solubility of 34 g KNO3 in 100 g H2O at 20 C. State if each of the following forms an unsaturated, saturated, or supersaturated solution. 34 g KNO3 and 200 g H2O __________________ 1.01 x 1023 molecules KNO3 and 50 g H2O __________________ Question 9. Would the following pairs of liquids be miscible or immiscible? a. carbon tetrafluoride, CF4 and chloroform CHCl3 _________________ b. carbon tetrafluoride, CF4, and water _________________ Question 10. What mass of solution containing 6.50% sodium sulfate, by mass contains 1.50g of sodium sulfate? Question 11. What is the molarity of a solution that contains 324.0 mg of acetic acid and 25.00 mL of solution? Question 12. If 10.00 mL of the solution from question 11 is diluted to 50.00 mL, what is the new molarity? Question 13. What mass in gram of potassium sulfite is needed to prepare 150.00 mL of a solution that has a molarity of 0.250 M potassium ions? Question 14. A solution is prepared with 70.0 g nitric acid and 130.0 g water. It has a density 1.21 g/mL. What is the mass percent of nitric acid solution? What is its molarity? Question 15. A flask contains 47.5 mL of 0.150 M calcium hydroxide solution. How many liters of a 0.450 M sodium carbonate solution are required to completely react? Question 16. A 20.00 mL aliquot of a 0.1500 M nickel(II) chloride solution reacts with 25.00 mL aliquot of a 0.2000 M sodium hydroxide solution to produce solid nickel(II) hydroxide and aqueous sodium chloride. a. How many grams of nickel(II) hydroxide are produced? b. What is the molarity of all ions that remain in the solution at the end of the reaction? Assume a 100% yield for nickel(II) hydroxide. Question 17. A 355 mL sample of hydrochloric acid solution reacts with excess magnesium to produce 4.20 L hydrogen gas measured at 745 mm Hg and 35 C. What is the molarity of the hydrochloric acid solution? Question 18. Consider the reaction of potassium hydroxide and nitrous acid. Calculate the mL of 0.122 M potassium hydroxide required to neutralize 36.0 mL of 0.250 M nitrous acid. Question 19. For each reaction identify the acid, base, conjugate acid, and conjugate base. H2CO3 (aq) + H2O (l) D H3O+(aq) + HCO3- (aq) HCN (aq) + NO2- (aq) D CN-(aq) HNO2 (aq) Question 20. Name each acid. Then identify each acid as monoprotic, diprotic, or triprotic. a. H2S (aq) ____________________________ ______________ b. H2SO3 (aq) ____________________________ ______________ c. H3PO4 (aq) ____________________________ ______________ Question 21. Write the balanced chemical, total ionic, and net ionic equations for the following reactions: lead metal + perchloric acid ( __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ nitric acid + lithium hydroxide ( __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ aqueous ammonia + hydrobromic acid ( __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ Question 22. If 38.2 mL of 0.163 M potassium hydroxide react with 25.0 mL of 0.134 M sulfuric acid solution, how many grams of potassium sulfate can be formed? Question 23. A vinegar solution has a [H3O+] of 2.0 x 10-3 M at 25 C. What is the [OH-] of the vinegar solution? Is the solution acidic, basic, or neutral? Question 24. What is the pH and pOH of a solution prepared by dissolving 2.5 g hydrochloric acid, HCl, in water to make 425 mL of solution?     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