Intro to Chem Chpts 12-14
80) A 50.0 mL solution of sodium chloride, NaCl (58.44 g/mol), weighing 50.320 g, is evaporated to dryness. If the white solute residue has a mass of 0.453 g, what is the mass/mass percent concentration and molarity of the saline solution? A) 0.900% and 0.155 M B) 0.900% and 0.172 M C) 0.900% and 0.180 M D) 0.906% and 0.155 M E) 0.906% and 0.180 M
A) 0.900% and 0.155 M
89)---1) What is the approximate concentration of fluoride in fluoridated water? A) 1 ppm B) 10 ppm C) 100 ppm D) 1000 ppm E) 10,000 ppm
A) 1 ppm
59) What is the molarity of a hydrochloric acid solution prepared by diluting 200.0 mL of 0.500 M HCl to a total volume of 1.00 L? A) 0.100 M B) 0.200 M C) 0.250 M D) 1.00 M E) 2.50 M
A) 0.100 M
48) What is the molarity of a saline solution that contains 0.900 g NaCl (58.44 g/mol) dissolved in 100.0 mL of solution? A) 0.154 M B) 0.527 M C) 1.54 M D) 1.90 M E) 5.27 M
A) 0.154 M
61) What is the molarity of a sulfuric acid solution if 30.00 mL of H2SO4 is required to neutralize 0.840 g of sodium hydrogen carbonate (84.01 g/mol)? H2SO4(aq) + 2 NaHCO3(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g) A) 0.167 M B) 0.300 M C) 0.333 M D) 0.500 M E) 0.667 M
A) 0.167 M
62) What is the molarity of a nitric acid solution if 25.00 mL of HNO3 is required to neutralize 0.500 g of calcium carbonate (100.09 g/mol)? 2 HNO3(aq) + CaCO3(s) → Ca(NO3)2(aq) + H2O(l) + CO2(g) A) 0.200 M B) 0.250 M C) 0.400 M D) 0.500 M E) 0.800 M
A) 0.200 M
70) If 25.0 mL of 0.100 M lithium iodide reacts completely with aqueous mercury(II) nitrate, what is the mass of HgI2 (454.39 g/mol) precipitate? 2 LiI(aq) + Hg(NO3)2(aq) → HgI2(s) + 2 LiNO3(aq) A) 0.568 g B) 1.14 g C) 2.27 g D) 2.75 g E) 5.50 g
A) 0.568 g
36) Which of the following is not a unit factor related to a 15.0% aqueous solution of potassium iodide, KI? A) 15.0 g KI / 85.0 g of water B) 85.0 g of water / 100 g solution C) 85.0 g of water / 15.0 g KI D) 100 g solution / 85.0 g of water E) 15.0 g KI / 100 g solution
A) 15.0 g KI / 85.0 g of water
6) How many kJ of heat are needed to completely melt 95.3 g of copper metal, given that the metal is at its melting point? The heat of fusion for this metal is 13.1 kj/mole. A) 19.6 B) 43.0 C) 1250 D) 0.114 E) none of the above
A) 19.6
42) Permanent antifreeze contains ethylene glycol dissolved in water. What is the mass of ethylene glycol dissolved in 5.00 kg of a 40.0% solution? A) 2.00 kg B) 3.33 kg C) 7.5 kg D) 12.5 kg E) 200 kg
A) 2.00 kg
34) Which of the following is not a unit factor related to a 5.00% aqueous solution of lithium chloride, LiCl? A) 5.00 g LiCl / 95.0 g solution B) 95.0 g water / 5.00 g LiCl C) 5.00 g LiCl / 95.0 g water D) 100 g solution / 5.00 g LiC E) 95.0 g water / 100 g solution
A) 5.00 g LiCl / 95.0 g solution
48) If 10.0 mL of 0.100 M HCl is titrated with 0.200 M NaOH, what volume of sodium hydroxide solution is required to neutralize the acid? HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) A) 5.00 mL B) 10.0 mL C) 20.0 mL D) 40.0 mL E) 80.0 mL
A) 5.00 mL
52) What is the mass of barium hydroxide (171.35 g/mol) dissolved in 0.500 L of 0.100 M Ba(OH)2 solution? A) 8.57 g B) 17.1 g C) 85.7 g D) 171 g E) 857 g
A) 8.57 g
6) Which of the following illustrates the like dissolves like rule for two liquids? A) A polar solute is miscible with a nonpolar solvent. B) A polar solute is immiscible with a polar solvent. C) A nonpolar solute is miscible with a polar solvent. D) A nonpolar solute is immiscible with a nonpolar solvent. E) none of the above
A) A polar solute is miscible with a nonpolar solvent.
21) When sufficient quantity of heat has been added to reach the boiling point of a solution, what happens to any additional heat added? A) Additional heat is used to evaporate the liquid as the process is endothermic and requires continued input of energy. B) Additional heat raises the temperature of the liquid which in turn increases the rate at which boiling occurs. C) Additional heat lowers the intermolecular forces of the liquid which in turn increases the volatility of the liquid. D) Additional heat alters the viscosity and the surface tension of the liquid which raises the vapor pressure and increases the boiling point which is why you must continually heat the solution. E) None of the above are correct statements.
A) Additional heat is used to evaporate the liquid as the process is endothermic and requires continued input of energy.
103) Hydrochloric acid is a strong acid and acetic acid is a weak acid. Which of the following correctly portrays aqueous solutions of the two acids? A) HCl(aq) and HC2H3O2(aq) B) H+(aq) + Cl-(aq) and HC2H3O2(aq) C) HCl(aq) and H+(aq) + C2H3O2-(aq) D) H+(aq) + Cl-(aq) and H+(aq) + C2H3O2-(aq) E) none of the above
B) H+(aq) + Cl-(aq) and HC2H3O2(aq)
29) Gaseous water vapor can frost the windows of a car on a cold morning. This process of a gas changing directly into a solid is known as: A) deposition. B) melting. C) condensation. D) sublimation. E) none of the above
A) deposition.
34) Which intermolecular force is present in all molecules and atoms? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
A) dispersion forces
35) Which intermolecular force is due to the formation of an instantaneous dipole? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
A) dispersion forces
38) Which intermolecular force increases with increasing molar mass? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
A) dispersion forces
49) Which intermolecular forces are found in CCL4? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
A) dispersion forces
50) Which intermolecular forces are found in CO2? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) dispersion forces and dipole-dipole forces E) none of the above
A) dispersion forces
51) What types of forces exist between I2 molecules? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) ion-dipole forces E) none of the above
A) dispersion forces
37) In the following reaction, which reactant is a Brønsted-Lowry acid? Na2HPO4(aq) + H2CO3(aq) → NaH2PO4(aq) + NaHCO3(aq) A) Na2HPO4 B) H2CO3 C) NaH2PO4 D) NaHCO3 E) none of the above
B) H2CO3
24) When fructose crystals, C6H12O6, dissolve in water, which of the following is formed in solution? A) hydrated clusters of C6H12O6 B) hydrated clusters of CO2 C) hydrated clusters of H2O D) hydrated clusters of H2CO3 E) none of the above
A) hydrated clusters of C6H12O6
72) Which of the following reactions represents the ionization of water? A) H2O + H2O → 2 H2 + O2 B) H2O + H2O → H3O+ + OH- C) H2O + H3O+ → H3O+ + H2O D) H3O+ + OH- → H2O + H2O E) none of the above
B) H2O + H2O → H3O+ + OH-
24) What acid and base are neutralized to give sodium bromide salt? A) HCl(aq) and NaOH(aq) B) HBr(aq) and NaOH(aq) C) HBr(aq) and NaBr(aq) D) HOH(aq) and NaBr(aq) E) none of the above
B) HBr(aq) and NaOH(aq)
13) Which of the following is an example of an Arrhenius acid? A) NH4C2H3O2(aq) B) HC2H3O2(aq) C) KC2H3O2(aq) D) all of the above E) none of the above
B) HC2H3O2(aq)
31) In the following reaction, which reactant is a Brønsted-Lowry acid? NaHS(aq) + HCN(aq) → NaCN(aq) + H2S(aq) A) NaHS B) HCN C) NaCN D) H2S E) none of the above
B) HCN
33) In the following reaction, which reactant is a Brønsted-Lowry acid? KC2H3O2(aq) + HCN(aq) → HC2H3O2(aq) + KCN(aq) A) KC2H3O2 B) HCN C) HC2H3O2 D) KCN E) none of the above
B) HCN
25) What acid and base are neutralized to give lithium fluoride salt? A) HCl(aq) and LiOH(aq) B) HF(aq) and LiOH(aq) C) HF(aq) and LiF(aq) D) HOH(aq) and LiF(aq) E) none of the above
B) HF(aq) and LiOH(aq)
23) When vitamin C crystals, C6H8O6, dissolve in water, which of the following is formed in solution? A) hydrated clusters of C6H8O6 B) hydrated clusters of CO2 C) hydrated clusters of H2O D) hydrated clusters of H2CO3 E) none of the above
A) hydrated clusters of C6H8O6
22) When citric acid crystals, C6H8O7, dissolve in water, which of the following is formed in solution? A) hydrated clusters of C6H8O7 B) hydrated clusters of CO2 C) hydrated clusters of H2O D) hydrated clusters of H2CO3 E) none of the above
A) hydrated clusters of C6H8O7
26) What acid and base are neutralized to give potassium nitrate salt? A) HCl(aq) and KOH(aq) B) HNO3(aq) and KOH(aq) C) HNO3(aq) and KNO3(aq) D) HOH(aq) and KNO3(aq) E) none of the above
B) HNO3(aq) and KOH(aq)
28) In the following reaction, which reactant is a Brønsted-Lowry base? HCl(aq) + KHS(aq) → KCl(aq) + H2S(aq) A) HCl B) KHS C) KCl D) H2S E) none of the above
B) KHS
101) Which of the following in aqueous solution is a strong electrolyte? A) H3PO4(aq) B) KOH(aq) C) PbCl2(s) D) all of the above E) none of the above
B) KOH(aq)
19) Which of the following is an example of an Arrhenius base? A) KCl(aq) B) KOH(aq) C) KNO3(aq) D) all of the above E) none of the above
B) KOH(aq)
105) Lithium nitrate is a soluble salt and silver iodide is a very slightly soluble salt. Which of the following correctly portrays aqueous solutions of the two salts? A) LiNO3(aq) and AgI(s) B) Li+(aq) + NO3-(aq) and AgI(s) C) LiNO3(aq) and Ag+(aq) + I-(aq) D) Li+(aq) + NO3-(aq) and Ag+(aq) + I-(aq) E) none of the above
B) Li+(aq) + NO3-(aq) and AgI(s)
26) When sodium bromide, NaBr, dissolves in water, which of the following is formed in aqueous solution? A) Na+ ----H-O I H B) Na+ ----O-H I H C) Br- ----O-H I H D) all of the above E) none of the above
B) Na+ ----O-H I H
104) Sodium hydroxide is a strong base and ammonium hydroxide is a weak base. Which of the following correctly portrays aqueous solutions of the two bases? A) NaOH(aq) and NH4OH(aq) B) Na+(aq) + OH-(aq) and NH4OH(aq) C) NaOH(aq) and NH4+(aq) + OH-(aq) D) Na+(aq) + OH-(aq) and NH4+(aq) + OH-(aq) E) none of the above
B) Na+(aq) + OH-(aq) and NH4OH(aq)
30) In the following reaction, which reactant is a Brønsted-Lowry base? H2CO3(aq) + Na2HPO4(aq) → NaHCO3(aq) + NaH2PO4(aq) A) H2CO3 B) Na2HPO4 C) NaH2PO4 D) NaHCO3 E) none of the above
B) Na2HPO4
111) Which of the following solutions is amphiprotic? A) H3PO4(aq) B) Na2HPO4(aq) C) Na3PO4(aq) D) all of the above E) none of the above
B) Na2HPO4(aq)
35) In the following reaction, which reactant is a Brønsted-Lowry acid? NaHCO3(aq) + NaH2PO4(aq) → Na2HPO4(aq) + H2CO3(aq) A) NaHCO3 B) NaH2PO4 C) Na2HPO4 D) H2CO3 E) none of the above
B) NaH2PO4
110) Which of the following solutions is amphiprotic? A) H2CO3(aq) B) NaHCO3(aq) C) Na2CO3(aq) D) all of the above E) none of the above
B) NaHCO3(aq)
62) Which atomic solid has the highest melting point? A) Cu B) Si C) Xe D) Fe E) not enough information
B) Si
96) If an unknown solution is a poor conductor of electricity, which of the following must be true? A) The solution is highly ionized. B) The solution is slightly ionized. C) The solution is highly reactive. D) The solution is slightly reactive. E) none of the above
B) The solution is slightly ionized.
117) Which of the following is true if the pH of a solution increases from 2 to 5? A) [ H+ ] increases B) [ H+ ] decreases C) Kw increases D) Kw decreases E) none of the above
B) [ H+ ] decreases
20) Apply the like dissolves like rule to predict which of the following vitamins is soluble in water. A) retinol, C20H30O B) ascorbic acid, C6H8O6 C) calciferol, C27H44O D) α-tocopherol, C29H50O2 E) none of the above
B) ascorbic acid, C6H8O6
120) Beakers W, X, Y, and Z contain either aqueous HCl, HNO3, H2SO4, or HC2H3O2. Which beaker contains acetic acid if the light bulb glows brightly when testing the conductivity of beakers W, Y, and Z? A) beaker W B) beaker X C) beaker Y D) beaker Z E) all of the above
B) beaker X
40) Which of the following indicators is yellow in an acidic solution and blue in a basic solution? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
B) bromthymol blue
43) Which of the following indicators is green at pH 7? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
B) bromthymol blue
12) You can increase the vapor pressure of a liquid by: A) increasing temperature. B) increasing the viscosity. C) establishing dynamic equilibrium. D) using a nonvolatile compound. E) all of the above
A) increasing temperature.
3) Yeast and sugar are added to champagne to give the sparkle of carbonation. Under what conditions is carbon dioxide gas most soluble? A) low temperature, high pressure B) low temperature, low pressure C) high temperature, low pressure D) high temperature, high pressure E) none of the above
A) low temperature, high pressure
39) Which of the following indicators is red in an acidic solution and yellow in a basic solution? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
A) methyl red
42) Which of the following indicators is orange at pH 5? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
A) methyl red
57) Dry ice (solid C) is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid
A) molecular solid
119) Which of the following is true if the hydrogen ion concentration of an aqueous solution decreases? A) pH increases B) pH decreases C) Kw increases D) Kw decreases E) none of the above
A) pH increases
21) Apply the like dissolves like rule to predict which of the following vitamins is insoluble in water. A) retinol, C20H30O B) thiamine, C12H17N4OS C) niacinamide, C6H6N2O D) pyridoxine, C8H11NO3 E) cyanocobalamin, C63H88CoN14O14P
A) retinol, C20H30O
7) If stomach digestive juice has a pH of 1, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic
A) strongly acidic
2) Which of the following is a general property of an acidic solution? A) tastes sour B) feels slippery C) turns litmus paper blue D) pH greater than 7 E) none of the above
A) tastes sour
115) What is the pH of an aqueous solution whose hydrogen ion concentration is 1 M? A) -1 B) 0 C) 1 D) 10 E) none of the above
B) 0
81) What is the hydrogen ion concentration in stomach acid that registers a pH of 2 on a strip of pH paper? A) 0.02 M B) 0.01 M C) 0.2 M D) 0.1 M E) 2 M
B) 0.01 M
60) What is the molarity of a hydrochloric acid solution if 20.00 mL of HCl is required to neutralize 0.424 g of sodium carbonate (105.99 g/mol)? 2 HCl(aq) + Na2CO3(aq) → 2 NaCl(aq) + H2O(l) + CO2(g) A) 0.100 M B) 0.200 M C) 0.300 M D) 0.400 M E) 0.500 M
B) 0.200 M
60) What is the molarity of a hydrochloric acid solution prepared by diluting 500.0 mL of 1.00 M HCl to a total volume of 2.50 L? A) 0.100 M B) 0.200 M C) 0.500 M D) 2.00 M E) 5.00 M
B) 0.200 M
64) What is the molarity of a sodium hydroxide solution if 35.00 mL of NaOH is required to neutralize 1.555 g of KHP, that is KHC8H4O4 (204.23 g/mol)? KHC8H4O4(aq) + NaOH(aq) → KNaC8H4O4(aq) + H2O(l) A) 0.109 M B) 0.218 M C) 0.267 M D) 0.435 M E) 3.75 M
B) 0.218 M
51) Which of the following unit factors is not related to a 0.250 M KOH solution? A) 1000 mL solution / 0.250 mol KOH B) 0.250 mol KOH / 1000 mL water C) 0.250 mol KOH / 1000 mL solution D) 0.250 mol KOH / 1 L solution E) 1 L solution / 0.250 mol KOH
B) 0.250 mol KOH / 1000 mL water
54) What is the mass of nickel(II) nitrate (182.71 g/mol) dissolved in 25.0 mL of 0.100 M Ni(NO3)2 solution? A) 0.250 g B) 0.457 g C) 4.00 g D) 45.7 g E) 457 g
B) 0.457 g
40) What is the mass of solute dissolved in 10.0 g of 5.00% sugar solution? A) 0.180 g B) 0.500 g C) 0.900 g D) 9.50 g E) 10.0 g
B) 0.500 g
78) What is the pH of an aqueous solution if the [H+] = 0.1 M? A) 0 B) 1 C) 2 D) 10 E) 13
B) 1
84) What is the pH of an aqueous solution if the [H+] = 0.055 M? A) 0.74 B) 1.26 C) 1.74 D) 2.26 E) 11.74
B) 1.26
22) What is the heat of vaporization(kJ/mol) if it takes 3,452 j of heat to completely vaporize 2.68 moles of the liquid at its boiling point? A) 1288 B) 1.29 C) 0.776 D) 12.2 E) none of the above
B) 1.29
67---1) How many kJ of heat are needed to completely vaporize 3.30 moles of H2O? The heat of vaporization for water at the boiling point is 40.6 kj/mole A) 12.3 B) 134 C) 67.0 D) 2.26 E) none of the above
B) 134
56) What is the volume of 6.00 M nitric acid that contains 6.302 g of HNO3 solute (63.02 g/mol)? A) 0.600 mL B) 16.7 mL C) 60.0 mL D) 167 mL E) 1670 mL
B) 16.7 mL
64) What volume of 0.255 M hydrochloric acid reacts completely with 0.400 g of sodium hydrogen carbonate, NaHCO3 (84.01 g/mol)? NaHCO3(s) + HCl(aq) → NaCl(aq) + H2O(l) + CO2(g) A) 4.76 mL B) 18.7 mL C) 53.6 mL D) 121 mL E) 132 mL
B) 18.7 mL
3) A 250 gram sample of water at the boiling point had 45.0 kJ of heat added. How many grams of water were vaporized? Heat of vaporization for water is 40.6 kj/mole. A) 1.11 B) 20.0 C) 0.902 D) 16.2 E) none of the above
B) 20.0
85) What is the pH of an aqueous solution if the [H+] = 0.000 042 M? A) 0.62 B) 4.38 C) 4.62 D) 5.38 E) 9.62
B) 4.38
82) A 25.0 mL solution of sodium dichromate, Na2Cr2O7 (261.98 g/mol), with a mass of 25.950 g, is evaporated to dryness. If the orange residue has a mass of 1.295 g, what is the mass/mass percent concentration and molarity of the solution? A) 4.99% and 0.190 M B) 4.99% and 0.198 M C) 4.99% and 0.396 M D) 5.18% and 0.190 M E) 5.18% and 0.198 M
B) 4.99% and 0.198 M
81) A 10.0 mL solution of glucose, C6H12O6 (180.18 g/mol), with a mass of 10.483 g, is evaporated to dryness. If the solid white residue has a mass of 0.524 g, what is the mass/mass percent concentration and molarity of the sugar solution? A) 5.00% and 0.277 M B) 5.00% and 0.291 M C) 5.00% and 0.582 M D) 5.24% and 0.277 M E) 5.24% and 0.291 M
B) 5.00% and 0.291 M
33) If 25.0 mL of seawater has a mass of 25.895 g and contains 1.295 g of solute, what is the mass/mass percent concentration of solute in the seawater sample? A) 3.862% B) 5.001% C) 5.18% D) 20.00% E) 96.5%
B) 5.001%
23) How many joules of heat are needed to completely vaporize 24.40 grams of water at its boiling point? Given H vap= 40.6 kJ/mol A) 54.97 B) 5.50 x 10^4 C) 29.98 D)3.00 x 10^4 E) none of the above
B) 5.50 x 10^4
71---5) How many kJ of heat are needed to completely melt 17.3 g of h2O, given that the water is at its melting point? The heat of fusion for water is 6.02kj/mole A) 0.961 B) 5.79 C) 1.04 D) 6.26 E) none of the above
B) 5.79
68---2) How many kJ of heat are needed to completely vaporize 23.4 g of H2O? The heat of vaporization for water at the boiling point is 40.6 kj/mole A) 31.2 B) 52.8 C) 23.4 D) 2.26 E) none of the above
B) 52.8
41) What is the mass of solute dissolved in 50.0 g of 12.5% saline solution? A) 4.00 g B) 6.25 g C) 7.14 g D) 43.8 g E) 625 g
B) 6.25 g
32) If 25.0 mL of urine has a mass of 25.725 g and contains 1.929 g of solute, what is the mass/mass percent concentration of solute in the urine sample? A) 3.887% B) 7.499% C) 7.72% D) 13.34% E) 97.2%
B) 7.499%
55) What is the volume of 12.0 M hydrochloric acid that contains 3.646 g of HCl solute (36.46 g/mol)? A) 1.20 mL B) 8.33 mL C) 83.3 mL D) 120 mL E) 833 mL
B) 8.33 mL
31) If 10.0 mL of blood plasma has a mass of 10.279 g and contains 0.870 g of protein, what is the mass/mass percent concentration of protein in the blood plasma? A) 0.870% B) 8.46% C) 8.70% D) 32.1% E) 97.3%
B) 8.46%
71) Lactic acid is found in sour milk and can be abbreviated HLac. If 47.50 mL of 0.275 M NaOH neutralizes 1.180 g of HLac, what is the molar mass of lactic acid? HLac(aq) + NaOH(aq) → NaLac(aq) + H2O(l) A) 45.1 g/mol B) 90.3 g/mol C) 111 g/mol D) 181 g/mol E) 204 g/mol
B) 90.3 g/mol
41) Which intermolecular force is common to all polar molecules but NOT nonpolar molecules? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
B) dipole-dipole forces
52) Which intermolecular force found in CCL2H2 is the strongest? A) dispersion forces B) dipole-dipole forces C) hydrogen bonding D) X-forces E) none of the above
B) dipole-dipole forces
8) Apply the like dissolves like rule to predict which of the following liquids is miscible with water. A) carbon tetrachloride, CCl4 B) ethanol, C2H5OH C) toluene, C7H8 D) all of the above E) none of the above
B) ethanol, C2H5OH
5) Which of the following is a general property of a basic solution? A) tastes sour B) feels slippery C) turns litmus paper red D) pH less than 7 E) none of the above
B) feels slippery
113) What is the color of bromthymol blue indicator at pH 7, the midpoint at which yellow and blue are in equal concentration? A) blue B) green C) orange D) red E) yellow
B) green
19) The amount of heat required to melt one mole of a solid is called the: A) heat of vaporization. B) heat of fusion. C) heating curve. D) cooling curve. E) none of the above
B) heat of fusion.
36) The ability of sodium chloride to mix with water is most likely due to: A) dispersion force B) ion-dipole force C) dipole-dipole force D) hydrogen bonding E) none of the above
B) ion-dipole force
59) NaCl is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid
B) ionic solid
27) When you make ice cubes: A) it is an endothermic process. B) it is an exothermic process. C) the heat of vaporization must be removed. D) the process is referred to scientifically as sublimation. E) none of the above
B) it is an exothermic process.
2) Which state of matter has a high density and an indefinite shape? A) solids B) liquids C) gases D) both solids and liquids E) none of the above
B) liquids
1) Coca-Cola is carbonated by injection with carbon dioxide gas. Under what conditions is carbon dioxide gas most soluble? A) low temperature, low pressure B) low temperature, high pressure C) high temperature, high pressure D) high temperature, low pressure E) none of the above
B) low temperature, high pressure
118) Which of the following is true if the hydrogen ion concentration of an aqueous solution increases? A) pH increases B) pH decreases C) Kw increases D) Kw decreases E) none of the above
B) pH decreases
65) The reason for many of the unique properties of water is: A) dispersion forces. B) the ability to form hydrogen bonds. C) high surface tension and low volatility. D) moderate viscosity and expanding upon freezing. E) all of the above
B) the ability to form hydrogen bonds.
12) Apply the like dissolves like rule to predict which of the following liquids is immiscible with liquid bromine, Br2. A) chloroform, CHCl3 B) toluene, C6H5CH3 C) water, H2O D) all of the above E) none of the above
B) toluene, C6H5CH3
18) Liquids that have high vapor pressure and low boiling points are called: A) abnormal liquids. B) volatile liquids. C) non-volatile liquids. D) viscous liquids. E) none of the above
B) volatile liquids.
8) If a vinegar sample has a pH of 5, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic
B) weakly acidic
91) What is the [OH-] in an ammonia solution if the pH is 10.20? A) 0.63 M B) 3.80 M C) 0.000 16 M D) 0.000 000 000 16 M E) 0.000 000 000 063 M
C) 0.000 16 M
83) After fasting overnight, a patient's normal blood glucose level is 70-90 mg/dL. Express this range as mass/mass percent concentration. (Assume the density of blood is 1.0 g/mL.) A) 7-9% B) 0.7-0.9% C) 0.07-0.09% D) 0.007-0.009% E) 0.0007-0.0009%
C) 0.07-0.09%
67) What is the molarity of aqueous silver nitrate if 50.0 mL of AgNO3 reacts with 25.0 mL of 0.100 M K2CrO4? 2 AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2 KNO3(aq) A) 0.0250 M B) 0.0500 M C) 0.100 M D) 0.200 M E) 0.400 M
C) 0.100 M
84) An hour after a meal, a patient's blood glucose level is 150 mg/dL. Express this glucose level as mass/mass percent concentration. (Assume the density of blood is 1.0g/mL.) A) 15% B) 1.5% C) 0.15% D) 0.015% E) 0.0015%
C) 0.15%
85) An hour after a meal, a patient's blood glucose level is 180 mg/dL. Express this glucose level as mass/mass percent concentration. (Assume the density of blood is 1.0g/mL.) A) 18% B) 1.8% C) 0.18% D) 0.018% E) 0.0018%
C) 0.18%
55) If a 50.0 mL sample of ammonium hydroxide is titrated with 25.0 mL of 0.200 M sulfuric acid to a methyl red endpoint, what is the molarity of the base? 2 NH4OH(aq) + H2SO4(aq) → (NH4)2SO4(aq) + 2 H2O(l) A) 0.100 M B) 0.150 M C) 0.200 M D) 0.300 M E) 0.400 M
C) 0.200 M
68) What is the molarity of aqueous lithium bromide if 25.0 mL of LiBr reacts with 10.0 mL of 0.250 M Pb(NO3)2? Pb(NO3)2(aq) + 2 LiBr(aq) → PbBr2(s) + 2 LiNO3(aq) A) 0.0500 M B) 0.100 M C) 0.200 M D) 0.250 M E) 1.25 M
C) 0.200 M
47) What is the molarity of a sucrose solution that contains 10.0 g of C12H22O11 (342.34 g/mol) dissolved in 100.0 mL of solution? A) 0.00292 M B) 0.0292 M C) 0.292 M D) 3.42 M E) 34.2 M
C) 0.292 M
46) What is the molarity of a glucose solution that contains 10.0 g of C6H12O6 (180.18 g/mol) dissolved in 100.0 mL of solution? A) 0.00555 M B) 0.0555 M C) 0.555 M D) 1.80 M E) 18.0 M
C) 0.555 M
58) What is the molarity of a hydrochloric acid solution prepared by diluting 250.0 mL of 6.00 M HCl to a total volume of 2.50 L? A) 0.0600 M B) 0.250 M C) 0.600 M D) 2.50 M E) 6.00 M
C) 0.600 M
114) What is the hydrogen ion concentration of an aqueous solution having a pH of 0? A) -1 M B) 0 M C) 1 M D) 10 M E) none of the above
C) 1 M
71) If 37.5 mL of 0.100 M calcium chloride reacts completely with aqueous silver nitrate, what is the mass of AgCl (143.32 g/mol) precipitate? CaCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Ca(NO3)3(aq) A) 0.269 g B) 0.537 g C) 1.07 g D) 537 g E) 269 g
C) 1.07 g
72) If 45.5 mL of 0.150 M sodium sulfate solution reacts completely with aqueous barium nitrate, what is the mass of BaSO4 (233.40 g/mol) precipitate? Ba(NO3)2(aq) + Na2SO4(aq) → BaSO4(s) + 2 NaNO3(aq) A) 0.0292 g B) 0.769 g C) 1.59 g D) 6.83 g E) 34.1 g
C) 1.59 g
35) Which of the following is not a unit factor related to a 10.0% aqueous solution of sodium hydroxide, NaOH? A) 10.0 g NaOH / 90.0 g water B) 10.0 g NaOH / 100 g solution C) 100 g solution / 90.0 g NaOH D) 100 g solution / 90.0 g water E) 90.0 g water / 100 g solution
C) 100 g solution / 90.0 g NaOH
70) Proline is an amino acid that can be abbreviated HPro. If 33.55 mL of 0.150 M NaOH neutralizes 0.579 g of HPro, what is the molar mass of proline? HPro(aq) + NaOH(aq) → NaPro(aq) + H2O(l) A) 8.69 g/mol B) 86.9 g/mol C) 115 g/mol D) 291 g/mol E) 772 g/mol
C) 115 g/mol
24) How many kilojoules of heat are needed to completely vaporize 42.8 grams of C4H10Oat its boiling point? Given H vap= 26.5kJ/mol A) 74.12 B) 9.49 C) 15.3 D) 16.3 E) none of the above
C) 15.3
53) What is the mass of zinc acetate (183.49 g/mol) dissolved in 0.200 L of 0.500 M Zn(C2H3O2)2 solution? A) 1.83 g B) 12.4 g C) 18.3 g D) 36.7 g E) 91.7 g
C) 18.3 g
59) A hydrochloric acid solution is 6.00 M and the density is 1.10 g/mL. What is the mass/mass percent concentration of HCl (36.46 g/mol)? A) 0.199% B) 0.241% C) 19.9% D) 21.9% E) 24.1%
C) 19.9%
32) How many grams of C4H10O can be melted by 2.00 X 10^3 J? Given H fus =7.27 kJ/mol A) 14.5 B) 3.64 C) 20.4 D) 74.1 E) none of the above
C) 20.4
65) What volume of 0.115 M hydrochloric acid reacts completely with 0.125 g of sodium carbonate, Na2CO3 (105.99 g/mol)? Na2CO3(s) + 2 HCl(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g) A) 9.75 mL B) 10.3 mL C) 20.5 mL D) 41.0 mL E) 97.5 mL
C) 20.5 mL
44) What is the mass of water required to prepare 250.0 g of 10.0% copper(II) sulfate solution? A) 25.0 g B) 27.8 g C) 225 g D) 278 g E) 2250 g
C) 225 g
51) If 25.0 mL of 0.100 M Ca(OH)2 is titrated with 0.200 M HNO3, what volume of nitric acid is required to neutralize the base? 2 HNO3(aq) + Ca(OH)2(aq) → 2 Ca(NO3)2(aq) + 2 H2O(l) A) 12.5 mL B) 20.0 mL C) 25.0 mL D) 40.0 mL E) 50.0 mL
C) 25.0 mL
66) If 1.020 g of KHC8H4O4 (204.23 g/mol) is completely neutralized with 0.200 M KOH, what volume of potassium hydroxide is required? KHC8H4O4(aq) + KOH(aq) → K2C8H4O4(aq) + 2 H2O(l) A) 12.5 mL B) 20.0 mL C) 25.0 mL D) 40.0 mL E) 50.0 mL
C) 25.0 mL
68) If 1.020 g of KHC8H4O4 (204.23 g/mol) is completely neutralized with 0.200 M KOH, what volume of potassium hydroxide is required? KHC8H4O4(aq) + KOH(aq) → K2C8H4O4(aq) + 2 H2O(l) A) 12.5 mL B) 20.0 mL C) 25.0 mL D) 40.0 mL E) 50.0 mL
C) 25.0 mL
79) What is the pH of an aqueous solution if the [H+] = 0.001 M? A) 1 B) 2 C) 3 D) 10 E) 11
C) 3
57) What is the volume of 3.00 M sulfuric acid that contains 9.809 g of H2SO4 solute (98.09 g/mol)? A) 0.300 mL B) 30.0 mL C) 33.3 mL D) 333 mL E) 3330 mL
C) 33.3 mL
57) An acetic acid solution is 6.00 M and has a density of 1.04 g/mL. What is the mass/mass percent concentration of HC2H3O2 (60.06 g/mol)? A) 0.347% B) 0.375% C) 34.7% D) 36.0% E) 37.5%
C) 34.7%
45) What is the mass of water required to prepare 5.25 kg of 15.0% calcium nitrate solution? A) 0.788 kg B) 0.926 kg C) 4.46 kg D) 6.18 kg E) 29.8 kg
C) 4.46 kg
52) If 20.0 mL of 0.200 M H2SO4 is titrated with 0.100 M NaOH, what volume of sodium hydroxide is required to neutralize the acid? H2SO4(aq) + 2 NaOH(aq) → Na2SO4(aq) + 2 H2O(l) A) 10.0 mL B) 20.0 mL C) 40.0 mL D) 60.0 mL E) 80.0 mL
C) 40.0 mL
61) What volume of 12 M acid must be diluted with distilled water to prepare 5.0 L of 0.10 M acid? A) 0.042 mL B) 6 mL C) 42 mL D) 60 mL E) 420 mL
C) 42 mL
43) What is the mass of water required to prepare 50.0 g of 10.0% sodium nitrate solution? A) 5.00 g B) 5.56 g C) 45.0 g D) 55.6 g E) 450 g
C) 45.0 g
80) What is the pH of an aqueous solution if the [H+] = 0.000 001 M? A) 1 B) 5 C) 6 D) 8 E) 10
C) 6
5) Which of the following illustrates the like dissolves like rule for two liquids? A) A polar solute is miscible with a nonpolar solvent. B) A polar solute is immiscible with a polar solvent. C) A nonpolar solute is miscible with a nonpolar solvent. D) A nonpolar solvent is miscible with a polar solvent. E) none of the above
C) A nonpolar solute is miscible with a nonpolar solvent.
97) If a battery acid solution is a strong electrolyte, which of the following must be true? A) Battery acid is highly reactive. B) Battery acid is slightly reactive. C) Battery acid is highly ionized. D) Battery acid is slightly ionized. E) none of the above
C) Battery acid is highly ionized.
20) Compare a small pot of water that is boiling vigorously to a large pot of water that is boiling gently. Which statement is TRUE? A) The small pot is boiling at higher temperature than the large pot. B) The large pot is boiling at a higher temperature than the small pot. C) Both pots are boiling at the same temperature. D) The vapor pressure of the liquid is greater than the pressure above the pot in each case. E) none of the above
C) Both pots are boiling at the same temperature.
98) If a drain cleaner solution is a strong electrolyte, which of the following must be true? A) Drain cleaner is highly reactive. B) Drain cleaner is slightly reactive. C) Drain cleaner is highly ionized. D) Drain cleaner is slightly ionized. E) none of the above
C) Drain cleaner is highly ionized.
93)---5) Why is fluoride beneficial for developing cavity-free teeth? A) Fluoride converts tooth enamel to CaF2. B) Fluoride converts tooth enamel to SnF2. C) Fluoride converts tooth enamel to Ca10(PO4)6F2. D) Fluoride converts tooth enamel to Ca10(PO4)6(OH)2. E) none of the above
C) Fluoride converts tooth enamel to Ca10(PO4)6F2.
107) Nitric acid is a strong acid, ammonium hydroxide is a weak base, and ammonium nitrate is a soluble salt. Which of the following is the net ionic equation for the reaction? HNO3(aq) + NH4OH(aq) → NH4NO3(aq) + H2O(l) A) H+(aq) + OH-(aq) → H2O(l) B) NO3-(aq) + NH4+(aq) → NH4NO3(aq) C) H+(aq) + NH4OH(aq) → NH4+(aq) + H2O(l) D) HNO3(aq) + OH-(aq) → NO3-(aq) + H2O(l) E) none of the above
C) H+(aq) + NH4OH(aq) → NH4+(aq) + H2O(l)
16) Which of the following is a weak acid? A) HCl(aq) (~ 100% ionized) B) HNO3(aq) (~ 100% ionized) C) HC2H3O2(aq) (~ 1% ionized) D) all of the above E) none of the above
C) HC2H3O2(aq) (~ 1% ionized)
27) When potassium iodide, KI, dissolves in water, which of the following is formed in aqueous solution? A) K+ -------H-O I H B) I- ----O-H I H C) I- -----H-O I H D) all of the above E) none of the above
C) I- -----H-O I H
58) Which substance below is an ionic solid? A) Cu (s) B) H2O (s) C) MgO (s) D) C6H12O6 (s) E) none of the above
C) MgO (s)
56) Rank the compounds NH3, CH4, and PH3 in order of increasing boiling point. A) NH3 < CH4< PH3 B) CH4< NH3 < PH3 C) NH3 < PH3< CH4 D) CH4 < PH3 < NH3 E) PH3< NH3 < CH4
C) NH3 < PH3< CH4
102) Which of the following in aqueous solution is a weak electrolyte? A) H2CO3(aq) B) LiOH(aq) C) NH4Cl(aq) D) all of the above E) none of the above
C) NH4Cl(aq)
53) Consider the three compounds below, then choose the compound(s) that have hydrogen bonding. 1) H2 2) CH4 3) HF A) Only compound 1 has hydrogen bonding. B) Only compound 2 has hydrogen bonding. C) Only compound 3 has hydrogen bonding. D) All three of these compounds have hydrogen bonding. E) None of these compounds have hydrogen bonding.
C) Only compound 3 has hydrogen bonding.
54) If a 50.0 mL sample of ammonium hydroxide is titrated with 25.0 mL of 0.200 M nitric acid to a methyl red endpoint, what is the molarity of the base? NH4OH(aq) + HNO3(aq) → NH4NO3(aq) + H2O(l) A) 0.100 M B) 0.150 M C) 0.200 M D) 0.300 M E) 0.400 M
D) 0.300 M
65) What is the molarity of a sodium hydroxide solution if 40.00 mL of NaOH is required to neutralize 0.900 g of oxalic acid, H2C2O4, (90.04 g/mol)? H2C2O4(aq) + 2 NaOH(aq) →Na2C2O4(aq) + 2 H2O(l) A) 0.125 M B) 0.250 M C) 0.400 M D) 0.500 M E) 0.800 M
D) 0.500 M
17) The rate of vaporization of a liquid can be increased by: 1. increasing the surface area 2. increasing the temperature 3. increasing the strength of the intermolecular forces A) 1 only B) 2 only C) 3 only D) 1 and 2 only E) 2 and 3 only
D) 1 and 2 only
63) What volume of 18 M acid must be diluted with distilled water to prepare 500.0 mL of 0.50 M acid? A) 0.014 mL B) 0.14 mL C) 1.4 mL D) 14 mL E) 140 mL
D) 14 mL
62) What volume of 16 M acid must be diluted with distilled water to prepare 500.0 mL of 0.50 M acid? A) 0.016 mL B) 0.16 mL C) 1.6 mL D) 16 mL E) 160 mL
D) 16 mL
37) What is the mass of a 10.0% blood plasma sample that contains 2.50 g of dissolved solute? A) 0.250 g B) 0.278 g C) 22.5 g D) 25.0 g E) 250 g
D) 25.0 g
50) If 25.0 mL of 0.100 M HCl is titrated with 0.150 M Ba(OH)2, what volume of barium hydroxide is required to neutralize the acid? 2 HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2 H2O(l) A) 8.33 mL B) 16.7 mL C) 18.8 mL D) 33.3 mL E) 37.5 mL
D) 33.3 mL
49) If 20.0 mL of 0.500 M KOH is titrated with 0.250 M HNO3, what volume of nitric acid is required to neutralize the base? HNO3(aq) + KOH(aq) → KNO3(aq) + H2O(l) A) 10.0 mL B) 20.0 mL C) 25.0 mL D) 40.0 mL E) 50.0 mL
D) 40.0 mL
53) If 30.0 mL of 0.100 M Ca(OH)2 is titrated with 0.150 M HC2H3O2, what volume of acetic acid is required to neutralize the base? 2 HC2H3O2(aq) + Ca(OH)2(aq) → Ca(C2H3O2)2(aq) + 2 H2O(l) A) 10.0 mL B) 22.5 mL C) 20.0 mL D) 40.0 mL E) 45.0 mL
D) 40.0 mL
91) ---3) In 2000, how many of the 50 largest cities in the United States had drinking water that was naturally or artificially fluoridated? A) 2 B) 10 C) 25 D) 42 E) 50
D) 42
31) How much energy does it take to melt a 16.87 g ice cube? Hfus= 6.02 kJ/mol A) 102 kJ B) 108 kJ C) 936 J D) 5.64 kJ E) none of the above
D) 5.64 kJ
86) What is the molar concentration of water molecules in a beaker of water? (The density of water is 1.00 g/mL.) A) 0.0555 M B) 1.00 M C) 18.0 M D) 55.5 M E) 18,000 M
D) 55.5 M
90)---2) What is the approximate percentage of the population in the United States who drink water that is naturally or artificially fluoridated? A) 1% B) 10% C) 50% D) 67% E) 100%
D) 67%
86) What is the pH of an aqueous solution if the [H+] = 0.000 000 075 M? A) 0.88 B) 6.12 C) 6.88 D) 7.12 E) 8.88
D) 7.12
69) Glycine is an amino acid that can be abbreviated HGly. If 27.50 mL of 0.120 M NaOH neutralizes 0.248 g of HGly, what is the molar mass of glycine? HGly(aq) + NaOH(aq) → NaGly(aq) + H2O(l) A) 26.6 g/mol B) 37.6 g/mol C) 56.8 g/mol D) 75.2 g/mol E) 151 g/mol
D) 75.2 g/mol
39) What is the mass of a 12.5% blood plasma sample that contains 10.0 g of dissolved solute? A) 1.25 g B) 1.43 g C) 70.0 g D) 80.0 g E) 125 g
D) 80.0 g
66) What volume of 0.100 M hydrochloric acid reacts completely with 0.500 g of sodium carbonate, Na2CO3 (105.99 g/mol)? Na2CO3(s) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g) A) 10.6 mL B) 23.6 mL C) 47.2 mL D) 94.3 mL E) 211 mL
D) 94.3 mL
15) Which of the following illustrates the like dissolves like rule for a solid solute in a liquid solvent? A) An ionic compound is soluble in a nonpolar solvent. B) A polar compound is soluble in a nonpolar solvent. C) A nonpolar compound is soluble in a polar solvent. D) A nonpolar compound is soluble in a nonpolar solvent. E) none of the above
D) A nonpolar compound is soluble in a nonpolar solvent.
15) Which of the following statements is FALSE? A) Evaporation is an endothermic process. B) A puddle of water cools down as it evaporates. C) As a liquid is converted into a gas, the liquid absorbs heat. D) All of the above are true. E) None of the above are true.
D) All of the above are true.
45) Which molecule below has hydrogen bonding? A) C B) HCl C)H2 D) CH3CH2OH E) all of the above
D) CH3CH2OH
54) Which compound will have the highest boiling point? A) CH4 B) CH3CH3 C) CH3C(O)CH3 D) CH3CH2OH E) not enough information
D) CH3CH2OH
43) Which substance is most likely to be miscible with water? A) CF4 B) Br2 C) CS2 D) CHCl3 E) none of the above
D) CHCl3
55) Which substance would be expected to have the highest boiling point? A) N2 B) O2 C) CO2 D) CO E) not enough information
D) CO
92)----4) What is the formula for hydroxyapatite, which is found in tooth enamel and is the hardest substance in the human body? A) CaF2 B) Ca3(PO4)2 C) Ca10(PO4)6F2 D) Ca10(PO4)6(OH)2 E) none of the above
D) Ca10(PO4)6(OH)2
37) Which substance below has dipole-dipole forces? A) CH4 B) CO2 C) F2 D) H2S E) none of the above
D) H2S
2) Pepsi-Cola is carbonated by injection with carbon dioxide gas. Under what conditions is carbon dioxide gas least soluble? A) low temperature, low pressure B) low temperature, high pressure C) high temperature, high pressure D) high temperature, low pressure E) none of the above
D) high temperature, low pressure
10) A situation where two opposite processes are occurring at equal rates, and no net change is taking place, is called: A) vaporization. B) condensation. C) evaporation. D) dynamic equilibrium. E) none of the above
D) dynamic equilibrium.
6) Which of the following is a general property of a basic solution? A) tastes sour B) turns litmus paper red C) pH less than 7 D) neutralizes bases E) none of the above
D) neutralizes bases
42) Substance A is a molecular compound that dissolves in gasoline but not in water. The molecules of A are very likely: A) metallic. B) nonmetallic. C) polar. D) nonpolar. E) none of the above
D) nonpolar.
77) Which of the following properties must be similar for two liquids to be soluble? A) boiling point B) density C) molar mass D) polarity E) reactivity
D) polarity
9) The change of a substance from a liquid to a gaseous form is called: A) dynamic equilibrium. B) heat of fusion. C) condensation. D) vaporization. E) volatile.
D) vaporization.
10) If milk of magnesia has a pH of 10, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic
D) weakly basic
92) What is the [OH-] in an oven-cleaning solution if the pH is 12.35? A) 0.45 M B) 1.65 M C) 0.022 M D) 0.000 000 000 002 2 M E) 0.000 000 000 000 45 M
E) 0.000 000 000 000 45 M
88) What is the [H+] in a blood sample that registers 7.30 using a pH meter? A) 0.86 M B) 0.000 020 M C) 0.000 000 50 M D) 0.000 000 020 M E) 0.000 000 050 M
E) 0.000 000 050 M
87) What is the [H+] in an acid rain sample that registers 3.22 using a pH meter? A) 0.51 M B) 0.017 M C) 0.0017 M D) 0.000 17 M E) 0.000 60 M
E) 0.000 60 M
63) What is the molarity of a acetic acid solution if 25.00 mL of HC2H3O2 is required to neutralize 0.424 g of sodium carbonate (105.99 g/mol)? 2 HC2H3O2(aq) + Na2CO3(aq) → 2 NaC2H3O2 (aq) + H2O(l) + CO2(g) A) 0.0800 M B) 0.100 M C) 0.160 M D) 0.200 M E) 0.320 M
E) 0.320 M
56) If a 25.0 mL sample of sulfuric acid is titrated with 50.0 mL of 0.200 M potassium hydroxide to a phenolphthalein endpoint, what is the molarity of the acid? H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l) A) 0.100 M B) 0.150 M C) 0.200 M D) 0.300 M E) 0.400 M
E) 0.400 M
75) If the solubility of nitrogen in blood is 1.90 cc per 100 cc at 1.00 atmosphere, what is the solubility of nitrogen in a scuba diver's blood at a depth of 150 feet where the pressure is 5.55 atmospheres? A) 0.190 cc/100 cc B) 0.380 cc/100 cc C) 1.90 cc/100 cc D) 3.80 cc/100 cc E) 10.5 cc/100 cc
E) 10.5 cc/100 cc
58) An ammonia solution is 6.00 M and the density is 0.950 g/mL. What is the mass/mass percent concentration of NH3 (17.04 g/mol)? A) 0.0971% B) 0.108% C) 9.71% D) 10.2% E) 10.8%
E) 10.8%
74) If the solubility of carbon dioxide in a bottle of champagne is 1.45 g per liter at 1.00 atmosphere, what is the solubility of carbon dioxide at 10.0 atmospheres? A) 0.145 g/L B) 0.725 g/L C) 1.45 g/L D) 2.90 g/L E) 14.5 g/L
E) 14.5 g/L
38) What is the mass of a 7.50% urine sample that contains 122 g of dissolved solute? A) 9.15 g B) 9.89 g C) 915 g D) 1500 g E) 1630 g
E) 1630 g
67) If 0.900 g of oxalic acid, H2C2O4, (90.04 g/mol) is completely neutralized with 0.500 M LiOH, what volume of lithium hydroxide is required? H2C2O4(aq) + 2 LiOH(aq) → Li2C2O4(aq) + 2 H2O(l) A) 10.0 mL B) 15.0 mL C) 20.0 mL D) 30.0 mL E) 40.0 mL
E) 40.0 mL
76) If the solubility of helium is 0.94 cc per 100 cc of blood at 1.00 atmosphere, what is the solubility of helium in a scuba diver's blood at a depth of 297 feet where the pressure is 10.0 atmospheres? A) 0.094 cc/100 cc B) 0.19 cc/100 cc C) 0.94 cc/100 cc D) 3.8 cc/100 cc E) 9.4 cc/100 cc
E) 9.4 cc/100 cc
39) Which noble gas has the highest boiling point? A) He B) Ne C) Ar D) Kr E) Xe
E) Xe
77) Given an aqueous solution in which the [H+] = 2.5 x 10-7 M, what is the molar hydroxide ion concentration? A) [OH-] = 2.5 x 10-7 M B) [OH-] = 2.5 x 10-8 M C) [OH-] = 4.0 x 10-6 M D) [OH-] = 4.0 x 10-7 M E) [OH-] = 4.0 x 10-8 M
E) [OH-] = 4.0 x 10-8 M
75) Given an aqueous solution in which the [H+] = 2.0 x 10-5 M, what is the molar hydroxide ion concentration? A) [OH-] = 2.0 x 10-9 M B) [OH-] = 2.0 x 10-10 M C) [OH-] = 5.0 x 10-8 M D) [OH-] = 5.0 x 10-9 M E) [OH-] = 5.0 x 10-10 M
E) [OH-] = 5.0 x 10-10 M
1) Intermolecular forces are responsible for: A) the taste sensations. B) the shape of protein molecules. C) the function of DNA. D) the existence of liquids and solids. E) all of the above
E) all of the above
1) Which of the following is a general property of an acidic solution? A) tastes sour B) turns litmus paper red C) pH less than 7 D) neutralizes bases E) all of the above
E) all of the above
11) Increasing the intermolecular forces of a liquid will do which of the following? A) increase the viscosity B) decrease the evaporation rate C) increase the surface tension D) decrease the vapor pressure E) all of the above
E) all of the above
14) Evaporation is: A) increased by increasing temperature. B) an endothermic process. C) the opposite process to condensation. D) a cooling process for humans when they sweat. E) all of the above
E) all of the above
19) Apply the like dissolves like rule to predict which of the following vitamins is soluble in water. A) thiamine, C12H17N4OS B) riboflavin, C17H20N4O6 C) niacinamide, C6H6N2O D) cyanocobalamin, C63H88CoN14O14P E) all of the above
E) all of the above
18) Apply the like dissolves like rule to predict which of the following solids is insoluble in water. A) cholesterol, C27H46O B) citric acid, C6H8O7 C) fructose, C6H12O6 D) glycine, CH2(NH2)COOH E) lactic acid, CH3CH(OH)COOH
A) cholesterol, C27H46O
73) Which of the following explains why bubbles form on the inside of a pan of water when the pan of water is heated? A) As temperature increases, the solubility of air is less. B) As temperature increases, the kinetic energy decreases. C) As temperature increases, the vapor pressure increases. D) As temperature increases, the atmospheric pressure decreases. E) none of the above
A) As temperature increases, the solubility of air is less.
47) Which compound in liquid form will have the highest vapor pressure? A) CH4 B) CH3CH3 C) CH3C(O)CH3 D) CH3CH2OH E) not enough information
A) CH4
40) Assuming that the molecules carbon monoxide (CO) and nitrogen (N2) have similar electron clouds, which statement below is TRUE? A) CO has the higher boiling point because it experiences dipole-dipole forces. B) N2 has the higher boiling point because it experiences dipole-dipole forces. C) The N2 has the higher boiling point because it has greater dispersion forces. D) Both CO and N2 must have the same boiling point. E) none of the above
A) CO has the higher boiling point because it experiences dipole-dipole forces.
126)---4) Steelmaking plants and electric power plants that burn low-grade coal release which of the following atmospheric pollutants that produces acid rain? A) CO2 B) NO2 C) SO2 D) all of the above E) none of the above
A) CO2
106) Nitric acid is a strong acid, sodium hydroxide is a strong base, and sodium nitrate is a soluble salt. Which of the following is the net ionic equation for the reaction? HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l) A) H+(aq) + OH-(aq) → H2O(l) B) NO3-(aq) + Na+(aq) → NaNO3(s) C) H+(aq) + NaOH(aq) → Na+(aq) + H2O(l) D) HNO3(aq) + OH-(aq) → NO3-(aq) + H2O(l) E) none of the above
A) H+(aq) + OH-(aq) → H2O(l)
108) Acetic acid is a weak acid, potassium hydroxide is a strong base, and potassium acetate is a soluble salt. Which of the following is the net ionic equation for the reaction? HC2H3O2(aq) + KOH(aq) → KC2H3O2(aq) + H2O(l) A) H+(aq) + OH-(aq) → H2O(l) B) C2H3O2-(aq) + K+(aq) → KC2H3O2(aq) C) H+(aq) + KOH(aq) → K+(aq) + H2O(l) D) HC2H3O2(aq) + OH-(aq) → C2H3O2-(aq) + H2O(l) E) none of the above
A) H+(aq) + OH-(aq) → H2O(l)
29) In the following reaction, which reactant is a Brønsted-Lowry acid? H2CO3(aq) + Na2HPO4(aq) → NaHCO3(aq) + NaH2PO4(aq) A) H2CO3 B) Na2HPO4 C) NaH2PO4 D) NaHCO3 E) none of the above
A) H2CO3
27) In the following reaction, which reactant is a Brønsted-Lowry acid? HCl(aq) + KHS(aq) KCl(aq) + H2S(aq) A) HCl B) KHS C) KCl D) H2S E) none of the above
A) HCl
34) In the following reaction, which reactant is a Brønsted-Lowry base? KC2H3O2(aq) + HCN(aq) → HC2H3O2(aq) + KCN(aq) A) KC2H3O2 B) HCN C) HC2H3O2 D) KCN E) none of the above
A) KC2H3O2
73) Which of the following is the ionization constant expression for water? A) Kw = [H+] [OH-] B) Kw = [H2O] [H2O] C) Kw = [H2O] / [H+] [OH-] D) Kw = [H+] [OH-] / [H2O] E) none of the above
A) Kw = [H+] [OH-]
25) When lithium chloride, LiCl, dissolves in water, which of the following is formed in aqueous solution? A) Li+-------O-H I H B) Li+-----H-O I H C) Cl- ---O-H I H D) all of the above E) none of the above
A) Li+----O-H I H
22) Which of the following is a weak base? A) NH4OH(aq) (~ 1% ionized) B) KOH(aq) (~ 100% ionized) C) LiOH(aq) (~ 100% ionized) D) all of the above E) none of the above
A) NH4OH(aq) (~ 1% ionized)
38) In the following reaction, which reactant is a Brønsted-Lowry base? Na2HPO4(aq) + H2CO3(aq) → NaH2PO4(aq) + NaHCO3(aq) A) Na2HPO4 B) H2CO3 C) NaH2PO4 D) NaHCO3 E) none of the above
A) Na2HPO4
36) In the following reaction, which reactant is a Brønsted-Lowry base? NaHCO3(aq) + NaH2PO4(aq) → Na2HPO4(aq) + H2CO3(aq) A) NaHCO3 B) NaH2PO4 C) Na2HPO4 D) H2CO3 E) none of the above
A) NaHCO3
32) In the following reaction, which reactant is a Brønsted-Lowry base? NaHS(aq) + HCN(aq) → NaCN(aq) + H2S(aq) A) NaHS B) HCN C) NaCN D) H2S E) none of the above
A) NaHS
30) Why does grinding solid crystals increase the rate of dissolving for a solid solute in water? A) Smaller crystals have more surface area. B) Smaller crystals have more energy. C) Smaller crystals are more nonpolar. D) Smaller crystals are more polar. E) none of the above
A) Smaller crystals have more surface area.
28) Which statement is TRUE in describing what occurs when a solid melts to a liquid? A) The process is endothermic and the heat of fusion is positive. B) The process is endothermic and the heat of fusion is negative. C) The process is exothermic and the heat of fusion is positive. D) The process is exothermic and the heat of fusion is negative. E) not enough information
A) The process is endothermic and the heat of fusion is positive.
93) If a light bulb in a conductivity apparatus glows brightly when testing a solution, which of the following must be true? A) The solution is highly ionized. B) The solution is slightly ionized. C) The solution is highly reactive. D) The solution is slightly reactive. E) none of the above
A) The solution is highly ionized.
94) If a light bulb in a conductivity apparatus glows dimly when testing a solution, which of the following must be true? A) The solution is highly ionized. B) The solution is slightly ionized. C) The solution is highly reactive. D) The solution is slightly reactive. E) none of the above
A) The solution is highly ionized.
95) If an unknown solution is a good conductor of electricity, which of the following must be true? A) The solution is highly ionized. B) The solution is slightly ionized. C) The solution is highly reactive. D) The solution is slightly reactive. E) none of the above
A) The solution is highly ionized.
116) Which of the following is true if the pH of a solution decreases from 5 to 2? A) [ H+ ] increases B) [ H+ ] decreases C) Kw increases D) Kw decreases E) none of the above
A) [ H+ ] increases
16) Apply the like dissolves like rule to predict which of the following solids is soluble in water. A) alanine (an amino acid), CH3CH(NH2)COOH B) benzopyrene (in charcoal), C20H12 C) DDT (an insecticide), C14H9Cl5 D) naphthalene (moth repellent), C10H8 E) paradichlorobenzene (fumigant), C6H4Cl2
A) alanine (an amino acid), CH3CH(NH2)COOH
87) Which of the following best explains why peanut butter can remove grease from soiled clothing? A) Peanut butter and grease are both organic. B) Peanut butter and grease are both polar. C) Peanut butter and grease are both nonpolar. D) Peanut butter is polar and grease is nonpolar. E) Peanut butter is nonpolar and grease is polar.
C) Peanut butter and grease are both nonpolar.
124)---2) Which of the following atmospheric pollutants that causes acid rain is mainly from the combustion of fossil fuels? A) CO2 B) NO2 C) SO2 D) all of the above E) none of the above
C) SO2
13) Which statement about boiling point is FALSE? A) The boiling point is higher for compounds with strong intermolecular forces. B) The boiling point is higher for compounds with a high viscosity. C) The boiling point of a compound is an absolute constant. D) The boiling point of a compound is higher for nonvolatile compounds. E) All of the above statements are true.
C) The boiling point of a compound is an absolute constant.
128)---6) What is the difference in pH between acid rain and normal rain? A) The pH of acid rain is below 1, and normal rain is about 5.5. B) The pH of acid rain is below 5, and normal rain is neutral. C) The pH of acid rain is below 5, and normal rain is about 5.5. D) The pH of acid rain is below 7, and normal rain is neutral. E) The pH of acid rain is below 7, and normal rain is about 5.5.
C) The pH of acid rain is below 5, and normal rain is about 5.5.
76) Given an aqueous solution in which the [H+] = 5.0 x 10-3 M, what is the molar hydroxide ion concentration? A) [OH-] = 2.0 x 10-10 M B) [OH-] = 2.0 x 10-11 M C) [OH-] = 2.0 x 10-12 M D) [OH-] = 5.0 x 10-11 M E) [OH-] = 5.0 x 10-12 M
C) [OH-] = 2.0 x 10-12 M
121) Beakers W, X, Y, and Z contain either aqueous NaOH, KOH, LiOH, or NH4OH. Which beaker contains aqueous ammonia if the light bulb glows brightly when testing the conductivity of beakers W, X, and Z? A) beaker W B) beaker X C) beaker Y D) beaker Z E) all of the above
C) beaker Y
60) Silicon is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid
C) covalent atomic solid
66) Which sequence correctly shows the increasing density of the three phases of water? A) solid < liquid < gas B) gas < liquid < solid C) gas < solid < liquid D) liquid < gas < solid E) none of the above
C) gas < solid < liquid
4) Which state of matter has a low density and an indefinite volume? A) solids B) liquids C) gases D) both solids and liquids E) none of the above
C) gases
5) Which state of matter has a low density and is easily compressed? A) solids B) liquids C) gases D) both solids and liquids E) none of the above
C) gases
48) Which intermolecular force is the strongest? A) dispersion force B) dipole-dipole force C) hydrogen bonding D) ion-dipole force E) none of the above
C) hydrogen bonding
63) What are the principal forces holding ice together? A) dispersion forces only B) electrostatic attraction C) intermolecular forces D) sea of electrons E) none of the above
C) intermolecular forces
9) If a saliva specimen has a pH of 7, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic
C) neutral
112) What is the color of methyl red indicator at pH 5, the midpoint at which red and yellow are in equal concentration? A) blue B) green C) orange D) red E) yellow
C) orange
41) Which of the following indicators is colorless in an acidic solution and pink in a basic solution? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
C) phenolphthalein
44) Which of the following indicators is pink at pH 9? A) methyl red B) bromthymol blue C) phenolphthalein D) all of the above E) none of the above
C) phenolphthalein
46) What is the color of phenolphthalein indicator at pH 10? A) red B) blue C) pink D) colorless E) none of the above
C) pink
127)---5) Steelmaking plants and electric power plants that burn low-grade coal produce which of the following acids in acid rain? A) carbonic acid B) nitric acid C) sulfuric acid D) all of the above E) none of the above
C) sulfuric acid
7) The tendency of a liquid to minimize its surface area is called: A) capillary action. B) viscosity. C) surface tension. D) vaporization. E) none of the above
C) surface tension.
8) The measure of the resistance to the flow of a liquid is called: A) vapor pressure. B) sublimation. C) viscosity. D) condensation. E) none of the above
C) viscosity.
89) What is the [H+] in a bleach sample that registers 9.55 using a pH meter? A) 0.98 M B) 0.000 000 002 8 M C) 0.000 000 003 5 M D) 0.000 000 000 28 M E) 0.000 000 000 35 M
D) 0.000 000 000 28 M
90) What is the [OH-] in a seawater sample if the pH is 8.65? A) 0.22 M B) 5.35 M C) 0.000 004 5 M D) 0.000 000 002 2 M E) 0.000 000 004 5 M
D) 0.000 000 002 2 M
83) What is the hydrogen ion concentration in a saliva specimen that registers a pH of 6 on a strip of pH paper? A) 0.6 M B) 0.000 01 M C) 0.000 06 M D) 0.000 001 M E) 0.000 006 M
D) 0.000 001 M
82) What is the hydrogen ion concentration in a urine specimen that registers a pH of 4 on a strip of pH paper? A) 0.4 M B) 0.001 M C) 0.004 M D) 0.0001 M E) 0.0004 M
D) 0.0001 M
50) Which of the following unit factors is not related to a 0.100 M NaBr solution? A) 0.100 mol NaBr / 1 L solution B) 1 L solution / 0.100 mol NaBr C) 1000 mL solution / 0.100 mol NaBr D) 0.100 mol NaBr / 1000 mL water E) 0.100 mol NaBr / 1000 g solution
D) 0.100 mol NaBr / 1000 mL water
What is the molarity of aqueous potassium hydroxide if 42.5 mL of KOH reacts with 25.0 mL of 0.100 M H3PO4? H3PO4(aq) + 3 KOH(aq) → K3PO4(aq) + 3 H2O(l) A) 0.0196 M B) 0.0567 M C) 0.0588 M D) 0.176 M E) 0.510M
D) 0.176 M
6) Which statement about surface tension is FALSE? A) Liquids tend to minimize their surface area. B) Molecules on the surface of the liquid have fewer molecules to interact with. C) Increased intermolecular forces increase surface tension. D) Items with densities lower than water will sink due to surface tension. E) All of the above statements are true.
D) Items with densities lower than water will sink due to surface tension.
88) Which of the following best explains why soap and water remove grease? A) Soap molecules are large polymers that absorb grease. B) Soap molecules are nonpolar and dissolve in grease. C) Soap molecules are ionic and attracted to grease. D) Soap molecules have ionic "heads" that dissolve in water and nonpolar "tails" that dissolve in grease. E) Soap molecules have ionic "heads" that dissolve in grease and nonpolar "tails" that dissolve in water.
D) Soap molecules have ionic "heads" that dissolve in water and nonpolar "tails" that dissolve in grease.
74) Which of the following explains why distilled water is neutral? A) Distilled water has no ions. B) Distilled water has no hydrogen ions. C) Distilled water has no hydroxide ions. D) The concentrations of hydrogen and hydroxide ions are equal. E) none of the above
D) The concentrations of hydrogen and hydroxide ions are equal.
33) In northern climates, it is common to have a layer of frost form on cars that have been out overnight in the winter. During the day the frost layer disappears despite the temperature of the ice remaining below freezing. How? A) The frost melts due to the sun heating the surface of the car above the melting point. B) The frost evaporates due to the sun heating the solid. C) The frost cycles as does the saturation level of moisture in the winter air does from night to day. D) The frost sublimes directly from solid ice to water vapor. E) none of the above
D) The frost sublimes directly from solid ice to water vapor.
10) Apply the like dissolves like rule to predict which of the following liquids is miscible with liquid bromine, Br2. A) benzene, C6H6 B) carbon tetrachloride, CCl4 C) hexane, C6H14 D) all of the above E) none of the above
D) all of the above
100) Which of the following aqueous solutions is slightly ionized? A) weak acid B) weak base C) very slightly soluble salt D) all of the above E) none of the above
D) all of the above
11) Apply the like dissolves like rule to predict which of the following liquids is miscible with liquid bromine, Br2. A) heptane, C7H16 B) methylene chloride, CH2Cl2 C) xylene, C8H10 D) all of the above E) none of the above
D) all of the above
12) Which of the following is an example of an Arrhenius acid? A) HCl(aq) B) HNO3(aq) C) H2SO4(aq) D) all of the above E) none of the above
D) all of the above
123)---1) Which of the following atmospheric pollutants contributes to acid rain? A) CO2 B) NO2 C) SO2 D) all of the above E) none of the above
D) all of the above
125)--3) Which of the following acids is found in acid rain? A) carbonic acid B) nitric acid C) sulfuric acid D) all of the above E) none of the above
D) all of the above
13) Which of the following illustrates the like dissolves like rule for a solid solute in a liquid solvent? A) An ionic compound is soluble in a polar solvent. B) A polar compound is soluble in a polar solvent. C) A nonpolar compound is soluble in a nonpolar solvent. D) all of the above E) none of the above
D) all of the above
15) Which of the following is a strong acid? A) HCl(aq) (~ 100% ionized) B) H2SO4(aq) (~ 100% ionized) C) HNO3(aq) (~ 100% ionized) D) all of the above E) none of the above
D) all of the above
18) Which of the following is an example of an Arrhenius base? A) NaOH(aq) B) Ca(OH)2(aq) C) Al(OH)3(s) D) all of the above E) none of the above
D) all of the above
21) Which of the following is a strong base? A) LiOH(aq) (~ 100% ionized) B) NaOH(aq) (~ 100% ionized) C) KOH(aq) (~ 100% ionized) D) all of the above E) none of the above
D) all of the above
28) Which of the following increases the rate of dissolving for a solid solute in a solvent? A) grinding the solute B) heating the solution C) stirring the solution D) all of the above E) none of the above
D) all of the above
4) Which of the following illustrates the like dissolves like rule for two liquids? A) A polar solute is miscible with a polar solvent B) A nonpolar solute is miscible with a nonpolar solvent C) A polar solute is immiscible with a nonpolar solvent D) all of the above E) none of the above
D) all of the above
7) Apply the like dissolves like rule to predict which of the following liquids is miscible with water. A) formic acid, HCHO2 B) glycerin, C3H5(OH)3 C) methyl ethyl ketone, C4H8O D) all of the above E) none of the above
D) all of the above
99) Which of the following aqueous solutions is highly ionized? A) strong acid B) strong base C) soluble salt D) all of the above E) none of the above
D) all of the above
122) Beakers W, X, Y, and Z contain either aqueous NaCl, K2SO4, NH4NO3, or H2O. Which beaker contains only distilled water if the light bulb glows brightly when testing the conductivity of beakers W, X, and Y? A) beaker W B) beaker X C) beaker Y D) beaker Z E) all of the above
D) beaker Z
3) Which state of matter has a high density and a definite volume? A) solids B) liquids C) gases D) both solids and liquids E) none of the above
D) both solids and liquids
26) If we supply additional heat to a solid in equilibrium with its liquid at the melting point, the thermal energy added is used to: A) overcome the intermolecular forces that hold the solid together. B) expand the solid. C) change the liquid back to solid. D) change solid to liquid. E) raise the temperature of the solid above its melting point.
D) change solid to liquid.
45) What is the color of phenolphthalein indicator at pH 7? A) red B) blue C) pink D) colorless E) none of the above
D) colorless
47) What is the color of phenolphthalein indicator in pure water? A) red B) blue C) pink D) colorless E) none of the above
D) colorless
25) What happens as you start to add heat to a solid substance? A) Thermal energy causes the components of the solid to vibrate faster. B) When the melting point is reached, the thermal energy is sufficient to overcome intermolecular forces holding the components at their stationary points. C) Increasing the rate of heating of a substance at its melting point only causes more rapid melting. D) If a liquid forms, continued heating results in increasing the liquid temperature. E) all of the above
E) all of the above
4) Which of the following is a general property of a basic solution? A) tastes bitter B) feels slippery C) turns litmus paper blue D) neutralizes acids E) all of the above
E) all of the above
46) Which molecule below has hydrogen bonding? A) NH3 B) CH3OH C) H2O D) HF E) all of the above
E) all of the above
49) Which of the following unit factors is related to a 0.500 M LiF solution? A) 0.500 mol LiF / 1 L solution B) 1 L solution / 0.500 mol LiF C) 0.500 mol LiF / 1000 mol solution D) 1000 mol solution / 0.500 mol LiF E) all of the above
E) all of the above
64) Why is water considered an unusual molecule? A) No molecule of similar size is a liquid at room temperature. B) No molecule of similar size has as high a boiling point. C) Water can dissolve many polar and ionic compounds. D) Water expands upon freezing. E) all of the above
E) all of the above
78) Predict which of the following is a fat-soluble vitamin. A) retinol, vitamin A, C20H30O B) calciferol, vitamin D, C27H44O C) α-tocopherol, vitamin E, C29H50O2 D) vitamin K, C31H46O2 E) all of the above
E) all of the above
79) Predict which of the following is a water-soluble vitamin. A) niacinamide, vitamin B3, C6H6N2O B) pyridoxine, vitamin B6, C8H11NO3 C) cyanocobalamin, vitamin B12, C63H88CoN14O14P D) ascorbic acid, vitamin C, C6H8O6 E) all of the above
E) all of the above
94)---6) What are alternate sources for fluoride besides fluoridated water? A) fluoride tablets B) fluoride toothpaste C) fluoride mouthwash D) fluoride treatments by a dentist E) all of the above
E) all of the above
17) Apply the like dissolves like rule to predict which of the following solids is soluble in hexane, C6H14. A) potassium iodide, KI B) potassium iodite, KIO2 C) potassium iodate, KIO3 D) potassium periodate, KIO4 E) iodine, I2
E) iodine, I2
61) Copper is which type of solid? A) molecular solid B) ionic solid C) covalent atomic solid D) nonbonding atomic solid E) metallic atomic solid
E) metallic atomic solid
109) Acetic acid is a weak acid, ammonium hydroxide is a weak base, and ammonium acetate is a soluble salt. Which of the following is the net ionic equation for the reaction? HC2H3O2(aq) + NH4OH (aq) → NH4C2H3O2(aq) + H2O(l) A) H+(aq) + OH-(aq) → H2O(l) B) C2H3O2-(aq) + NH4+(aq) → NH4C2H3O2(aq) C) H+(aq) + Ba(OH)2(aq) → NH4+(aq) + H2O(l) D) HC2H3O2(aq) + OH-(aq) → C2H3O2-(aq) + H2O(l) E) none of the above
E) none of the above
14) Which of the following illustrates the like dissolves like rule for a solid solute in a liquid solvent? A) An ionic compound is soluble in a nonpolar solvent. B) A polar compound is soluble in a nonpolar solvent. C) A nonpolar compound is soluble in a polar solvent. D) all of the above E) none of the above
E) none of the above
14) Which of the following is an example of an Arrhenius acid? A) Al(OH)3(s) B) Ba(OH)2(aq) C) RbOH(aq) D) H2O(l) E) none of the above
E) none of the above
16) The opposite process of freezing is: A) evaporation. B) sublimation. C) boiling. D) condensation. E) none of the above
E) none of the above
17) Which of the following is a strong acid? A) HNO2(aq) (~ 1% ionized) B) H2SO3(aq) (~ 1% ionized) C) H3PO4(aq) (~ 1% ionized) D) all of the above E) none of the above
E) none of the above
20) Which of the following is an example of an Arrhenius base? A) HNO3(aq) B) H2CO3(aq) C) H3PO4(aq) D) H2O(l) E) none of the above
E) none of the above
23) Which of the following is a weak base? A) Ba(OH)2(aq) (~ 100% ionized) B) Ca(OH)2(aq) (~ 100% ionized) C) Sr(OH)2(aq) (~ 100% ionized) D) all of the above E) none of the above
E) none of the above
29) Which of the following decreases the rate of dissolving for a solid solute in a solvent? A) grinding the solute B) heating the solution C) stirring the solution D) all of the above E) none of the above
E) none of the above
3) Which of the following is a general property of an acidic solution? A) tastes bitter B) feels slippery C) turns litmus paper blue D) neutralizes acids E) none of the above
E) none of the above
44) Which statement below is FALSE? A) A hydrogen bond is the strongest of the intermolecular forces. B) A hydrogen atom must be bonded directly to fluorine, oxygen, or nitrogen to exhibit hydrogen bonding. C) The large electronegativity difference between hydrogen and an F, O, or N atom is essential for the formation of a hydrogen bond. D) A hydrogen bond is only 2-5% the strength of a typical covalent bond. E) none of the above
E) none of the above
9) Apply the like dissolves like rule to predict which of the following liquids is immiscible with water. A) acetic acid, CH3COOH B) acetone, C3H6O C) methanol, CH3OH D) all of the above E) none of the above
E) none of the above
11) If a drain cleaner has a pH of 14, the solution is which of the following? A) strongly acidic B) weakly acidic C) neutral D) weakly basic E) strongly basic
E) strongly basic
30) Paradichlorobenzene, a material used in "moth balls," is known to go directly from a solid form to a gaseous form. This process is known as: A) melting B) evaporation C) condensation D) boiling E) sublimation
E) sublimation