chem

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____    1.   According to the kinetic-molecular theory, gases condense into liquids because of

____    2.   An ideal gas is a hypothetical gas

____    3.   A real gas

____    4.   What determines the average kinetic energy of the molecules of any gas?

____    5.   Which is an example of gas diffusion?

____    6.   Which substance has the lowest density?

____    7.   What happens to the volume of a gas during compression?

____    8.   Under which conditions do real gases most resemble ideal gases?

____    9.   The particles in a liquid are usually

____  10.   Which of these best describes vaporization?

____  11.   Which term best describes the process by which particles escape from the surface of a nonboiling liquid and enter the gas state?

____  12.   Particles within a solid

____  13.   Forces holding particles together are strongest in a

____  14.   At about what temperature does water reach its maximum density?

____  15.   Which of the following is a homogeneous mixture?

____  16.   Which of the following is a homogeneous mixture of substances in a single phase?

____  17.   Increasing the surface area of the solute

____  18.   Stirring increases the rate of dissolution because it

____  19.   In a solution at equilibrium,

____  20.   The solubility of a substance at a given temperature is generally expressed as

____  21.   Solubilities, expressed as grams/100. g of water,

____  22.   The rate of dissolution is

____  23.   In the expression "like dissolves like," the word like refers to similarity in molecular

____  24.   What is the molality of a solution that contains 5.10 mol KNO₃ in 4.47 kg water? (molar mass of KNO₃ = 101.11 g/mol)

____  25.   What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (molar mass of NaCl = 58.44 g/mol)

____  26.   What is the molality of a solution that contains 31.0 g HCl in 5.00 kg water? (molar mass of HCl = 36.46 g/mol)

____  27.   How many moles of HCl are present in 0.70 L of a 0.33 M HCl solution? (molar mass of HCl = 36.46 g/mol)

____  28.   The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much NaCl is in the solution? (molar mass of NaCl = 58.44 g/mol)

____  29.   An NaOH solution contains 1.90 mol of NaOH, and its concentration is 0.555 M. What is its volume? (molar mass of NaOH = 40.00 g/mol)

____  30.   What mass of water must be used to make a 1.35 m solution that contains 8.20 mol of NaOH? (molar mass of NaOH = 40.00 g/mol)

____  31.   How many milliliters of a 0.171 M solution contain 1.00 g of NaCl? (molar mass of NaCl = 58.44 g/mol)

____  32.   A reaction in which products can react to re-form reactants is

____  33.   Under suitable conditions, roughly what proportion of all chemical reactions are reversible?

____  34.   At equilibrium,

____  35.   What two processes are at equilibrium in a saturated sugar solution?

____  36.   At equilibrium, the total amount of the product(s)

____  37.   What symbol represents the equilibrium constant?

____  38.   A very low value of K indicates that

____  39.   A very high value of K indicates that

____  40.   A value of K near 1 indicates that at equilibrium probably

____  41.   In the equation , what represents the concentrations of the reactants?

____  42.   In the equation, what represents the concentrations of the products?

____  43.   What is the chemical equilibrium expression for the equation

2A₂B + 3CD  A₄D + C₃B₂?

____  44.   An equilibrium mixture of SO₂, O₂, and SO₃ gases at 1500 K is determined to consist of 0.344 mol/L SO₂, 0.172 mol/L O₂, and 0.56 mol/L SO₃. What is the equilibrium constant for the system at this temperature? The balanced equation for this reaction is

2SO₂(g) + O₂(g)  2SO₃(g).

____  45.   If the system 2CO(g) + O₂(g)  2CO₂(g) has come to equilibrium and then more CO(g) is added,

____  46.   If the pressure on the equilibrium system 2CO(g) + O₂(g)  2CO₂(g) is increased,

____  47.   If the temperature of the equilibrium system CH₃OH(g) + 101 kJ  CO(g) + 2H₂(g) increases,

____  48.   If more CO(g) is added to the system 2CO(g) + O₂(g)  2CO₂(g) at constant temperature, K

____  49.   The common-ion effect promotes

____  50.   The common-ion effect is a consequence of

____  51.   What is the acid-ionization expression for the ionization of acetic acid, shown in the reaction represented by the equation CH₃COOH(aq) + H₂O(l)  H₃O⁺(aq) + CH₃COOH^–(aq)?

____  52.   To what degree does water ionize?

____  53.   What is the value of the ion-product constant for water?

____  54.   What is the symbol for the ion-product constant for water?

____  55.   An example of a good buffer is

____  56.   The anion of the salt of a weak acid and a strong base is the

____  57.   The cation of the salt of a strong acid and a weak base is the

____  58.   What is the solubility-product constant of magnesium hydroxide, Mg(OH)₂? Its solubility is 9.0 ´ 10^–4 g/100 g H₂O. The molar mass of Mg(OH)₂ is 58.32 g/mol.

____  59.   What is the solubility in mol/L of silver iodide, AgI? Its K_sp value is 8.3 ´ 10^–17.

____  60.   What is the solubility in mol/L of calcium carbonate, CaCO₃? Its K_sp value is

1.4 ´ 10^–8.

____  61.   Calculate the ion product for mixing 100.0 mL of 0.0030 M CaCl₂ with 100 mL of 0.0020 M Na₂CO₃. K_sp for CaCO₃ is 1.4  10^–8. Does a precipitate form?

____  62.   Acids generally release H₂ gas when they react with

____  63.   Acids react with

____  64.   Bases feel

____  65.   Bases react with

____  66.   Which of the following is a binary acid?

____  67.   Which of the following is not an oxyacid?

____  68.   Which of the following is perchloric acid?

____  69.   Which of the following is chlorous acid?

____  70.   Which acid is produced in the stomach?

____  71.   An Arrhenius acid contains

____  72.   Which of the following is not a strong acid?

____  73.   Which of the following is a weak base?

____  74.   Which of the following is a strong base?

____  75.   Which of the following is a triprotic acid?

____  76.   A Brønsted-Lowry acid is a(n)

____  77.   In the equation HCl(g) + H₂O(l) ® H₃O⁺(aq) + Cl^–(aq), which species is a Brønsted-Lowry acid?

____  78.   A Lewis acid is

____  79.   An electron-pair donor is a

____  80.   A conjugate acid is the species that

____  81.   A species that remains when an acid has lost a proton is a

____  82.   In the reaction represented by the equation   , a conjugate acid-base pair is

____  83.   In the reaction represented by the equation   , a conjugate acid-base pair is

____  84.   The conjugate of a strong acid is a

____  85.   Which of the following is amphoteric?

____  86.   In the reaction represented by the equation    acts as a(n)

____  87.   In the reaction represented by the equation    acts as a(n)

____  88.   In the reaction represented by the equation     acts as a(n)

____  89.   What is the concentration of H₃O⁺ ions in pure water?

____  90.   Which expression represents the concentration of H₃O⁺ ions in solution?

____  91.   Which expression represents the pH of a solution?

____  92.   What is the pH of a neutral solution at 25ºC?

____  93.   The pH scale in general use ranges from

____  94.   The pH of an acidic solution is

____  95.   The pH of a basic solution is

____  96.   What is the pH of a 10^–5 M KOH solution?

____  97.   If [H₃O⁺] = 1.7 ´ 10^–3 M, what is the pH of the solution?

____  98.   If [H₃O⁺] = 8.26 ´ 10^–5 M, what is the pH of the solution?

____  99.   What is the pH of a 0.027 M KOH solution?

____ 100.   What is the pH of a 0.001 62 M NaOH solution?