Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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A substance that does NOT conduct an electric current when it forms a solution
is a(n) ____.
a. | electrolyte | c. | liquid | b. | nonelectrolyte | d. | solid |
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2.
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A solution that contains all of the solute it can hold at a given temperature is
____.
a. | diluted | c. | supersaturated | b. | saturated | d. | unsaturated |
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3.
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When a gas is dissolved in a liquid, the gas dissolves faster if the liquid is
____.
a. | cooled | c. | heated | b. | an electrolyte | d. | under low
pressure |
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4.
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Which of the following combinations would increase the solubility of a gas in a
liquid?
a. | Decrease the pressure and decrease the temperature. | b. | Decrease the
pressure and increase the temperature. | c. | Increase the pressure and decrease the
temperature. | d. | Increase the pressure and increase the temperature. |
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5.
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Which of the following will speed up the dissolving of a solid solute in
water?
a. | Cool the solution. | c. | Grind up the solvent. | b. | Freeze the
solute. | d. | Stir the
solution. |
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6.
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A substance that speeds up a chemical reaction without being permanently changed
itself is a(n) ____.
a. | catalyst | c. | inhibitor | b. | coefficient | d. | reactant |
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7.
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____ change color in the presence of an acid or a base.
a. | Acids | c. | Buffers | b. | Glycerins | d. | Indicators |
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8.
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Coffee has a pH of about 5. Coffee is ____.
a. | extremely acidic | c. | somewhat acidic | b. | extremely basic | d. | somewhat basic |
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9.
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Increasing the surface area of a solid ____.
a. | causes the solid to ionize | c. | slows the rate of
solution | b. | has no effect on the rate of solution | d. | speeds the rate of
solution |
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10.
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Increasing temperature generally increases the solubility of a solute in a
solvent.
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11.
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In a solution, the substance that is being dissolved is the ____.
a. | gas | c. | solute | b. | liquid | d. | solvent |
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12.
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If two liquids are soluble in each other, they are said to be _____.
a. | soluble | c. | miscible | b. | insoluble | d. | immiscible |
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13.
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The substance in a solution that dissolves another substance is called
___.
a. | solute | c. | electrolyte | b. | solvent | d. | nonelectrolyte |
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14.
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According to the graph above, about how many grams of KBr are needed to make a
saturated soultion in 100 g of water at 30° C?
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15.
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According to the graph above, which salt is more soluble in water KCl or
KBr?
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16.
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According to the graph above, at what temperature is the solubility of KBr the
same as KNO3?
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17.
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According to the graph above, what kind of solution would you have if you
dissolved 10 g of KCl in 100 g of water at 0°C?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | polysaturated |
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18.
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According to the graph above, which of the following substance’s
solubility increases the least as temperature goes up?
a. | potassium nitrate | c. | potassium chloride | b. | potassium bromide | d. | sodium chloride |
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19.
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According to the graph, how many grams of KCl wil form a saturated solution in
100 g of water at 60°C?
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SOLUBILITY OF SUBSTANCES IN WATER AT
20°C | Solid Substances | Solubility in g/100 g of
Water | Barium sulfate
Lithium carbonate
Potassium chloride
Sodium
nitrate
Lithium bromide | 0.00025
1.3
34.0
87.6
166.0 | | |
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20.
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According to the chart above, what type of solution would you have if 1.5 g of
lithium carbonate is dissolved in 100 g of water at 20 °C?
a. | saturated | c. | unsaturated | b. | supersaturated | d. | polysaturated |
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21.
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According to the chart above, what type of solution would you have if 166.0 g of
lithium bromide is dissolved in 100 g of water at 20 °C?
a. | saturated | c. | unsaturated | b. | supersaturated | d. | polysaturated |
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22.
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A mixture with particles that will settle out if left undisturbed is a(n)
___.
a. | suspension | c. | colloid | b. | emulsion | d. | electrolyte |
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23.
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A solution in which the solvent is water is called ___.
a. | concentrated | c. | aqueous | b. | dilute | d. | amphoteric |
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24.
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A solution is made by dissolving 17.0 g of Lithium iodide in enough water to
make 500.0 mL of solution. What is the molarity of the solution?
a. | 34 M | c. | 0.25 M | b. | 0.034 M | d. | 2.54 x
10-4 |
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25.
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Calculate the molarity of a water soluiton of CaCl2 made by
dissolving 612 g of CaCl2 in 5.04 L of solution.
a. | 1.09 M | c. | 0.775 M | b. | 22.0 M | d. | 1.88 M |
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26.
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What is the molarity of an aqueous solution containing 40.0 g of glucose
(C6H12O6) in 1.5 L of solution?
a. | 27 M | c. | 0.22 M | b. | 60 M | d. | 0.15 M |
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27.
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What is the molarity of an aqueous solution containing 14.2 g of NaCl dissolved
in 2000 mL of solution?
a. | 7.1 M | c. | 0.12 M | b. | 0.24 M | d. | 3.6 M |
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28.
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____________ are the products of a neutralization reaction between a strong acid
& a strong base.
a. | water & acid | c. | water & salt | b. | base & salt | d. | acid & base |
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29.
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A ___ solution contains more hydroxide ions that it does hydrogen ions.
a. | acidic | c. | neutral | b. | basic | d. | saturated |
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30.
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Since nitric acid is a ____ acid, it ionizes completely in solution
a. | concentrated | c. | strong | b. | dilute | d. | weak |
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31.
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The negative logarithm of the hydrogen ion concentration is ___.
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32.
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The substances produced when KOH neutralizes HCl are
a. | KH + ClOH | c. | KClH + OH | b. | KCl + H2O | d. | HOH +
KCl2 |
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33.
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Which expression represents the pH of a solution?
a. | log [H+] | c. | antilog
[-pOH] | b. | - log [H+] | d. | -antilog
[pOH] |
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34.
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Which is a strong base?
a. | H2O | c. | NaOH | b. | CH4 | d. | HCH3COO |
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35.
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The formula for the products between sodium hydroxide and sulfuric acid are
___.
a. | NaSO4 + H2O | c. | NaS2 +
H2O | b. | Na2SO4 + H2O | d. | NaH + SOH |
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36.
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If 50.0 ml of a 0.500 M solution of HCl is diluted to 150.0 ml, what will the
final molarity be?
a. | 0.667 | c. | 1.50 | b. | 5.99 | d. | 0.167 |
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37.
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What would the final volume of a solution be if 5.0 mL of a 0.040 M stock
solution is diluted to 0.030 M?
a. | 6.67 | c. | 0.00244 | b. | 0.150 | d. | 416 |
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38.
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What explains the solubility of ionic substances in water?
a. | water is polar | c. | water is poly polar | b. | water is nonpolar | d. | water dissolves
everything |
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39.
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A chemist is having some difficulty getting a yellow crystalline solid compound
to dissolve in water. What strategy might she employ to increase the solubility of the
solid?
a. | heat the solution | c. | shake it | b. | grind up the solid | d. | all of these would
work |
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40.
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A student pours a sample of a clear liquid – whose identify is unknown
– into a test tube of water. The water and the liquid form two distinct layers, with the
unknown on the bottom. What is true of the system?
a. | the two solutions are miscible | c. | the density of the unknown liquid
is less dense than the water | b. | the unknown solution is non
polar | d. | the two are soluble
in each other |
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41.
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Weak acids and bases produce what type of ions in solution?
a. | many | c. | H+ ions only | b. | only a few | d. | OH- ions
only |
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42.
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A substance that slows down a chemical process is called what?
a. | exothermic | c. | inhibitor | b. | endothermic | d. | catalyst |
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43.
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What happens to the rate of a reaction if the temperature is lowered?
a. | it speeds up | c. | it stays the same | b. | it slows down |
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44.
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What is the minimum energy required for an effective collision called?
a. | joule | c. | kinetic energy | b. | calorie | d. | activation
energy |
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45.
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What is the primary reason that an increase in temperature results in an
increase in reaction rates?
a. | it has greater potential energy | c. | there are less
calories | b. | it has greater kinetic energy | d. | the molecules hit each other
less |
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46.
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To react, what must gas particles do?
a. | bounce off each other | c. | collide with opposing orientation
| b. | collide with the correct orientation | d. | get close to each
other |
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47.
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To slow down the rate of reaction, what would you do?
a. | increase the concentration of the reactants | c. | lower the
temperature | b. | increase the surface area of the reactants | d. | adding a
catalyst |
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48.
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Which energy difference in the reaction profile
below corresponds to the activation energy for the forward reaction?
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49.
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What type of solution that contains less solute than it is able to hold at a
given temperature?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly satuated |
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50.
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What type of solution that contains more solute than it can hold at a given
temperature?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly saturated |
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51.
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What is the general rule for solubility?
a. | like dissolves unlike | c. | like dissolves like | b. | unlike dissolves unlike | d. | unlike dissolves
like |
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52.
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If a crystal is added to an aqueous solution and it causes many crystals to come
out of the solution, what type of solution was it originally?
a. | saturated | c. | supersaturated | b. | unsaturated | d. | poly saturated |
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53.
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What term refers to the ease with which an acid or base forms ions in
solution?
a. | pH | c. | base | b. | acid | d. | strength |
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54.
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What type of solution contains more hydrogen ions than it does hydroxide
ions?
a. | acid | c. | neutral | b. | base | d. | amphoteric |
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55.
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What will increase the rate of reaction?
a. | lower the temperature | c. | stir | b. | decreast the surface area | d. | grind up the
solvent |
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56.
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What will happen to the rate of reaction if the surface area of reactants is
increased?
a. | speed up | c. | remains constant | b. | slow down | d. | unable to tell with this
information |
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57.
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What is the molarity of a solution made by dissolving 34.0 g of sodium chloride
(NaCl) in enough water to make 500 mL of solution?
a. | 0.068 | c. | 1.16 | b. | 68 | d. | 0.00232 |
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58.
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Calculate the molarity of a water solution of KCl, given that 2.50 L of the
solution contains 350 g of KCl.
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59.
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What would the final volume of a solution be if 25.0 mL of a 1.0 M stock
solution is diluted to
0.50 M?
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60.
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What is the molarity of a solution containing 9.0 moles of a solute in 500.0 mL
of solution?
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61.
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What would the final volume of a solution be if 6.0 mL of a 0.050 M stock
solution is diluted to
0.020 M?
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62.
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If 40.0 ml of a 0.400 M solution of HCl is diluted to 50.0 ml, what will the
final molarity be?
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63.
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When one element replaces another element in a compound, the reaction is a ____
reaction.
a. | decomposition | c. | single–displacement | b. | double–displacement | d. | synthesis |
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64.
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What type of reaction is shown in the following chemical equation:
2H2O ® 2H2 + O2?
a. | decomposition | c. | single–displacement | b. | double–displacement | d. | synthesis |
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65.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
If 3.0 moles of potassium chlorate
are used, how many moles of water would be produced?
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66.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
If 25.0 g of carbon dioxide
are produced, how many grams of sugar (C12H22O11) were used?
a. | 0.0473 | c. | 16.2 | b. | 21.1 | d. | 0.0617 |
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67.
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8 KClO3 +
C12H22O11 ® 8 KCl
+ 12 CO2 + 11 H2O
How many grams of sugar
(C12H22O11) were oxidized by the potassium chlorate, if 3.16 g of
water were produced?
a. | 0.183 | c. | 62.7 | b. | 0.0159 | d. | 5.46 |
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68.
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8 KClO3 +
C12H22O11 ®8 KCl +
12 CO2 + 11 H2O
How many moles of potassium chlorate
are required to produce 18.0 g of water?
a. | 89.0 | c. | 54.1 | b. | 0.726 | d. | 6.72 |
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69.
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What is a reaction in which oxygen combines with a substance and releases heat
and light known as?
a. | single replacement | c. | synthesis | b. | double replacement | d. | combustion |
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70.
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Ammonia (NH3) is used to make fertilizer. If you have 2.00 x 10
3g of N2 how many grams of ammonia can be
produced?
N2 +
3H2 à
2NH3
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71.
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Calculate the number of moles in 250.0g of potassium chlorate
(KClO3).
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72.
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Determine the molar mass of KC2H3O2.
a. | 68.12 | c. | 86.14 | b. | 98.15 | d. | 82.15 |
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73.
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Determine the number of moles in 25.50 g Ag.
a. | 0.236 | c. | 3.64 x 10-4 | b. | 2750 | d. | 4.24 |
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74.
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Given 3.25 mol of AgNO3, determine the number of formula
units.
a. | 0.0191 | c. | 1.96 x 1024 | b. | 5.40 x
10-24 | d. | 52.4 |
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75.
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Given the following combustion reaction of a hydrocarbon, balance the equation
and determine the coefficient of
H2O.
C4H6 + O2 ®
CO2 + H2O
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76.
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How many atoms of Cu are in 4.00 moles?
a. | 254 | c. | 2.41 x 1024 | b. | 0.00393 | d. | 6.64 x
10-24 |
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77.
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How many grams of CCl4 are in 4.00 moles? The formula mass of
carbon tetrachloride is 153.8 g/mol.
a. | 0.026 | c. | 2.41 x 1024 | b. | 615 | d. | 4.15 x
10-25 |
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78.
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How many grams of CH3Br could be made from 10.0 g of CH3OH
and excess PBr3?
3 CH3OH +
PBr3 à 3
CH3Br + P(OH)3
a. | 23.4 | c. | 4.27 | b. | 0.0428 | d. | 0.234 |
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79.
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How many grams of ZnCl2 are produced from 75.00 g of ZnO in the
reaction
ZnO + 2HCl ® ZnCl2 + H2O ?
a. | 44.79 | c. | 125.6 | b. | 0.0223 | d. | 0.00796 |
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80.
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How many hydrogen atoms are there in 1.0 x 102 g of glucose,
C6H12O6?
a. | 0.555 | c. | 3.34 x 1023 | b. | 4.01 x
1024 | d. | 2.49 x
10-25 |
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81.
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How many moles are in 1.2 X 1024 molecules of water?
a. | 0.503 | c. | 7.72 x 1047 | b. | 1.38 x
10-48 | d. | 1.99 |
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82.
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How many moles of CH3Br could be made from 3.0 moles of
PBr3 and excess
CH3OH?
3 CH3OH +
PBr3 à 3
CH3Br + P(OH)3
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83.
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In the equation HCl + KOH ® KCl +
H2O, how many grams of water are produced if 3.000 moles of HCl are used?
a. | 0.166 | c. | 54.06 | b. | 6.01 | d. | 0.0185 |
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84.
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In the reaction 2Na + Cl2 ®
2NaCl, how many grams of sodium chloride can be produced from 120.0 g of sodium in the presence
of excess chlorine?
a. | 305 | c. | 0.0212 | b. | 47.2 | d. | 0.00328 |
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85.
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One in a series of reactions that inflates airbags in automobiles is the
decomposition of sodium azide
(NaN3).
2 NaN3 (s) ® 2 Na (s)
+ 3 N2 (g)
Determine
the mass of N2 produced if 1.00 x 102 g NaN3 is decomposed.
a. | 21.5 | c. | 0.00215 | b. | 464 | d. | 64.64 |
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86.
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What is the coefficient that belongs in front of carbon dioxide in the
equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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87.
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What is the correct molar mass of Ca(OH)2 ?
a. | 74.1 | c. | 58.11 | b. | 57.09 | d. | 60.75 |
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88.
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The
following reaction is an example of which type of reaction?
AgNO3(aq) + NaCl
(aq) ® AgCl(s)
+ NaNO3(aq)a. | synthesis | c. | single replacement | b. | decomposition | d. | double
replacement |
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89.
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What is the formula mass of (NH4)3PO4?
a. | 121.1 | c. | 144.07 | b. | 149.12 | d. | 153.20 |
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90.
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The molar mass of CO2 is 44 g/mol. How many moles are present
in 110 g?
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91.
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The molar mass of H2O is 18.015 g/mol. How many moles of water
are present in 3.6 g?
a. | 0.015 | c. | 5.00 | b. | 64.85 | d. | 0.20 |
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92.
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The molar mass of NH3 is 17.0 g/mol. How many grams of NH3
are present in 3.50 moles?
a. | 59.5 | c. | 0.210 | b. | 0.0170 | d. | 4.85 |
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93.
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What type of reaction is 2Hg + O2 ®
2HgO?
a. | single replacement | c. | synthesis | b. | double replacement | d. | decomposition |
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94.
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What are the coefficients to correctly balance the formula equation
Pb(NO3)2 (aq) + KI (aq) ® PbI2 (s) + KNO3(aq)
a. | 1 2 1 2 | c. | 1 4 1 4 | b. | 2 1 2 1 | d. | 4 1 4 1 |
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95.
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What are the coefficients to correctly balance the formula equation
AlCl3(aq) + Pb(NO3)2(aq) ® PbCl2(s) +
Al(NO3)3(aq)
a. | 3 2 3 2 | c. | 1 7 4 2 | b. | 2 3 3 2 | d. | 5 1 1 2 |
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96.
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What is the balanced equation when aluminum reacts with
copper(II)sulfate?
a. | Al + CuSO4 ® Cu +
AlSO4 | c. | 4Al + 3Cu2(SO4)2 ®
6Cu + 2Al2(SO4)3 | b. | 2Al + 3CuSO4 ® 3Cu + Al2(SO4)3 | d. | 2Al +
Cu2(SO4)2 ® 2Cu +
2AlSO4 |
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97.
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What volume of oxygen is needed to completely combust 2.36 L of methane gas
(CH4)?
CH4 (g) + 2 O2
(g) ®CO2
(g) + 2 H2O (g)
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98.
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What is the coefficient that belongs in front of oxygen in the equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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99.
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What is the coefficient that belongs in front of water in the equation?
____C3H8 + ___O2 ®
____CO2 + ___H2O
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100.
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What are the coefficients to correctly balance the formula
equation?
Al2(SO4)3 + KOH à Al(OH)3 +
K2SO4
a. | 2,3,3,2 | c. | 1,6,2,3 | b. | 3,2,3,2 | d. | 2,6,3,1 |
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101.
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What are the coefficients to correctly balance the formula equation?
Cr + Fe(NO3)2 à
Fe + Cr(NO3)3
a. | 2,3,3,2 | c. | 3,2,2,3 | b. | 3,2,3,2 | d. | 1,3,3,1 |
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102.
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The following reaction : Cr +
Fe(NO3)2 à Fe +
Cr(NO3)3, can be classified as what type of
reaction?
a. | synthesis | c. | single replacement | b. | decomposition | d. | double
replacement |
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