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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