Integrated Science TEST: Chemical Reactions, Acids and Bases (mrk 2012)
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____1.The substances that undergo change in a chemical reaction are called
a. / reactants. / c. / coefficients.b. / products. / d. / elements.
____2.The substances that are formed as a result of a chemical reaction are called
a. / products. / c. / coefficients.b. / reactants. / d. / elements.
____3.Hydrochloric acid, HCl, is added to solid NaOH. After the reaction is complete, NaCl dissolved in water remains. What are the products of this chemical reaction?
a. / NaOH and HCl / c. / HCl and NaClb. / NaOH and H2O / d. / NaCl and H2O
____4.Which of the following does NOT state what the arrow means in a chemical equation?
a. / forms / c. / conservesb. / produces / d. / yields
____5.Which of the following does NOT show the law of conservation of mass?
a. / 24 g of Mg burn in 32 g O2 to produce 56 g of MgO.b. / 24 mL of Mg burn in 32 mL O2 to produce 56 mL of MgO.
c. / 2 atoms of Mg react with 1 molecule of O2 to produce 2 units of MgO.
d. / 1 atom of Mg reacts with 1 atom of O to produce a unit of MgO that contains 2 atoms.
____6.Which of the following is a chemical equation that accurately represents what happens when sulfur and oxygen react to form sulfur trioxide?
a. / Sulfur and oxygen react to form sulfur trioxide.b. / S and O2 produce SO3.
c. / S + O2 SO3
d. / 2S + 3O22SO3
____7.Which of the following is a balanced chemical equation for the synthesis of NaBr from Na and Br2?
a. / Na + Br2 NaBrb. / 2Na + Br2 NaBr
c. / Na + Br2 2NaBr
d. / 2Na + Br2 2NaBr
____8.Methane, CH4, burns in oxygen gas to form water and carbon dioxide. What is the correct balanced chemical equation for this reaction?
a. / CH4 + O H2O + CO2b. / CH4 + 4O 2H2O + CO2
c. / CH4 + O2 H2O + CO2
d. / CH4 + 2O2 2H2O + CO2
____9.How many atoms are present in 3 moles of chromium?
a. / 6.02 1023 atoms / c. / 1.80 1024 atomsb. / 1.80 1023 atoms / d. / 52.0 atoms
____10.How many grams of CO2 are in 2.1 mol of the compound?
a. / 21.0 g / c. / 66.0 gb. / 44.0 g / d. / 92.4 g
____11.How many moles of He are in 16 g of the element?
a. / 1.0 mol / c. / 8.0 molb. / 4.0 mol / d. / 16 mol
____12.An industrial process makes calcium oxide by decomposing calcium carbonate. Which of the following is NOT needed to calculate the mass of calcium oxide that can be produced from 4.7 kg of calcium carbonate?
a. / the balanced chemical equationb. / molar masses of the reactants
c. / molar masses of the product
d. / the volume of the unknown mass
____13.The coefficients in a balanced chemical equation always can express the ratio of
a. / moles of reactants and products.b. / volume of reactants and products.
c. / atoms of reactants and products.
d. / mass of reactants and products.
____14.When magnesium carbonate, MgCO2, reacts with nitric acid, HNO3, magnesium nitrate and carbonic acid form. Carbonic acid then breaks down into water and carbon dioxide. Which two types of reactions take place in this process?
a. / synthesis and decompositionb. / single-replacement and combustion
c. / double-replacement and decomposition
d. / double-replacement and combustion
____15.Which of the following is NOT always true about a synthesis reaction?
a. / One product is formed.b. / There is only one reactant.
c. / The general formula is A + B C.
d. / A reactant might be a compound, or it might be an element.
____16.Which of the following is the general formula for a synthesis reaction?
a. / The general formula is A B + C.b. / The general formula is AB + C CB + A.
c. / The general formula is A + B C.
d. / The general formula is AB + CD AD + BC
____17.Which of the following is the general formula for a decomposition reaction?
a. / The general formula is A B + C.b. / The general formula is AB + C CB + A.
c. / The general formula is A + B C.
d. / The general formula is AB + CD AD + BC
____18.Which of the following is the general formula for a single-replacement reaction?
a. / The general formula is A B + C.b. / The general formula is AB + C CB + A.
c. / The general formula is A + B C.
d. / The general formula is AB + CD AD + BC
____19.Which of the following is the general formula for a double-replacement reaction?
a. / The general formula is A B + C.b. / The general formula is AB + C CB + A.
c. / The general formula is A + B C.
d. / The general formula is AB + CD AD + BC
____20.Which of the following takes place during a redox reaction?
a. / Electrons are gained only.b. / Electrons are lost only.
c. / Electrons are both gained and lost.
d. / Electrons are neither gained nor lost.
____21.In a chemical reaction, an iron atom became the ion Fe2+. What happened to the iron atom?
a. / It lost electrons and was oxidized.b. / It lost electrons and was reduced.
c. / It gained electrons and was oxidized.
d. / It gained electrons and was reduced.
____22.The total amount of energy before and after a chemical reaction is the same. Thus, energy, like mass, is
a. / created. / c. / conserved.b. / destroyed. / d. / the same as mass.
____23.Which of the following is NOT a property of an acid?
a. / tastes sour / c. / changes the color of an indicatorb. / usually reacts with a metal / d. / feels slippery
____24.A girl tasted each of the following foods. Which of the following would NOT taste acidic to her?
a. / lime / c. / orangeb. / tomato / d. / celery
____25.A student had each of the following items in a grocery cart. Which of the following items would be basic?
a. / lime / c. / soapb. / tomato / d. / celery
____26.A base is defined as a compound that produces
a. / hydroxide ions in solution. / c. / hydronium ions in solution.b. / hydrogen ions in solution. / d. / sodium ions in solution.
____27.Which of the following is NOT a common property of bases?
a. / feels slippery / c. / reacts with metalsb. / tastes bitter / d. / changes colors of indicators
____28.The products of the neutralization reaction between hydrochloric acid and magnesium hydroxide are
a. / MgCl and H2O. / c. / HCl and MgOH.b. / MgCl2 and H2O. / d. / HCl and Mg(OH)2.
____29.The salt that is formed during the reaction between potassium hydroxide and hydrochloric acid is
a. / NaCl. / c. / KCl.b. / H2O. / d. / K2Cl.
____30.An acid can be defined as
a. / a proton acceptor.b. / a proton donor.
c. / neither a proton donor nor a proton acceptor.
d. / both a proton donor and a proton acceptor.
____31.An base can be defined as
a. / a proton acceptor.b. / a proton donor.
c. / neither a proton donor nor a proton acceptor.
d. / both a proton donor and a proton acceptor.
____32.Ammonia, NH3, can be classified as a base because in a chemical reaction with an acid, ammonia will
a. / produce hydroxide ions in solution. / c. / donate a proton and become NH2.b. / produce hydronium ions in solution. / d. / accept a proton and become NH4+.
____33.Distilled water has a hydronium ion concentration of 1 107 M. What is the pH of a distilled water?
a. / 7 / c. / 10b. / 7 / d. / 1 107
____34.The hydroxide ion concentration in pure water at 25ºC is NOT equal to
a. / the hydronium ion concentration.b. / 1 107 M.
c. / the hydroxide concentration in a solution with a pH of 7.
d. / 1 107 M.
____35.A compound has a pH of 6 in solution, where very little of it has ionized. The compound is a
a. / weak base. / c. / weak acid.b. / strong base. / d. / strong acid.
____36.Calcium hydroxide forms very few hydroxide ions in solution, but it is still considered a strong base because
a. / calcium hydroxide is insoluble.b. / all the calcium hydroxide in solution ionizes.
c. / all the calcium hydroxide in solution dissociates.
d. / very little of the calcium hydroxide in solution ionizes.
____37.Which of the following would NOT form a buffer solution?
a. / NH3 + NH4Cl / c. / HCl + NaClb. / HC2H3O2 + NaC2H3O2 / d. / H2CO3 + NaHCO3
____38.A small amount of acid is added to a buffer solution. The pH of the solution will
a. / increase. / c. / stay about the same.b. / decrease. / d. / become neutral.
____39.A substance that ionizes or dissociates into ions when placed in water is always a(an)
a. / conductor. / c. / strong acid.b. / electrolyte. / d. / strong base.
____40.Which of the following are examples of strong electrolytes?
a. / strong and weak bases / c. / weak acids and weak basesb. / strong acids and strong bases / d. / pure water and buffers
Completion
For # 41 - 60, complete each statement using the word bank below. If the answer is a letter combination, darken all of the letters that make up the combination on the Scantron answer sheet. One of the words is used twice but not all of the words are used.
a. 3 molesae. oxygenabd. acid
b. 12 gbc. hydromium ions abe. weak
c. potassium nitratebd. 7acd. oxidation
d. reductionbe. 3g/molace. electrolyte
e. 160 g/molcd. coefficientade. synthesis
ab. conservationce. 12g/mol abcd. ionize
ac. twode. C + BAabce. reduction
ad. 160 g abc. 24 molesacde. dissociating
41.The statement that in chemical reactions, the total mass of the reactants equals the total mass of the products is the law of ______of mass or energy.
42.In an experiment, 44 g of propane was burned, producing 132 g of carbon dioxide and of water. The mass of oxygen that was needed for the reaction was ______.
43.A(An) ______is the number that appears before a formula in a chemical equation.
44.The molar mass of carbon is ______.
45.A sample of NaCl contains 174 g of the compound. The sample contains ______of NaCl.
46.Butane burns as shown in the balanced chemical equation 2C4H10 + 13O2 10H2O + 8CO2. If 6 mol of butane burn, ______of carbon dioxide are produced.
47.An iron fence is left unpainted, and it reacts with the oxygen in the air, forming rust. The formation of rust is an oxidation-reduction reaction, but it is also an example of a(an) ______reaction.
48.Single-replacement reactions can take place with nonmetals. In the following equation, assume that A and C are nonmetals and B is a metal. Complete the following general equation for the replacement of a nonmetal in a compound by another nonmetal: A + BC ______.
49.The element ______is always present in a combustion reaction.
50.In a double-replacement reaction, there are two reactants and ______product(s).
51.When fluorine reacts with a metal, it forms an F– ion. The fluorine atom has gained an electron and undergone ______.
52.An acid produces ______when it is dissolved in water.
53.Most acids form ions in solution by ionizing, and most bases form ions in solution by ______.
54.The products of the reaction between potassium hydroxide, KOH, and nitric acid, HNO3, are ______and water.
55.When a substance donates a proton during a chemical reaction, that substance can be classified as a(an) ______.
56.The concentration of hydronium ions in the solution is 1 107M. What is the pH?
57.The pH of a solution describes the concentration of ______in solution.
58.Acids that contain carbon are weak acids, which means that they ______only to a small extent in solution.
59.Many foods are acidic. These foods do not hurt you when you eat them because they contain ______acids.
60.Acetic acid is considered a weak ______because it only partially ionizes.
Other
USING SCIENCE SKILLS
Figure 7-2
61.Interpreting Graphics How many oxygen atoms are on the left side of the equation? How many oxygen atoms are on the right side of the equation?
a. 1; 4b. 2; 3c. 3; 2d. 1; 1
62.Inferring If the total number of atoms on the left side of the equation in Figure 7-2 equaled the total number of atoms on the right side of the equation, would this necessarily mean that the equation was balanced?
a. yesb. no
63.Drawing Conclusions If there are 4 hydrogen atoms on the left side of equation in Figure 7-2, how many hydrogen atoms must there be on the right side in order to balance this reaction?
a. 1b. 2c. 3d. 4
64.Problem Solving How do you balance the number of hydrogen atoms in the equation in Figure 7-2?
a. Place a coefficient of 2 in front of carbon dioxide on the right side.
b. Place a coefficient of 2 in front of water on the right side.
c. Place a coefficient of 3 in front of water on the right side.
d. Place a coefficient of 2 in front of methane on the left side.
65.Communicating Results What is the balanced chemical equation for the reaction represented in Figure 7-2?
a. 2CH4 + 2O2CO2 + H2O
b. CH4 + 4O2CO2 + 4H2O
c. CH4 + 2O2CO2 + H2O
d. CH4 + O2CO2 + 2H2O
Figure 7-3
66.Applying Concepts In an exothermic reaction as seen in Figure 7-3, do the reactants or the products contain more chemical energy?
a. reactantsb. products
67.Inferring Cooking an egg white involves an endothermic reaction. Which has more chemical energy in its chemical bonds—an uncooked egg white or a cooked egg white? Use Figure 7-3 to explain your answer.
a. The cooked egg white has more chemical energy in its chemical bonds because energy was absorbed during the reaction.
b. The uncooked egg white has more chemical energy in its chemical bonds because energy was absorbed during the reaction.
c. There is not enough information
68.Problem Solving If the bonds in the reactants of Figure 7-3 contained 432 kJ of chemical energy and the bonds in the products contained 478 kJ of chemical energy, what would be the amount of energy change during the reaction? (hint: Energy is conserved!)
a. 432 kJ b. 478 kJc. 910 kJd. 46 kJ
69.Using Tables and Graphs What do the peaks on the graphs in Figure 7-3 represent?
a. the amount of mass required to break the chemical bonds of the reactants
b. the amount of energy required to from the chemical bonds of the reactants
c. the amount of energy required to break the chemical bonds of the reactants
d. the amount of energy required to break the chemical bonds of the products
70.Interpreting Graphics Although the amount of energy involved is small enough that it is not noticed, iron rusts according to the following word equation:
iron + oxygen rust + energy
Which of the energy diagrams in Figure 7-3 could be applied to the formation of rust?
a. the diagram on the left
b. the diagram on the right
c. neither diagram explains the chemical reaction.
Figure 8-3
71.Interpreting Graphics Detergent has a pH of about 10. Is detergent acidic or basic? Use Figure 8-3 to answer this question.
a. acidicb. basic
72.Drawing Conclusions Oven cleaner has a pH of 14, and household ammonia has a pH of about 11.2. What generalization might you make about whether most cleaners contain acids or bases? Use Figure 8-3 to answer this question.
a. Most cleaners contain acids.
b. Most cleaners contain bases.
c. Most cleaners are neutral.
73.Applying Concepts Unpolluted rain has a pH of about 6. Is this rain acidic, basic, or neutral? Why is the term acid rain used to refer to rain that has been polluted with oxides of nitrogen and sulfur? This rain frequently has a pH between 4 and 5 and has been found to have a pH as low as 1.8. Use Figure 8-3 to answer these questions.
a. very basic b. very acidicc. slightly basicd. slightly acidic
74.Problem Solving Stomach acid has a pH of about 2. What conclusion can you reach about the pH of an antacid solution that is used to neutralize excess stomach acid? Use Figure 8-3 to answer this question.
a. acidicb. basic
75.Inferring Sea water has a pH of about 8, and pure water has a pH of 7. Would sea water change the color of red litmus paper?
a. yesb. no