Q&A Hero

Q: For the following electrolysis reaction:2 AlOF3-2 + C -> 2 Al + CO2 + F-Where would the aluminum form?A) cathodeB) anodeC) in solutionD) Aluminum formation does not happen because electrons do not flow in above reaction.E) none of the above

Q: How is electrolysis different from what is going on chemically inside a battery? A) They are the same process, just reversed. B) Electrolysis does not use electrons. C) Electrolysis only uses electrons from a cathode. D) You cannot make pure compounds with electrolysis. E) You do not produce a chemical change in electrolysis.

Q: Why don't the electrodes of a fuel cell deteriorate the way the electrodes of a battery do? A) As long as fuel is supplied, fuel cells don't run down, but car batteries die when the electron-producing chemicals are consumed. B) Fuel cell electrodes are made of graphite, which does not deteriorate. C) Fuel cell electrodes are self-replenishing thanks to the KOH-containing paste. D) Fuel cell do not use electrodes, so there are none to deteriorate.

Q: What is one of the drawbacks to using fuel cells? A) The fuel of the fuel cells is hard to handle. B) They are less efficient than combustion energy sources or batteries. C) They are very big and bulky, which makes them hard to use in small devices. D) There are no drawbacks. E) only A and B

Q: What is one of the advantages of a fuel cell? A) They can run for a very long time as long as you keep adding fuel. B) They are more efficient than combustion. C) They have lower emission of pollutants than combustion. D) all of the above E) only A and B

Q: In one type of fuel cell, the following oxidation-reduction reactions are taking place:2 H2 + O2 -> 2 H2OWhat is the oxidant?A) H2B) O2C) H2OD) all of the aboveE) none of the above

Q: In one type of fuel cell the following oxidation-reduction reactions are taking place:2 H2 + O2 -> 2 H2OWhat is the fuel?A) H2B) O2C) H2OD) all of the aboveE) none of the above

Q: What is the primary difference between a fuel cell and a battery? A) Fuel cells do not run down because they can be refueled; batteries run down and need to be recharged. B) Batteries can be recharged, fuel cells cannot. C) Batteries supply electricity; fuel cells supply heat. D) Fuel cells oxidize to supply electricity, batteries reduce to supply electricity. E) Fuel cells do not use metals as oxidants and reductants, batteries have a static reservoir of oxidant and reductant.

Q: Why does a battery that has thick zinc walls last longer than one that has thin zinc walls? A) Thick zinc walls prevent the battery from over heating. B) Thicker zinc walls prevent electrons from being lost into the surrounding environment. C) Thicker zinc walls last longer at holding in the battery acid. D) The zinc walls are transformed into zinc ions as the battery provides electricity.

Q: Your car lights were left on while you were shopping, and now your car battery is dead. Has the pH of the battery fluid increased or decreased? A) The pH of the battery fluid has increased. B) The pH of the battery fluid has decreased. C) The pH of the battery fluid does not change. D) Since the lights were left on and the battery is dead, the pH of the battery fluid must be zero.

Q: Why might disposing of a lead-acid battery, nickel-cadmium battery or mercury battery in a landfill be a bad thing? A) Cadmium, mercury, and lead are all toxic metals and could leak out of the landfill. B) Cadmium, mercury, and lead are all very reactive and generate highly unstable compounds. C) Cadmium, mercury, and lead are all radioactive and release radiation. D) all of the above E) none of the above

Q: In a battery, if the following oxidation-reduction reactions takes place normally:Mn2O3 + ZnO -> 2 MnO2 + ZnWhat reaction would be taking place if you were charging the battery?A) 2 MnO2 + Zn -> Mn2O3 + ZnOB) ZnO -> ZnC) Mn2O3 -> MnO2D) all of the aboveE) none of the above

Q: In a battery, the following oxidation-reduction reactions are taking place:Mn2O3 + ZnO -> 2 MnO2 + ZnWhat is being formed at the anode?A) ZnB) ZnOC) MnO2D) Mn2O3E) none of the above

Q: In a battery, the following oxidation-reduction reactions are taking place:Mn2O3 + ZnO -> 2 MnO2 + ZnWhat is being formed at the cathode?A) ZnB) ZnOC) MnO2D) Mn2O3E) none of the above

Q: In a battery, the following oxidation-reduction reactions are taking place:Mn2O3 + ZnO -> 2 MnO2 + ZnWhat is undergoing an oxidation as written?A) ZnB) ZnOC) MnO2D) Mn2O3E) none of the above

Q: In a battery, the following oxidation-reduction reaction is taking place:Mn2O3 + ZnO -> 2 MnO2 + ZnWhat is undergoing reduction as written?A) ZnB) ZnOC) MnO2D) Mn2O3E) none of the above

Q: In a battery, the following two oxidation-reduction reactions are taking place:rxn A: Zn + 2 OH- -> ZnO + H2O + 2e-rxn B: 2 MnO2 + H2O + 2e- -> Mn2O3 + 2 OH-What is undergoing reduction?A) ZnB) ZnOC) MnO2D) H2OE) OH-

Q: In a battery, the following two oxidation-reduction reactions are taking place:rxn A: Zn + 2 OH- -> ZnO + H2O + 2e-rxn B: 2 MnO2 + H2O + 2e- -> Mn2O3 + 2 OH-What is undergoing oxidation?A) ZnB) ZnOC) MnO2D) H2OE) OH-

Q: In a battery, the following two oxidation-reduction reactions are taking place:rxn A: Zn -> Zn+2 + 2e-rxn B: 2 NH4+ + 2e- -> 2 NH3 + H2Which reaction is taking place at the cathode?A) rxn AB) rxn BC) Both reactions are happening at both the anode and cathode.D) Both reactions are happening are happening at the electrode.E) The reaction takes place at the electrode, not the cathode.

Q: In a battery, the following two oxidation-reduction reactions are taking place:rxn A: Zn -> Zn+2 + 2e-rxn B: 2 NH4+ + 2e- -> 2 NH3 + H2Which reaction is taking place at the anode?A) rxn AB) rxn BC) Both reactions are happening at both the anode and cathode.D) Both reactions are happening at the electrode.E) The reaction takes place at the electrode, not the anode.

Q: In the oxidation-reduction reaction Mg(s) + (aq) → 3 (aq) + Cu(s), which atom or ion is reduced? Which atom or ion is oxidized? A) The ion is oxidized as it gains electrons from the copper metal, Cu. The magnesium metal, Mg, is reduced as it loses electrons to form . B) The ion is reduced as it gains electrons from the copper metal, Cu. The is oxidized as it loses electrons to the . C) The ion is reduced as it gains electrons to form copper metal, Cu. The magnesium metal, Mg, is oxidized as it loses electrons to form . D) Since Mg goes from a solid to an aqueous solution and Cu goes from an aqueous solution to a solid, an oxidation-reduction reaction did not occur.

Q: What is the purpose of the salt bridge in a voltaic cell? A) to prevent any further migration of electrons through the wire B) to allow for the build up of positively charged ions in one container and negatively charged ions in the other container C) to allow the and the to flow freely between the two containers D) to allow for a balance of charge between the two chambers

Q: Which of the following statements best describes an anode? A) the negatively charged electrode of a battery or electrochemical apparatus B) the place where oxidation is taking place in a battery or electrochemical apparatus C) the place from which electrons are flowing away from D) all of the above E) none of the above

Q: Which of the following statements best describes a cathode? A) the negatively charged electrode of a battery or electrochemical apparatus B) the place where oxidation is taking place in a battery or electrochemical apparatus C) the place from which electrons are flowing away from D) all of the above E) none of the above

Q: Which of the following describes an electrode? A) Any material that conducts electrons into a media where electrochemical reactions are taking place. B) Any material that conducts electrons out of a media where electrochemical reactions are taking place. C) Any material that conducts electrons. D) Any material that is undergoing an oxidation-reduction reaction in a battery. E) either A or B

Q: The following set of redox reactions takes place as shown.Container A Container BFe -> Fe+2 + 2e- Cu +2 + 2e- -> CuIf you had two containers filled with the ion solution described above with a wire connecting a piece of iron (in container A) and a piece of copper (in container B) and a salt-bridge connecting the two containers, which way do the positive ions in the salt-bridge flow?A) There is no flow of positive ions in the salt-bridge.B) The positive ions flow from container A to container B.C) The positive ions flow from container B to container A.D) The positive ions flow back and forth between the two containers.E) The ions only move in the containers they originate in.

Q: The following set of redox reactions takes place as shown.Container A Container BFe -> Fe+2 + 2e- Cu+2 + 2e- -> CuIf you had two containers filled with the ion solution described above with a wire connecting a piece of iron (in container A) and a piece of copper (in container B) and a salt-bridge connecting the two containers, which way do the electrons flow?A) There is no continuous flow of electrons.B) The electrons flow from container A to container B.C) The electrons flow from container B to container A.D) The electrons flow back and forth between the two containers.E) The electrons only move in the containers they originate in.

Q: The following set of redox reactions takes place as shown.Container A Container BFe -> Fe+2 + 2e- Cu+2 + 2e- -> CuIf you had two containers filled with the ion solution described above with a wire connecting a piece of iron (in container A) and a piece of copper (in container B) and a salt-bridge connecting the two containers, describe what happens.A) A little bit of iron is converted into iron ions and a little bit of copper ion is converted into copper metal.B) All of the iron is transformed into iron ions and all of the copper is transformed into copper ions.C) All of the iron is transformed into iron ions and all of the copper ions are transformed into copper metal.D) All of the iron ions are transformed into iron metal and all of the copper is transformed into copper ions.E) All of the iron ions are transformed into iron metal and all of the copper is transformed into copper metal.

Q: What is the purpose of a salt-bridge? A) to allow ions to migrate between solutions B) to allow people to cross over salt water C) to allow electrons to migrate through solutions D) to allow salt to form in the oxidation-reduction reactions E) none of the above

Q: The following set of redox reactions takes place as shown.Container A Container BFe -> Fe+2 + 2e- Cu+2 + 2e- -> CuIf you had two containers filled with the ion solution described above with only a wire connecting a piece of iron (in container A) and a piece of copper (in container B), which way do the electrons flow?A) There is no continuous flow of electrons.B) The electrons from from container A to container B.C) The electrons flow from container B to container A.D) The electrons flow back and forth between the two containers.E) The electrons only move in the containers they originate in.

Q: The following set of redox reactions takes place as shown.Container A Container BFe -> Fe+2 + 2e- Cu+2 + 2e- -> CuIf you had two containers filled with the ion solution described above with only a wire connecting a piece of iron (in container A) and a piece of copper (in container B), describe what happens.A) A little bit of iron is converted into iron ions and a little bit of copper ion is converted into copper metal.B) All of the iron is transformed into iron ions and all of the copper is transformed into copper ions.C) All of the iron is transformed into iron ions and all of the copper ions are transformed into copper metal.D) All of the iron ions are transformed into iron metal and all of the copper is transformed into copper ions.E) All of the iron ions are transformed into iron metal and all of the copper is transformed into copper metal.

Q: The following set of redox reactions takes place when iron is dipped into a solution of copper ions.Fe -> Fe+2 + 2e-Cu+2 + 2e- -> CuWhich of the following describes what is happening with the electrons in the solution?A) The iron metal is releasing electrons and they are traveling to the copper ions.B) The copper is releasing electrons and they are traveling to the iron ions.C) The iron ions are gaining electrons from the copper metal.D) The copper ions are releasing electrons and they are traveling to the iron metal.E) none of the above

Q: The following set of redox reactions takes place when iron is dipped in a solution of copper ions.Fe -> Fe+2 + 2e-Cu+2 + 2e- -> CuWhich of the following describes what is happening on the surface of the iron?A) The copper starts to plate out on iron.B) The iron rusts in the water.C) The iron starts to plate out on the copper.D) The iron corrodes the copper.E) none of the above

Q: Which of the following statements about electrochemistry is not true? A) It is the study of how electrical energy and chemical reactions are related. B) It involves the use of a set of oxidation-reduction reactions to produce electrical current. C) It involves the use of electrical current to produce an oxidation-reduction reaction. D) It is the study of how electrons are transferred from one chemical compound to another. E) All of the above are true.

Q: Upon ingestion, grain alcohol, O, is metabolized into acetaldehyde, O, which is a toxic substance causing headaches as well as joint pains typical of a "hangover." Is the grain alcohol oxidized or reduced as it transforms into acetaldehyde? A) The grain alcohol is reduced. B) The grain alcohol is oxidized. C) Some of the grain alcohol is oxidized and some is reduced to other products. D) The grain alcohol is neither oxidized nor reduced.

Q: Glucose, , is a simple sugar that the body metabolizes into two molecules of pyruvic acid, . Is the glucose oxidized or reduced as it transforms into pyruvic acid? A) The glucose is oxidized. B) The glucose is reduced. C) Parts of the glucose molecule are oxidized while others are reduced. D) Glucose is neither oxidized or reduced as it transforms into pyruvic acid.

Q: When lightning strikes, nitrogen molecules, , and oxygen molecules, , in the air react to form nitrates, -, which come down in the rain to help fertilize the soil. Is this this an example of oxidation or reduction?A) The formation of nitrates is an example of oxidation.B) The formation of nitrates is an example of reduction.C) Both. The nitrogen is oxidized as it reacts with the oxygen while the oxygen is reduced.D) Neither. Although the bonds of both the and molecules are broken to form the , neither oxidation nor reduction occurs.

Q: Clorox is a laundry bleaching agent used to remove stains from white clothes. Suggest why the name begins with Clor- and ends with -ox. A) Clor~ because it has chlorine, ~ox because it is as strong as an ox. B) The active ingredient contains chlorine atoms, which behave as strong oxidizing agents. C) Chlor~ because it has chlorine ions, ~ox because it is reduced. D) Chlor~ because it has chlorine ions, ~ox because it uses oxygen.

Q: Which element is closer to the upper right corner of the periodic table, the one indicated by the lighter colored atoms or the darker colored atoms? A) the element indicated by the darker color B) the element indicated by the lighter color C) More information is needed in order to determine which element is closer to the upper right of the periodic table. D) Both the lighter and darker colored elements are likely found at the upper right corner of the periodic table.

Q: Chemical equations need to be balanced not only in terms of the number of atoms, but also by the charge. In other words, just as there should be the same number of atoms before and after the arrow of an equation, there should be the same charge. What set of coefficients is necessary to balance the following chemical equation?________ + ________ Cl- -> ________ + ________ A) 1, 2, 1, 1B) 2, 2, 2, 1C) 1, 4, 1, 2D) 3, 4, 3, 2

Q: Chemical equations need to be balanced not only in terms of the number of atoms, but also by the charge. In other words, just as there should be the same number of atoms before and after the arrow of an equation, there should be the same charge. What set of coefficients is necessary to balance the following chemical equation?________ + ________ Ag -> ________ Sn + ________ Ag+A) 1, 2, 1, 2B) 1, 1, 1, 2C) 1, 2, 2, 2D) 1, 1, 2, 1

Q: The general chemical equation for photosynthesis is shown below. Through this reaction are the oxygens of the water molecules, H2O, oxidized or reduced?6 + 6O -> + 6 A) The oxygens of the water molecules are oxidized.B) The oxygens of the water molecules are reduced.C) The oxygens of some of these water molecules are oxidized while others are reduced.D) The oxygens of the water molecules are neither oxidized nor reduced.

Q: The general chemical equation for photosynthesis is shown below. Through this reaction is the carbon oxidized or reduced? How can you tell?6 + 6O -> + 6 A) Oxidized, since carbon is in the +4 oxidation state in but in the +6 oxidation state in the product, , glucose.B) Reduced, since in carbon dioxide there are two oxygen atoms for every one carbon but within the product, , (glucose), there is only one oxygen for every one carbon.C) Neither, since carbon does not change its oxidation state and is neither oxidized nor reduced.D) Both, since the carbon atoms within the glucose molecules display two different charge states.

Q: How does an atom's electronegativity relate to its ability to become oxidized? A) The greater the electronegativity of an atom, the greater its ability to become oxidized. B) The lower the electronegativity of an atom, the lower its ability to become oxidized. C) The greater the electronegativity of an atom, the lower its ability to become oxidized. D) Electronegativity does not effect the atom's ability to become oxidized.

Q: In the above diagram, which atom behaves as the oxidizing agent, the lighter colored atom or the darker colored atom? A) Both atoms behave as the oxidizing agent. B) Neither of the atoms behave as the oxidizing agent. C) The darker colored atom behaves as the oxidizing agent. D) The lighter colored atom behaves as the oxidizing agent.

Q: In the above diagram, which atom is oxidized, the darker colored atom or the lighter colored atom? A) Both of the atoms are oxidized. B) Neither of the atoms is oxidized. C) Only the darker colored atom is oxidized. D) Only the lighter colored atom is oxidized.

Q: For each of the following unbalanced equations, which is depicted: oxidation or reduction?a) Cr -> b)Sn -> A) a) oxidation; b) reductionB) a) reduction; b) oxidationC) a) reduction; b) reductionD) a) oxidation; b) oxidation

Q: Hydrogen sulfide, H2S, burns in the presence of oxygen, , to produce water, O, and sulfur dioxide, SO2. Through this reaction, is sulfur oxidized or reduced?2 S + 3 -> 2 O + 2 A) Sulfur is reduced.B) Sulfur is oxidized.C) Sulfur is both oxidized and reduced.D) Sulfur is neither oxidized nor reduced.

Q: What element is behaves as the oxidizing agent in the following equation and what element behaves as the reducing agent?+ 2 Ag -> Sn + 2 Ag+A) The tin ion, , is the oxidizing agent while silver, Ag, is the reducing agent.B) The tin ion, Sn2+, is the reducing agent while silver, Ag, is the oxidizing agent.C) The tin, Sn, is the reducing agent while silver ion, Ag+, is the oxidizing agent.D) The tin, Sn, is the oxidizing agent while silver ion,Ag+, is the reducing agent.

Q: What element is oxidized in the following equation and what element is reduced?+ 2 Ag -> Sn + 2 Ag⁺A) The tin ion, , is oxidized, while the silver, Ag, is reduced.B) The tin ion, , is reduced, while the silver, Ag, is oxidized.C) Both the tin ion, , and the silver, Ag, are reduced.D) Both the tin ion, , and the silver, Ag, are oxidized.

Q: What might the relationship be between an element's electronegativity and its ability to behave as an oxidizing agent? A) As the electronegativity goes up the ability of an element to act as an oxidant increases. B) As the electronegativity goes up the ability of an element to act as an oxidant decreases. C) As the electronegativity goes up the ability of an element to act as an oxidant stays the same. D) As the electronegativity increases the element has a tendency to undergo oxidation. E) none of the above

Q: Which of the following materials is most likely to act as a reducing agent? A) Na B) Na+ C) Cl2 D) Cl- E) both A and B

Q: Which of the following materials is most likely to undergo reduction? A) Na B) Na+ C) Cl2 D) Cl- E) both A and B

Q: Which of the following materials is most likely to act as an oxidizing agent? A) Na B) Na+ C) Cl2 D) Cl- E) both A and B

Q: Which of the following materials is most likely to undergo oxidation? A) Na B) Na+ C) Cl2 D) Cl- E) both A and B

Q: Which of the following species is the reducing agent?2 CuBr -> 2Cu + Br2A) CuB) CuBrC) Cu+D) Br-E) Br2

Q: Which of the following species is the oxidizing agent?2 CuBr -> 2Cu + Br2A) CuB) CuBrC) Cu+D) Br-E) Br2

Q: Which of the following species is undergoing reduction?2 CuBr -> 2Cu + Br2A) CuB) CuBrC) Cu+D) Br-E) Br2

Q: Which of the following species is undergoing oxidation?2 CuBr -> 2Cu + Br2A) CuB) CuBrC) Cu+D) Br-E) Br2

Q: Which of the half-reactions below would be complementary and balance the following half-reaction?Zn+2 ->ZnA) Cu ->Cu+2B) K+ -> KC) 2 Cu -> 2 Cu+2D) 2 K+ -> 2 KE) Cl2 -> 2 Cl-

Q: Which of the half-reactions below would be complementary, balance the following half-reaction, and be chemically reasonable?Br2 -> 2 Br-A) 2 K -> 2 K+B) K+ -> KC) K -> K+D) 2 K+ -> 2 KE) K -> K+2

Q: How many electrons are gained or lost in the following half-reaction?Zn -> Zn+2A) 2 electrons are lostB) 1/2 electron is gainedC) 1/2 electron is lostD) 2 electrons are gainedE) 4 electrons are gained

Q: How many electrons are gained or lost in the following half-reaction?Cl2 -> 2 Cl-A) 2 electrons are lostB) 1/2 electron is gainedC) 1/2 electron is lostD) 2 electrons are gainedE) 4 electrons are gained

Q: How many electrons are gained or lost in the following half-reaction?2 Na -> 2 Na+A) 2 electrons are lostB) 1/2 electron is gainedC) 1/2 electron is lostD) 2 electrons are gainedE) 4 electrons are gained

Q: How many electrons are gained or lost in the following half-reaction?Na -> Na+A) 1 electron is lostB) 1/2 electron is gainedC) 1/2 electron is lostD) 1 electron is gainedE) 2 electrons are gained

Q: Which of the following statements about oxidation and reduction reactions is true? A) More than one electron can be transferred in an oxidation and reduction reaction. B) In a half-reaction, only half of an electron is transferred. C) Only neutral atoms are formed in oxidation and reduction reactions. D) A half-reaction is only used for reduction reactions. E) None of the above are true.

Q: Which of the following statements is untrue about oxidation and reduction processes? A) An oxidation can happen without a reduction. B) It involves the exchange of electrons. C) Often ions are generated or consumed. D) Electrons are often involved in oxidation and reduction reactions. E) All of the above are true.

Q: What is a reduction? A) the gain of electrons B) the reduction of the number of electrons C) the loss of an electron from the valence shell D) the reaction of oxygen with a reductant E) the formation of red compounds in the presence of an oxidant

Q: What is oxidation? A) the loss of electrons B) the reaction with oxygen C) the reduction of oxygen D) the gaining of electrons E) the addition of an electron to the valence shell

Q: Cutting back on the pollutants that cause acid rain is one solution to the problem of acidified lakes. Suggest another. A) stop using NaCl to salt the roads in the winter B) add a neutralizing substance such as limestone C) add ammonium ions to the lakes D) add chlorine and filter the water to remove any acidity in the lake

Q: Lakes lying in granite basins, such as those in the northeastern U.S., tend to become acidified by acid rain more readily than lakes lying in limestone basins, such as those found in the midwestern U.S. Why is this so? A) The granite contains acidic minerals that dissolve in the rain water and are added to the lakes. B) Since the acidified water cannot percolate through the granite, the acid in the lakes becomes more concentrated. C) The limestone, which is calcium carbonate, serves to neutralize the acid in the rain. D) There is more acid rain in the northeast than in the midwestern regions of the U.S.

Q: How might you tell whether or not your toothpaste contained either calcium carbonate, CaC, or baking soda, NaHC, without looking at the ingredients label? A) if the toothpaste bubbles when heated B) if the toothpaste bubbles when added to ammonia, such as window cleaner C) if the toothpaste produces a salt (NaCl) when added to HCl D) if the toothpaste bubbles when added to vinegar

Q: Why might a small piece of chalk made of calcium carbonate be useful for alleviating acid indigestion? A) Calcium carbonate is a base that reacts to neutralize any excess acids. B) Calcium carbonate is able to absorb excess acid and carry it out of the system. C) Calcium carbonate is able to add an extra lining to the stomach to protect it from the excess acid. D) Calcium carbonate is able to turn the acid into a gas which can relieve the build up of excess acid.

Q: Why is carbon dioxide able to be stored more effectively in ocean water vs. fresh water? A) The pH of the ocean is pretty high and so the carbon dioxide is trapped in a neutralization reaction. B) The oceans are large and so you can dissolve more CO2 in them. C) Gases are more soluble in cold water than warm water and the oceans are colder than fresh water lakes so you can dissolve more CO2 in them. D) The pH of the ocean is very low and so the carbon dioxide is trapped as an acid because like dissolves like. E) none of the above

Q: Why might an area with a large amount of limestone (CaCO3) be less susceptible to acid rain? A) The acid in the rain is neutralized by the natural base in the limestone. B) The rain travels quickly through the porous limestone and therefore the rate of reaction is slower. C) Limestone is degraded by acid rain and therefore acid rain has the same damaging effects. D) Only acid rain made from sulfur compounds reacts with the limestone. E) none of the above

Q: What is the source of acid rain? A) Acid rain is from dissolved carbon dioxide. B) All rain is acid rain because rain has a pH is less than 7. C) Rain is normally basic, but depending on the weather it can get slightly acidic. D) All rain is acid rain because rain has a hydronium ion concentration greater than 10-7 M. E) none of the above

Q: What would be the best explanation for the fact that most natural water has a pH of about 5.6? A) Carbon dioxide reacts with water to form an acid. B) Air contains acid rain particles. C) Minerals that are dissolved in water are often acidic. D) Many salts that dissolve in natural waters make the water basic. E) none of the above

Q: Pour vinegar onto beach sand from the Caribbean and the result is a lot of froth and bubbles. Pour vinegar onto beach sand from California, however, and nothing happens. Why? A) Beaches in tropical climates generally have remnants of volcanic deposit not present in California sand. These deposits contain soil with organic residue. Vinegar's acetic acid reacts with organic matter. B) The pH of the warm sands of tropical waters is well into the basic range, unlike the beach sand in California. Therefore, the acidic vinegar reacts with Caribbean beach sand but not with sand from California. C) Beach sand from the Caribbean and many other tropical climates is made primarily of the calcium carbonate remains of coral and shelled creatures. Vinegar is an acid and the calcium carbonate is a base. D) Caribbean beach sand contains deposits from the mouth of the Mississippi river which carries with it a great deal of contamination from urban waste. These warm water contaminates react with the acid in vinegar.

Q: What happens to the pH of soda water as it loses its carbonation? A) It does not change since the carbonation has nothing to do with pH. B) It decreases as it loses the carbon dioxide molecules which form the carbonic acid in the soda. C) It increases as it loses the carbon dioxide molecules which form the carbonic acid in the soda. D) It decreases as the soda becomes more concentrated through the loss of the carbon dioxide gases.

Q: What is the hydroxide ion concentration in an aqueous solution where the pH = 5?A) The hydronium ion concentration equals 1 .B) The hydronium ion concentration equals 1 .C) The hydronium ion concentration equals 1 .D) The hydronium ion concentration equals 1 .