Q&A Hero

Q: The [ H3O+] of a solution with pH = 5.60 is A) 3 x 10-6 M. B) 2.5 x 10-8 M. C) 2.5 x 10-6 M. D) 4.0 x 10-6 M. E) 4.0 x 10-9 M.

Q: In a sulfuric acid solution, where the [ H3O+] is 0.01 M, what is the pH? A) pH = 12.0 B) pH = 2.0 C) pH = 3.0 D) pH = 11.0 E) pH = 5.0

Q: In which of the following are the pH values arranged from the most acidic to the most basic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 1.1 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

Q: In which of the following are the pH values arranged from the most basic to the most acidic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 11 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

Q: The [ H3O+] of a solution with pH = 2 is A) 10 M. B) -10 M. C) 1 x 102 M. D) 1 x 10-2 M. E) 1 x 10-12 M.

Q: What is the pH of a solution with [OH-] = 2.0 x 10-10 M? A) 9.70 B) -9.70 C) 4.30 D) -4.30 E) 2.0 x 10-10

Q: What is the pH of a solution with [OH-] = 1 x 10-4 M? A) 10.0 B) -10.0 C) 4.0 D) -4.0 E) 1.0 x 10-10

Q: What is the pH of a solution with [ H3O+] = 3.0 x 10-3 M? A) 3.0 x 10-3 B) 2.52 C) 3.0 D) -2.52 E) 9.0

Q: What is the pH of a solution with [ H3O+] = 1 x 10-9 M? A) 1.0 x 10-5 M B) -9.0 C) 5.0 D) -5.0 E) 9.0

Q: A solution with a pH of 4 is A) extremely acidic. B) moderately acidic. C) neutral. D) slightly basic. E) extremely basic.

Q: A solution which has [OH-] = 3.4 x 10-12 M is A) acidic. B) basic. C) neutral..

Q: A solution which has [OH-] = 4.6 x 10-6 M is A) acidic. B) basic. C) neutral.

Q: A solution which has [ H3O+] = 6.7 x 10-8 M is A) acidic. B) basic. C) neutral.

Q: What is the [ H3O+] in a solution that has a [OH-] = 5.0 x 10-2 M? A) 2.0 x 10-12 M B) 2.0 x 10-2 M C) 1.0 x 10-14 M D) 2.0 x 10-4 M E) 5.0 x 10-12 M

Q: What is the [OH-] in a solution that has a [ H3O+] = 2.0 x 10-4 M? A) 2.0 x 10-10 M B) 5.0 x 10-10 M C) 1.0 x 10-10 M D) 2.0 x 10-4 M E) 5.0 x 10-11 M

Q: What is the [OH-] in a solution that has a [ H3O+] = 1 x 10-6 M? A) 1 x 10-2 M B) 1 x 10-6 M C) 1 x 10-8 M D) 1 x 10-10 M E) 1 x 10-12 M

Q: What is the [ H3O+] in a solution with [OH-] = 1 x 10-12 M? A) 1 x 10-12 M B) 1 x 102 M C) 1 x 10-7 M D) 1 x 10-8 M E) 1 x 10-2 M

Q: Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? A) In acids, [OH-] is greater than [ H3O+]. B) In bases, [OH-] = [ H3O+]. C) In neutral solutions, [ H3O+] = [ H2O]. D) In bases, [OH-] is greater than [ H3O+]. E) In bases, [OH-] is less than [ H3O+].

Q: For Kw, the product of [ H3O+] and [OH-] is A) 1.0 x 10-14. B) 1.0 x 10-7. C) 1.0 x 10-1. D) 1.0. E) 1.0 x 1014.

Q: Predict whether the equilibrium of the following reaction favors reactants or products:NH4+ + H2O -> NH3 + H3O+A) Reactants are favored.B) Products are favored.C) Neither side is favored.

Q: The Ka for hydrofluoric acid is 7.2 x 10-4. This means that HF is A) neutral in water solution. B) able to react with HCl. C) a weak acid. D) a strong acid. E) ionic.

Q: Which of the following is the weakest acid? A) HF (Ka for HF is 7.2 x 10-4) B) HCN (Ka for HCN is 4.9 x 10-10) C) HCNO (Ka for HCNO is 2 x 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 x 10-10)

Q: Which of the following is the strongest acid? A) HF (Ka for HF is 7.2 x 10-4) B) HCN (Ka for HCN is 4.9 x 10-10) C) HCNO (Ka for HCNO is 2 x 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 x 10-10)

Q: Ammonium hydroxide is a weak base because A) it is a dilute solution. B) it is only slightly soluble in water. C) it cannot hold on to its hydroxide ions. D) it dissociates only slightly in water. E) it is completely ionized in aqueous solution.

Q: Which of the following is correctly identified? A) NH3, strong acid B) NaOH, strong base C) HCl, weak acid D) H2CO3, strong acid E) Ca(OH)2, weak base

Q: Which of the following is the strongest base? A) H3PO4 B) NH3 C) NaOH D) NaCl E) HCl

Q: The stronger the acid, the ________ the conjugate base. A) stronger B) weaker

Q: Which of the following is the strongest acid? A) H3PO4 B) NH4+ C) NaOH D) H2CO3 E) HCl

Q: The conjugate acid of HSO4- is A) SO42-. B) HSO4. C) H2SO4. D) H2SO4-. E) HSO3-.

Q: The conjugate base of HClO3 is A) HClO2. B) ClO3-. C) Cl(OH)2. D) ClO3. E) HClO.

Q: Identify the Brnsted-Lowry acids in the following reaction.H2O + CO32- ->HCO3- + OH-A) H2O/HCO3-B) CO32-/HCO3-C) OH-/HCO3-D) CO32-/OH-E) H2CO3/H2O

Q: According to the Brnsted-Lowry definition, A) an acid is a proton acceptor. B) a base produces H+ ions in aqueous solutions. C) a base is a proton donor. D) a base is a proton acceptor. E) an acid acts as the solvent.

Q: The name of Al(OH)3 is A) aluminum trihydroxide. B) monoaluminum trihydroxide. C) aluminum hydroxide. D) aluminum(III) hydroxide. E) aluminum oxygen hydride.

Q: The correct formula for sulfuric acid is A) H2SO4. B) H2SO3. C) H2SO4-. D) H2SO3-. E) SO42-.

Q: Which one of the following is characteristic of a base? A) produces H3O+ in water B) has a sour taste C) has a slippery, soapy feel D) turns blue litmus red E) is insoluble in water

Q: The name given to an aqueous solution of HClO3 is A) chlorous acid. B) hypochlorous acid. C) chloric acid. D) hydrochloric acid. E) hypochloric acid.

Q: The name given to an aqueous solution of HNO3 is A) nitric acid. B) nitrous acid. C) hydrogen nitrate. D) hydronitrogen acid. E) hyponitric acid.

Q: The name given to an aqueous solution of HBr is A) hydrogen bromide. B) hydrobromic acid. C) bromic acid. D) bromous acid. E) hypobromous acid.

Q: According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydroxide ions. D) a source of H- ions. E) a proton acceptor.

Q: According to the Arrhenius concept, if NaOH were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydronium ions. D) a source of H- ions. E) a proton donor.

Q: Indicate the effect of each change upon the rate of a reaction. A) decreases B) increases 1> adding a catalyst 2> removing some reactant 3> The temperature is doubled. 4> The concentration of a reactant is decreased. 5> More collisions between molecules occur.

Q: An example of a stress on an equilibrium is the increase of pressure in a closed system when the pressure of a reactant gas is increased from 1.0 atm to 2.0 atm.

Q: The equilibrium constant for a reaction does not change with temperature.

Q: If the equilibrium constant for a reaction is 1 10-5, this means that the equilibrium mixture contains mostly reactants.

Q: An equilibrium constant Kc = 1 10-3 for a reaction indicates that the reaction favors product formation.

Q: An equilibrium constant greater than 1 for a reaction indicates that the reaction favors formation of the products.

Q: An equilibrium constant Kc = 1 107 for a reaction indicates that the reaction favors product formation.

Q: The equilibrium constant for the reaction of H2 and F2 to form HF, the concentration of HF is raised to the second power.

Q: The equilibrium constant is the ratio of the concentrations of the reactants over the concentrations of the products.

Q: At equilibrium, the concentrations of the reactants and products are always equal.

Q: One of the substances acted upon by a catalytic converter in an automobile is carbon dioxide.

Q: A catalyst for a chemical reaction affects the magnitude of the equilibrium constant.

Q: The rate of a chemical reaction is not affected by the concentration of reactants.

Q: The rate of a chemical reaction depends on temperature.

Q: Activation energy is always a large amount of energy.

Q: A catalyst lowers the activation energy of a chemical reaction.

Q: The rule or principle that describes the effect of changing reaction conditions on an equilibrium is known as ________ principle.

Q: An equilibrium constant with a value greater than 1 means the reaction favors the ________.

Q: A mixture at equilibrium that contains less product than reactant has a Kc that is ________ than 1.

Q: The equilibrium between hemoglobin and oxyhemoglobin in the blood can be represented by the following reaction. Write the form of the equilibrium constant expression.Hb + O2 -> HbO2

Q: Write the equilibrium constant expression for the reaction of nitrogen and hydrogen to give ammonia, NH3.

Q: 2SO2(g) + O2(g) -> 2SO3(g)For the reaction at equilibrium, if O2 is removed, the amount of SO2 present willA) decreaseB) increaseC) stay the same

Q: For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. Write the equilibrium constant expression of the equilibrium constant, Kc.2NOBr(g) -> 2NO(g) + Br2(g)A) B) C) D) E)

Q: What is the correct form of the equilibrium constant for this reaction?2H2O2 (g) -> 2H2O (g) + O2 (g)A) B) C) D)

Q: 3H2(g) + N2(g) -> 2NH3(g) + heatFor the reaction at equilibrium, if the temperature is raised, the amount of N2 willA) decrease.B) increase.C) stay the same.

Q: For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. Bromine can be liquefied easily and removed from the reaction vessel as it is formed. If this is done, how will it affect the equilibrium reaction?2NOBr(g) -> 2NO(g) + Br2(g)A) More products will be made as Br2 is removed.B) There will be a larger proportion NOBr in the vessel when equilibrium is reached.C) Less NO will be made.D) The pressure in the vessel will increase.E) The equilibrium constant will change.

Q: For the following reaction, the equilibrium constant Kc is 2.0 at a certain temperature. The reaction is endothermic. What do you expect to happen to the concentration of NO if the temperature is doubled?2NOBr(g) -> 2NO(g) + Br2(g)A) The concentration of NO will increase.B) The concentration of NO will decrease.C) There will be no change in [NO].D) A catalyst will be needed to make a change in concentration.E) The change in concentration of [NO] will depend on the size of the vessel.

Q: In an exothermic reaction, heat can be considered a A) reactant. B) product. C) rate. D) catalyst. E) determinant.

Q: In the reaction of carbon dioxide with water to give carbonic acid, the only gaseous component is the carbon dioxide. What will happen to the equilibrium concentration of carbonic acid if the pressure of carbon dioxide is increased in the container? A) The concentration of carbonic acid will increase. B) The carbonic acid concentration will decrease. C) The carbonic acid concentration will stay the same. D) There will be twice as much carbonic acid as carbon dioxide. E) There will be more water available for the reaction.

Q: Treatment of carbon monoxide poisoning can be accomplished by the use of pure oxygen for breathing. This is an example of the use of ________ in a clinical setting. A) the ideal gas law B) Le Chtelier's principle C) Henry's law D) conservation of mass E) a precipitation reaction

Q: PCl5 (g) -> PCl3 (g)+ Cl2 (g)For the reaction at equilibrium, if the volume of the container is increased, the amount of PCl5 present willA) decrease.B) increase.C) double.D) stay the same.E) triple.

Q: 2SO2(g) + O2(g) -> 2SO3(g)For the reaction at equilibrium, if O2 is added, the amount of SO2 present willA) decrease.B) increase.C) stay the same.

Q: N2(g) + O2(g) -> 2NO(g)For the reaction at equilibrium, if the volume of the container is decreased, the amount of NO present willA) decrease.B) increase.C) double.D) stay the same.E) triple.

Q: The reaction of hemoglobin with oxygen can be written as follows.Hb + O2-> HbO2If the amount of oxygen available to the blood decreases significantly, what happens to the individual involved?A) Hypoxia results.B) Anemia results.C) Nitrogen narcosis results.D) Oxygen poisoning results.E) Acclimatization results.

Q: In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide, what is the effect of adding more oxygen gas to the initial reaction mixture? The reaction is shown below.N2(g) + O2(g) -> 2NO(g)A) The equilibrium shifts to produce more N2.B) The equilibrium shifts to produce more NO.C) The equilibrium is not affected.D) Extra catalyst is required to reach equilibrium.E) The temperature of the reaction mixture is raised.

Q: In the following gas phase reaction, what is the effect on the direction of the reaction if more SO3 is added to the reaction mixture?2SO2(g) + O2(g) -> 2SO3(g)A) The equilibrium shifts to produce more products.B) The position of the equilibrium remains unchanged.C) The rate of formation of products is increased.D) The equilibrium shifts to produce more reactants.E) The catalyst for the reaction is used up.

Q: Iron metal reacts with oxygen gas to produce iron(III) oxide. What will be the effect of increasing the pressure of oxygen gas in a closed reaction vessel? A) Less reaction will take place. B) More iron oxide will be produced. C) The reaction mixture will catch fire. D) There is no effect; a catalyst is needed. E) The rate of production of iron oxide will slow down.

Q: When you open a bottle of a soft drink and leave it open, the drink eventually goes flat. This happens because the equilibrium between carbonic acid and carbon dioxide shifts to produce A) more carbonic acid. B) more water. C) more oxygen. D) more carbon dioxide. E) more hydrogen ions.

Q: The physiological equilibrium system that keeps the temperature of the body constant is called A) stimulation. B) regulation. C) metabolism. D) homeostasis. E) catalysis.

Q: In the following gas phase reaction, what is the effect of adding more NO2 to the starting reaction mixture?2NO2(g) -> N2O4(g)A) It would make the reaction more endothermic.B) It would make the reaction more exothermic.C) It would slow the reaction down.D) It would decrease the final quantity of products.E) It would increase the final quantity of products.