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Questions and Answers of Chemistry Principles And Practice

Complete and balance each half-reaction in acid solution,and identify it as an oxidation or a reduction.
Complete and balance each half-reaction in acid solution,and identify it as an oxidation or a reduction.
Balance each of the following redox reactions in acid solution.
Balance each of the following redox reactions in acid solution.
Balance each of the following redox reactions in acid solution.
Balance each of the following redox reactions in acid solution.
Balance each of the following redox reactions in basic solution.
Balance each of the following redox reactions in basic solution.
Balance each of the following redox reactions in basic solution.
Balance each of the following redox reactions in basic solution.
Why is the following balanced reaction not a proper redox reaction?
Why is the following balanced reaction not a proper redox reaction?
A voltaic cell is based on the reactionVoltage measurements show that the Ag electrode is positive.Sketch the cell, and label the anode and cathode, the positive and negative electrodes, the
A voltaic cell is based on the reactionVoltage measurements show that the Ni electrode is positive.Sketch the cell, and label the anode and cathode, the positive and negative electrodes, the
A platinum wire is in contact with a mixture of mercury and solid mercury(I) chloride (Hg2Cl2) in a beaker containing 1 M KCl solution. A salt bridge connects this half cell to a beaker that contains
Two electrodes are immersed in a 1 M HBr solution. One of the electrodes is a silver wire coated with a deposit of AgBr(s). Th e second electrode is a platinum wire in electrical contact with a
For each of the reactions, calculate E° from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard
For each of the reactions, calculate E° from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the
The standard potential for the cell reactionis E° = +0.460 V. Use the tabulated standard potential of the lead half-reaction to find the standard reduction potential of the uranium half-reaction.
The standard potential of the cell reactionis E° = +1.23 V. Use the tabulated standard potential of the silver half-reaction to fi nd the standard reduction potential for the europium half-reaction.
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. Th e
A half-cell that consists of a silver wire in a 1.00 M AgNO3 solution is connected by a salt bridge to a 1.00 M thallium(I) acetate solution that contains a metallic Tl electrode. The voltage of the
Use the data in Appendix H and assume standard conditions when answering the following questions.
Use the data in Appendix H and assume standard conditions when answering the following questions.
Use the standard reduction potentials in Table 18.1 To find(a) A metal ion that reduces Ni2+.(b) A metal ion that can oxidize Cu.(c) A metal ion that is reduced by Cr2+ but not H2.Table 18.1
Use the standard reduction potentials in Table 18.1 to find(a) A reducing agent that will reduce Cu2+ but not Pb2+.(b) An oxidizing agent that will react with Cu but not Fe2+.(c) A metal ion that can
Write an expression and determine a value for Keq for each voltaic cell in Exercise 18.43 .Exercise 18.43Use the standard reduction potentials in Table18.1 to find(a) A metal ion that reduces
Write an expression and determine a value for Keq for each voltaic cell in Exercise 18.44 .Exercise 18.44Use the standard reduction potentials in Table18.1 to find(a) A reducing agent that will
What is ΔG° for the oxidation of metallic iron by dichromate(Cr2O2-7) in acidic solution assuming that the iron is oxidized to Fe2+? Use the data in Appendix H.
What is ΔG° for the oxidation of metallic copper by permanganate(MnO-4) in acidic solution assuming that the copper is oxidized to Cu2+? Use the data in Appendix H.
The standard potential of the half-reactionIn a mixture of hydrogen and deuterium, which isotope more favors its elemental form under standard conditions?
Disproportionation is a type of redox reaction in which the same species is simultaneously oxidized and reduced. One species that undergoes disproportionation is Cu+(aq).
Calculate the potential for each of the voltaic cells in Exercise 18.43 when the concentrations of the soluble species and gas pressures are as follows:Exercise 18.43Use the standard reduction
Calculate the potential for each of the voltaic cells in Exercise 18.44 when the concentrations of the soluble species and gas pressures are as follows:Exercise 18.44For each of the reactions,
A voltaic cell consists of a lead electrode and a reference electrode with a constant potential. This cell has a voltage of 53 mV when the lead electrode is placed in a 0.100 M Pb(NO3)2 solution (the
Consider the voltaic cell
The voltaic cell in Exercise 18.63 produced a voltage of 0.010 V in an unknown test solution. What is the concentration of lead ions in the unknown solution?Exercise 18.63A voltaic cell consists of
Using the voltaic cell in Exercise 18.64 , a voltage of 0.425 V was measured when the cell was placed in a solution of unknown ion concentrations. What is the ratio [Cd2+]/[Ag+]2 in this
Calculate the value of the solubility product constant for Cd(OH)2 from the half-cell potentials.
Calculate the value of the solubility product constant for PbSO4 from the half-cell potentials.
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M ? What is the spontaneous reaction?
What is the voltage of a concentration cell of Cl- ions where the concentrations are 1.045 and 0.085 M ? What is the spontaneous reaction?
(a) Use standard reduction potentials to calculate the potential of a silver-zinc cell that uses a basic electrolyte.The silver oxide is reduced from Ag2O to Ag, and zinc metal is oxidized to
(a) Use standard reduction potentials to calculate the potential of a nickel-cadmium cell that uses a basic electrolyte. The nickel in NiO(OH)(s) is reduced to Ni(OH)2(s), and cadmium metal is
A possible reaction for a fuel cell is(a) Write the oxidation and reduction half-reactions that occur, assuming a basic electrolyte.(b) Use standard free energies of formation to calculate ΔG° for
A possible reaction for a fuel cell is(a) Write the oxidation and reduction half-reactions that occur, assuming a basic electrolyte.(b) Use standard free energies of formation from Appendix G to
Write the half-reactions and the balanced chemical equations for the reactions that occur in the electrolysis of(a) A zinc chloride aqueous solution, using zinc electrodes.(b) A calcium bromide
Write the half-reaction and the chemical equations for the reactions that occur in the electrolysis of(a) Molten CaCl2, using inert electrodes.(b) A saturated solution of magnesium sulfate, using
A solution contains the ions H+, Ag+, Pb2+, and Ba2+,each at a concentration of 1.0 M.(a) Which of these ions would be reduced first at the cathode during an electrolysis?(b) After the first ion has
A solution contains the ions H+, Cu2+, Ca2+, and Ni2+,each at a concentration of 1.0 M.(a) Which of these ions would be reduced first at the cathode during an electrolysis?(b) After the first ion has
The commercial production of fluorine uses a mixture of molten potassium fluoride and anhydrous hydrogen fluoride as the electrolyte. The products of the electrolysis are hydrogen and fluorine.(a)
The commercial production of magnesium is accomplished by electrolysis of molten MgCl2.(a) Why is electrolysis of an aqueous solution of MgCl2not used in this process?(b) Write the anode and cathode
How many coulombs of charge are needed to accomplish each of the following conversions by electrolysis?(a) Produce 0.50 mol Al by electrolysis of Al2O3.(b) Reduce all of the Cu2+ in 100 mL of 0.20 M
How many coulombs of charge are needed to accomplish each of the following conversions by electrolysis?(a) Form 0.50 mol Ca from CaCl2.(b) Produce 3.0 g Al by electrolysis of Al2O3.(c) Form 0.52 g O2
Find the mass of hydrogen produced by electrolysis of hydrochloric acid for 59.0 minutes, using a current of 0.500 A.
What mass of cadmium is deposited from a CdCl2 solution by passing a current of 1.50 A for 38.0 minutes?
How many minutes are needed to deposit 15.0 g copper from a Cu2+ solution, using a current of 3.00 A?
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
Like zinc, sodium is a rather active metal. Would it be possible to use metallic sodium for cathodic protection of the iron hull of an ocean vessel? Explain.
The electrochemical processes that occur in the corrosion of iron are represented by the half-reactions(a) Write the overall reaction.(b) What is the standard potential for the overall chemical
An aluminum bulkhead in a swimming pool collapsed.Stainless steel (mostly iron) braces were bolted to the aluminum to strengthen the bulkhead. Within a few months,the bulkhead collapsed again and
Magnesium is used in the cathodic protection of metal coffins that are guaranteed to last a century without corroding.If the average current produced by the electrochemical cell is 2.0 mA, how much
Assign the oxidation states of all elements in each of the following:(a) CaC2O4 (b) Ba(ClO4)2 (c) Tl3+
Sphalerite is the naturally occurring mineral zinc sulfide,from which zinc metal is extracted. The ore is heated in oxygen to form zinc oxide and sulfur dioxide, followed by the reaction of metal
What is the reduction potential of the hydrogen electrode at 298 K if the pressure of gaseous hydrogen is 2.5 atm in a solution of pH 6.00?
Use the standard reduction potentials in Appendix H to answer the following questions.(a) What products, if any, are formed when KClO3 and KCl are mixed in an acid solution?(b) Which is a stronger
Write the chemical equation and calculate the standard potentials for each of the following, using the data in Appendix H.(a) Fe3+ is added to H2SO3(aq).(b) Iron(II) is titrated with K2Cr2O7.(c)
The standard free energy change at 25 °C, ΔG°, is equal to -34.3 kJ forCalculate the standard potential for this reaction.
The equilibrium constant at 25 °C is 1.58 × 102 forCalculate ΔG° and E° for this reaction.
Calculate the potential of the half-reactionwhen the concentrations in solution are [Fe3+] = 0.033 M and [Fe2+] = 0.0025 M, and the temperature is 298 K.
Another type of battery is the alkaline zinc-mercury cell,in which the cell reaction is(a) What is the standard free energy change for this reaction?(b) The standard free energy change in a voltaic
In the analytical technique called electrogravimetry, electrolysis is used to separate the analyte from a solution by depositing it on an inert electrode. The electrode is weighed before and after
At 298 K, the solubility product constant for PbC2O4is 8.5 × 10-10, and the standard reduction potential of the Pb2+(aq) to Pb(s) is -0.126 V.(a) Find the standard potential of the half-reactionThe
At 298 K, the solubility product constant for Pb(IO3)2is 2.6 × 10-13, and the standard reduction potential of the Pb2+ (aq) to Pb(s) is -0.126 V.(a) Find the standard potential of the
The acid-base titration curves discussed in Chapter 16 can be determined using a pH meter, which measures the potential of a cell made up of a reference electrode and an indicating electrode that
Calculate the rate of oxygen gas production at standard temperature and pressure, in units of milliliters per minute (mL/min), by the electrolysis of water at a 0.250-A current.
An electrolytic cell produces aluminum from Al2O3 at the rate of 10 kg/day. Assuming a yield of 100%,(a) how many moles of electrons must pass through the cell in one day?(b) how many coulombs are
Cardiac pacemakers use a lithium-iodine battery that is based on the reaction(a) What are the E°, ΔG°, and Keq for this reaction?(b) Given the phases of the reactants and products, what do you
An object with a surface area of 100 cm2 is gold plated. The source of the gold is a solution of Au(CN)-4.How many minutes does it take to cover the object with gold to a thickness of 0.0020 mm,
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 × 10-9. Use the standard reduction potential of Ba2+(aq) to fi nd the standard potential for the half-reactionFind ΔG° for both
Another type of fuel cell uses CH4 as the fuel and O2 as the oxidizer. Without having the half-reactions for the fuel cell reaction, use other data available to predict what the E° for this fuel
Identify the conjugate acid-base pairs in
Calculate the hydrogen ion concentration in a solution whose hydroxide ion concentration is 2.0 × 10-5 M.
The hydrogen ion concentration of orange juice is 3.6 × 10-4 M. Calculate the pH.
Calculate the hydrogen ion concentration in a solution that has a pH of 4.76.
Calculate the pH of a solution made by dissolving 1.00 g HI in enough water to make 250 mL of solution.
Calculate the pH when 0.010 g calcium hydroxide is dissolved in enough water to make 100.0 mL of solution.
Calculate Ka for hydrazoic acid, HN3, if a 0.050 M solution is 1.93% ionized.
The pH of a 0.100 M acetic acid solution is 2.88. Calculate Ka.
Calculate the percentage ionized in solutions that are 0.0100 and 0.0010 M naphthol.
Calculate the pH of 0.20 M pyridine. Use Table 15.8 to find Kb.Table 15.8
Calculate Ka for the ammonium ion at 25 °C.
Rank the following bases in order of strength, from weakest to strongest: nitrite ion, fluoride ion, and benzoate ion.
Calculate the pH of a 0.010 M sodium nitrite solution.
Calculate the pH of 0.020 M pyridinium chloride.
How do you calculate the pH of a solution that is 0.050 M HCl and 0.15 M HCOOH?
Explain how to calculate the pH of the following solutions:(a) A solution that is 0.25 M KOH and 1.00 M ammonia(b) A solution that is 0.40 M HCl, 0.20 M HBr, 0.10 M HCOOH, and 0.20 M HF(c) A solution
Set up the equations needed to calculate the pH of a solution that is 0.050 M ammonium ion.StrategyThe strategy is detailed in the steps listed in the margin.

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