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introductory chemistry concepts
Introductory Chemistry Concepts And Critical Thinking 7th Edition Charles Corwin - Solutions
A redox reaction occurs when the tin(II) ion reacts with the iodate ion as follows: Indicate each of the following for the preceding redox reaction:(a) Substance oxidized(b) Substance reduced(c) Oxidizing agent(d) Reducing agent. 6 H+ (aq) + 3 Sn²+ (aq) 3 Sn²+ (aq) + IO3(aq) 3 Sn¹+ (aq) +
What is the coefficient of H2O after balancing the following redox reaction in acidic solution using the half-reaction method? Cu(s) + NO3–(aq) → Cu2+(aq) + NO(aq)(a) 1(b) 2(c) 3(d) 4(e) None of the above.
State the oxidation number for each of the following monoatomic ions.(a) Au3+(b) Mn2+(c) P3–(d) O2–.
Balance the following redox reaction using the oxidation number method: M2O3(s) + X2(g) → MX3(aq) + O2(g)
Balance the following redox reaction in an acidic solution using the oxidation number method: MnO4 (aq) + SO3² (aq) Mn²+ (aq) + SO² (aq)
An industrial blast furnace reduces iron ore, Fe2O3, to molten iron. Balance the following redox equation using the oxidation number method: Fe2O3(l) + CO(g) → Fe(l) + CO2(g)
Which substance listed is the strongest oxidizing agent, given the following spontaneous redox reaction? Mg(s) + Pb2+(aq) → Mg2+(aq) + Pb(s)(a) Mg(b) Pb2+(c) Mg2+(d) Pb(e) None of the above.
Calculate the oxidation number for nitrogen in the following compounds.(a) NH3(b) N2O4(c) Li3N(d) KNO3.
Balance the following redox equation by the oxidation number method: Cl2O5(g) + CO(g) → Cl2(g) + CO2(g)
Aqueous sodium iodide reacts with a potassium dichromate solution. Write a balanced equation for the following redox reaction: H+(aq) + I–(aq) + Cr2O7 2–(aq) → I2(s) + Cr3+(aq) + H2O(l)
Which of the statements listed is true regarding the following redox reaction occurring in a spontaneous electrochemical cell? Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq)(a) Mg is oxidized at the anode.(b) Cu2+ is reduced at the cathode.(c) Electrons flow from the Mg electrode to the Cu
Write a balanced equation for the following redox reaction: H+ (aq) + MnO4 (aq) + NO₂ (aq) Mn²+ (aq) + NO3(aq) + H₂O(1)
Calculate the oxidation number for silicon in the following compounds.(a) Si2H6(b) SiO2(c) Si3N4(d) CaSiO3.
Balance the following redox reaction in a basic solution using the half-reaction method. MnO4 (aq) + SO3² (aq) - MnO₂ (s) + SO4 (aq)
Write a balanced ionic equation for the reaction of iron(II) sulfate and potassium permanganate in acidic solution. The ionic equation is MnO4–(aq) + Fe2+(aq) → Fe3+(aq) + Mn2+(aq)
Which of the statements listed is true regarding the following redox reaction occurring in a nonspontaneous electrochemical cell?(a) Oxidation half-reaction: C + 2 O2– → CO2 + 4e– (b) Reduction half-reaction: Co3+ + 3e– → Co(c) CO2 gas is produced at the anode.(d) Co metal is
Write a balanced ionic equation for the reaction of sodium nitrite and potassium permanganate in acidic solution. The ionic equation is MnO4 (aq) + NO₂ (aq) → Mn²+ (aq) + NO3(aq)
Refer to Figure 17.4 and predict which of the following metals reacts spontaneously in an aqueous FeSO4 solution.(a) Ag(b) Al(c) Cr(d) Ni.Figure 17.4 STRONGEST Oxidizing Agent F₂(g) Cl₂(g) Br₂(1) Ag+ (aq) Fe³+ (aq) 1₂(s) Cu²+ (aq) 2 H+ (aq) Pb²+ (aq) Sn²+ (aq) Ni²+ (aq) Fe²+
Predict whether the following reaction is spontaneous or nonspontaneous. Ni2+(aq) + Sn(s) → Ni(s) + Sn2+(aq)
Refer to the redox reaction and identify the following items: H2O2(aq) + NO2–(aq) → H2O(l) + NO3–(aq)(a) Oxidation half-reaction(b) Reduction half-reaction(c) Substance oxidized(d) Substance reduced(e) Oxidizing agent(f) Reducing agent.
Calculate the oxidation number for carbon in the following polyatomic ions.(a) CO32–(b) HCO3–(c) CN–(d) CNO–.
Predict whether the following reaction is spontaneous or nonspontaneous. Ni2+(aq) + Al(s) → Ni(s) + Al3+(aq)
Draw and illustrate the voltaic cell described in the practice exercise. Refer to Figure 17.4 and label the anode and cathode; show the direction of electron and anion flow.Figure 17.4 STRONGEST Oxidizing Agent F₂(g) Cl₂(g) Br₂(1) Ag+ (aq) Fe³+ (aq) 1₂(s) Cu²+ (aq) 2 H+ (aq) Pb²+
Nickel can react with aqueous silver nitrate solution according to the following ionic equation: Ni(s) + 2 Ag+(aq) → 2 Ag(s) + Ni2+(aq) Assume the half-reactions are separated into two compartments. A Ni electrode is placed in a compartment with 1.00 M Ni(NO3)2, and a Ag electrode is placed in
Magnesium metal is produced by passing an electric current through molten MgCl2 obtained from evaporated seawater. Carbon and platinum rods serve as electrodes, and we can write the redox equation as follows:Indicate each of the following for this nonspontaneous process:(a) Oxidation half-cell
Refer to the voltaic cell illustration and identify the following items:(a) Oxidation half-cell reaction(b) Reduction half-cell reaction(c) Anode and cathode(d) Direction of electron flow(e) Direction of SO42– ion flow.
Draw and illustrate the electrolytic cell described in the practice exercise. Refer to Figure 17.6 and label the anode and cathode; show the direction of electron flow.Figure 17.6 Zn anode Zn²+ Zn is oxidized to Zn²+ at anode. Zn(s) SO Zn²+ So ² Zn²+(aq) + 2 e So, 2- Cu²+ Cu²+ (aq) + 2
Aluminum metal is produced by passing an electric current through bauxite, which contains Al2O3 dissolved in the molten mineral cryolite. Graphite rods serve as electrodes, and we can write the redox equation as follows:Indicate each of the following for this nonspontaneous process:(a) Oxidation
Nickel-cadmium batteries are used in rechargeable electronic calculators. Given the reaction for a discharging NiCad battery, what substance is being oxidized? Cd(s) + NiO₂(s) + 2 H₂O(1) Cd(OH)2(s) + Ni(OH)2(s)
Nickel-cadmium batteries are used in rechargeable electronic calculators. Given the reaction for a recharging NiCad battery, what substance is being oxidized? Cd(OH)2(s) + Ni(OH)2(s) Cd(s) + NiO₂(s) + 2 H₂O(l)
Supply the term that corresponds to each of the following.(a) A redox process characterized by electron loss(b) A substance undergoing oxidation in a redox reaction.
State the substances undergoing oxidation and reduction in the following redox reactions:(a) Co(s) + S(s) → CoS(s)(b) Cd(s) + Cl2(g) → CdCl2(s).
State the substances undergoing oxidation and reduction in the following redox reactions.(a) Mg(s) + S(s) → MgS(s)(b) Mn(s) + Br2(l) → MnBr2(s).
Calculate the pH of the following solutions given the molar hydrogen ion concentration:(a) Vinegar, [H+] = 0.001 M(b) Antacid, [H+] = 0.000 000 001 M.
Calculate the pH for apple juice if the molar hydrogen ion concentration is 0.0001 M.
Classify milk of magnesia as weakly acidic, neutral, or weakly basic given a pH of 10.
Determine the acid and base that were neutralized to produce each of the following salts.(a) Sodium fluoride, NaF(aq)(b) Magnesium iodide, MgI2(aq)(c) Calcium nitrate, Ca(NO3)2( aq)(d) Lithium carbonate, Li2CO3( aq).
Nitric acid is a strong acid, sodium hydroxide is a strong base, and sodium nitrate is a soluble salt. Which of the following is the net ionic equation for the reaction? HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)(a) H+(aq) + OH–(aq) → H2O(l)(b) NO3–(aq) + Na+(aq) → NaNO3(s)(c) H+(aq)
Calculate the molar hydrogen ion concentration given the pH of the following solutions:(a) Lemon juice, pH 2(b) Tomato juice, pH 5.
Calculate the hydrogen ion concentration for milk of magnesia if the pH is 10.
Classify grape juice as weakly acidic, neutral, or weakly basic given a pH of 4.05.
Determine the acid and base that were neutralized to produce each of the following salts.(a) Potassium bromide, KBr(aq)(b) Barium chloride, BaCl2(aq)(c) Cobalt(II) sulfate, CoSO4(aq)(d) Sodium phosphate, Na3PO4(aq).
What must be done first before applying unit analysis to solve an acid–base titration problem?
Calculate the pH of the following solutions given the molar hydrogen ion concentration:(a) Stomach acid, [H+] = 0.020 M(b) Blood, [H+] = 0.000 000 048 M.
Calculate the pH of grape juice if the hydrogen ion concentration is 0.000 089 M.
Classify wine as weakly acidic, neutral, or weakly basic given a pH of 3.25.
Complete and balance the following neutralization reactions.(a) HNO3(aq) + Ca(OH)2(aq) →(b) H2CO3(aq) + Ba(OH)2(aq) →
Beakers X and Y contain either sulfuric acid or sulfurous acid. Based on the conductivity test shown, which beaker contains H2SO4? Which contains H2SO3?
Calculate the molar hydrogen ion concentration given the pH of the following solutions:(a) Acid rain, pH 3.68(b) Seawater, pH 7.85.
Calculate the hydrogen ion concentration in wine if the pH is 3.25.
As the temperature of water increases above 25 °C, the kinetic energy increases and more water molecules ionize. Does the value of Kw increase or decrease above 25 °C? Is the pH of distilled water at 50 °C greater or less than 7.0?
Complete and balance the following neutralization reactions.(a) HC2H3O2(aq) + Sr(OH)2(aq) →(b) H2SO4(aq) + NH4OH(aq) →
The smell of fish is due to a basic organic compound related to ammonia. What common kitchen chemical can be used to neutralize an unpleasant fish odor?
Indicate the change in hydroxide ion concentration for the following changes in hydrogen ion concentration.(a) What happens to the [OH–], if the [H+] increases?(b) What happens to the [OH–], if the [H+] decreases?
Indicate the change in pH for the following changes in molar hydrogen ion concentration.(a) What happens to the pH, if the [H+] increases?(b) What happens to the pH, if the [H+] decreases?
When the weak acid HF(aq) neutralizes the weak base NH4OH(aq), will a conductivity apparatus glow brightly or dimly?
Identify the Brønsted–Lowry acid and base in each of the following neutralization reactions.(a) HC2H3O2(aq) + LiOH(aq) → LiC2H3O2(aq) + H2O(l)(b) NH3(aq) + HCl(aq) → NH4Cl(aq).
What color is the solution in a test tube that contains 10 mL of acid, 1 drop of phenolphthalein, and 1 drop of bromthymol blue indicator?
Write the ionized or nonionized formula for each of the following aqueous solutions given the electrolyte strength:(a) HNO3(aq), strong(b) NH4OH(aq), weak(c) K2CO3(aq), strong.
Write the ionized or nonionized formula for each of the following aqueous solutions given the electrolyte strength:(a) HF(aq), weak(b) Ba(OH)2(aq), strong(c) CaCO3(s), weak.
When the strong acid HNO3(aq) neutralizes the strong base Ba(OH)2(aq), will a conductivity apparatus glow brightly or dimly?
Identify the Brønsted–Lowry acid and base in each of the following neutralization reactions.(a) HNO3(aq) + NaHCO3(aq) → NaNO3(aq) + H2O(l) + CO2(g) (b) NaCN(aq) + HBr(aq) → NaBr(aq) + HCN(aq).
Write a net ionic equation for the reaction between nitric acid and aqueous potassium hydrogen carbonate. HNO3(aq) + KHCO3(aq) → KNO3(aq) + H2O(l) + CO2(g)
Write a net ionic equation for the reaction between aqueous solutions of nitric acid and barium hydroxide. 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)
When the two strong electrolytes, AgNO3(aq) and AlCl3(aq), react to give insoluble AgCl(s), will a conductivity apparatus glow brightly or dimly?
Identify the Brønsted–Lowry acid and base in each of the following neutralization reactions.(a) HI(aq) + H2O(l) → H3O+(aq) + I–(aq)(b) HC2H3O2(aq) + HS–(aq) → H2S(aq) + C2H3O2–(aq).
Write a net ionic equation for the reaction between aqueous solutions of silver nitrate and aluminum chloride. AgNO3(aq) + AlCl3(aq) → AgCl(s) + Al(NO3)3(aq)
Write a net ionic equation for the reaction between aqueous solutions of lithium sulfate and magnesium nitrate. Li2SO4(aq) + Mg(NO3)2(aq) → MgSO4(aq) + 2 LiNO3(aq)
Complete and balance the following Brønsted–Lowry neutralization reactions.(a) HF(aq) + NaHS(aq) →(b) HNO2(aq) + NaC2H3O2(aq) →.
Complete and balance the following Brønsted–Lowry neutralization reactions.(a) H3O+(aq) + SO4 2–(aq) →(b) H2PO4–(aq) + NH3(aq) →
Given the following pH values for solutions containing a drop of phenolphthalein indicator, state the color of each solution.(a) pH 6(b) pH 12.
What is the color of phenolphthalein indicator in deionized water?
Given the following pH values for solutions containing a drop of methyl red indicator, state the color of each solution.(a) pH 3(b) pH 7.
What is the color of methyl red indicator in a solution of pH 5?
Given the following pH values for solutions containing a drop of bromthymol blue indicator, state the color of each solution.(a) pH 5(b) pH 9.
What is the color of bromthymol blue indicator in a solution of pH 7?
If 21.50 mL of 0.115 M barium hydroxide is required to neutralize 25.0 mL of nitric acid, what is the molarity of the acid? 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)
If 27.55 mL of 0.101 M barium hydroxide is required to neutralize 25.0 mL of nitrous acid, what is the molarity of the acid? 2 HNO2(aq) + Ba(OH)2(aq) → Ba(NO2)2(aq) + 2 H2O(l)
If 28.15 mL of 0.100 M ammonium hydroxide is required to neutralize 10.0 mL of sulfuric acid, what is the molarity of the acid? H2SO4(aq) + 2 NH4OH(aq) → (NH4)2SO4(aq) + 2 H2O(l)
If 27.05 mL of 0.105 M ammonium hydroxide is required to neutralize 10.0 mL of sulfurous acid, what is the molarity of the acid? H2SO3(aq) + 2 NH4OH(aq) → (NH4)2SO3(aq) + 2 H2O(l)
If 42.45 mL of 0.500 M lithium hydroxide is required to neutralize 50.0 mL of phosphoric acid, what is the molarity of the acid? H3PO4(aq) + 3 LiOH(aq) → Li3PO4(aq) + 3 H2O(l)
If 45.05 mL of 0.488 M lithium hydroxide is required to neutralize 50.0 mL of phosphorous acid, what is the molarity of the acid? H3PO3(aq) + 3 LiOH(aq) → Li3PO3(aq) + 3 H2O(l)
Given the molarity and density for each of the following acidic solutions, calculate the mass/mass percent concentration.(a) 6.00 M HCl (d = 1.10 g/mL)(b) 1.00 M HC2H3O2 (d = 1.01 g/mL)(c) 0.500 M HNO3 (d = 1.01 g/mL)(d) 3.00 M H2SO4 (d = 1.18 g/mL).
Given the molarity and density for each of the following basic solutions, calculate the mass/mass percent concentration.(a) 3.00 M NaOH (d = 1.12 g/mL)(b) 0.500 M KOH (d = 1.02 g/mL)(c) 6.00 M NH3 (d = 0.954 g/mL)(d) 1.00 M Na2CO3 (d = 1.10 g/mL).
What is the molarity of hydrochloric acid if 33.25 mL of HCl is required to neutralize 1.115 g of sodium hydrogen carbonate? HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO2(g).
What is the molarity of hydrochloric acid if 29.75 mL of HCl is required to neutralize 0.515 g of sodium carbonate? 2 HCl(aq) + Na2CO3(aq) → 2 NaCl(aq) + H2O(l) + CO2(g).
What is the molarity of lithium hydroxide if 28.85 mL of LiOH is required to neutralize 0.506 g of oxalic acid, H2C2O4? H2C2O4(aq) + 2 LiOH(aq) → Li2C2O4(aq) + H2O(l)
What is the molarity of potassium hydroxide if 29.05 mL of KOH is required to neutralize 0.627 g of oxalic acid, H2C2O4? H2C2O4(aq) + 2 KOH(aq) → K2C2O4(aq) + 2 H2O(l)
What volume of 0.128 M calcium hydroxide is required to neutralize 1.466 g of potassium hydrogen phthalate, KHC8H4O4 (204.23 g/mol)? 2 KHC8H4O4(aq) + Ca(OH)2(aq) → CaK2(C8H4O4)2(aq) + 2 H2O(l)
What volume of 0.150 M barium hydroxide is required to neutralize 1.655 g of potassium hydrogen phthalate, KHC8H4O4 (204.23 g/mol)? 2 KHC8H4O4(aq) + Ba(OH)2(aq) → BaK2(C8H4O4)2(aq) + 2 H2O(l)
Ascorbic acid, abbreviated HAsc, is the chemical name for vitamin C. If 30.95 mL of 0.176 M NaOH neutralizes 0.959 g of acid, what is the molar mass of vitamin C? HAsc(aq) + NaOH(aq) → NaAsc(aq) + H2O(l)
Tartaric acid, abbreviated H2Tart, gives grapes a sour taste. If 28.15 mL of 0.295 M NaOH neutralizes 0.623 g of acid, what is the molar mass of tartaric acid? H2Tart(aq) + 2 NaOH(aq) → Na2Tart(aq) + 2 H2O(l)
Indicate each of the following for the ionization of pure water.(a) The simplified ionization equation(b) The ionization constant equation, Kw(c) The ionization constant at 25 °C.
Indicate each of the following for the ionization of pure water.(a) The molecular collision equation(b) The molar hydrogen ion concentration at 25 °C(c) The molar hydroxide ion concentration at 25 °C.
Given the molar concentration of hydrogen ion, calculate the concentration of hydroxide ion.(a) [H+] = 0.025(b) [H+] = 0.000 017.
Given the molar concentration of hydrogen ion, calculate the concentration of hydroxide ion.(a) [H+] = 6.2 x 10–7(b) [H+] = 4.6 x 10–12.
Given the molar concentration of hydroxide ion, calculate the concentration of hydrogen ion.(a) [OH–] = 0.0016(b) [OH–] = 0.000 29.
Given the molar concentration of hydroxide ion, calculate the concentration of hydrogen ion.(a) [OH–] = 8.8 x 10–8(b) [OH–] = 4.6 x 10–13.
Calculate the pH of each of the following given the molar hydrogen ion concentration.(a) Soft drink, [H+] = 0.001 M(b) Coffee, [H+] = 0.000 01 M.
Calculate the pH of each of the following given the molar hydrogen ion concentration.(a) Egg white, [H+] = 0.000 000 01 M(b) Sour milk, [H+] = 0.000 001 M.
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