Chapter 4 Part 2 Mastering Chemistry
15. What is the oxidation state of Cl in each of the following ions? Part A ClO− Part B ClO−2 Part C ClO−3 Part D ClO−4
Part A: 1 Part B: 3 Part C: 5 Part D: 7
12. Part A Which element is oxidized in this reaction? 2CuO+C→2Cu+CO2 Enter the chemical symbol of the element. Part B Which substance is the oxidizing agent in this reaction? 2CuO+C→2Cu+CO2 Express your answer as a chemical formula. Part C Which element is reduced in this reaction? 16H^+ + 2Cr2O7^2− + C2H5OH → 4Cr^3+ + 11H2O+2CO2 Enter the chemical symbol of the element. Part D Which substance is the reducing agent in this reaction? 16H^+ + 2Cr2O7^2− + C2H5OH → 4Cr^3+ + 11H2O + 2CO2 Express your answer as a chemical formula.
Part A: C is oxidized Part B: CuO is the oxidizing agent Part C: Cr is reduced Part D: C2H5OH is the reducing agent.
13. Determine the oxidation state of nitrogen in NO. A. +2 B. 0 C. +3 D. +5 E. +4
+2
14. Determine the oxidation state of P in PO3^3-. A. -3 B. +2 C. +6 D. 0 E. +3
+3
11. In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution? A. 0.775 M B. 0.387 M C. 1.29 M D. 0.194 M
0.194 M
17. A 32.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.28 mL of NaOH solution is added. Part A What is the concentration of the unknown H3PO4 solution? The neutralization reaction is H3PO4(aq) + 3NaOH(aq) → 3H2O(l) + Na3PO4(aq) concentration =
2.74×10^−2 M
6. If 18.2 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia? Express your answer with the appropriate units.
2.91 M
3. When aqueous solutions of sodium iodide, NaI, and lead(II) acetate, Pb(C2H3O2)2, are mixed, which of the following correctly describes the outcome? Hints A. No reaction occurs when these two solutions are mixed. B.A precipitate of sodium acetate, NaC2H3O2, is formed when the solutions are mixed. C. These two aqueous solutions cannot form a precipitate because both reactants are soluble. D. A precipitate of lead(II) iodide, PbI2, is formed when the solutions are mixed.
A precipitate of lead(II) iodide, PbI2, is formed when the solutions are mixed.
7. Part A Classify these compounds as acid, base, salt, or other. Drag the appropriate items to their respective bins.
Acid: HCOOH and HNO3 Base: NaOH and NH3 Salt: NaBr and KCl Other: CO2 and CH3CH3
5. What is formed when hydrobromic acid, HBr, and calcium hydroxide, Ca(OH)2, are combined? Hints A. Water, H2O, is formed. B. Both water, H2O, and a salt, CaBr2, are formed. C. A salt, CaBr2, is formed. D. Nothing is formed; HBr and Ca(OH)2 do not react with each other.
Both water, H2O, and a salt, CaBr2, are formed.
8. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed. A. H2^2+(aq) + OH-(aq) → H2(OH)2(l) B. H+(aq) + OH-(aq) + 2 K+(aq) + SO4^2-(aq) → H2O(l) + K2SO4(s) C. H+(aq) + OH-(aq) → H2O(l) D. 2 K+(aq) + SO4^2-(aq) → K2SO4(s) E. No reaction occurs.
H+(aq) + OH-(aq) → H2O(l)
9. Identify the spectator ions in the following molecular equation. LiCl(aq) + AgNO3(aq) → AgCl(s) + LiNO3(aq) A. Ag+ and Cl- B. Li+ and Cl- C. Ag+ and NO3- D. Li+ and NO3- E. There are no spectator ions in this reaction.
Li+ and NO3-
10. Which of the following pairs of aqueous solutions will form a precipitate when mixed? A. MgCl2 + KOH B. Li2S + HF C. HI + LiOH D. K2CO3 + HNO3 E. All of these solution pairs will produce a precipitate.
MgCl2 + KOH
2. Which of the ionic compounds shown below will be soluble in water? Hints Fe(OH)3 Na2SO4 AgCl Ag2CO3
Na2SO4
4. Which statement below concerning molecular, complete ionic, and net ionic equations, is true? Hints A. Weak electrolytes are written as ions in complete ionic equations. B. Only spectator ions are seen in the net ionic equation. C. Net ionic equations only show the species that actually change during the reaction. D. In molecular equations, strong electrolytes are shown as ions.
Net ionic equations only show the species that actually change during the reaction.
1. Part A Each of the following reactions shows a solute dissolved in water. Classify each solute as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. M(l)→M(aq) AC(aq)⇌A+(aq)+C−(aq) BD(s)→B+(aq)+D−(aq) PR(aq)→P+(aq)+R−(aq) N(s)→N(aq) Drag the appropriate items to their respective bins. Part B Classify each of these soluble solutes as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. Solutes Formula Nitric acid HNO3 Calcium hydroxide Ca(OH)2 Carbonic acid H2CO3 Methyl amine CH3NH2 Aluminum chloride AlCl3 Ethanol C2H5OH Sucrose C12H22O11 Drag the appropriate items to their respective bins.
Part A: Strong electrolyte: BD and PR Weak electrolyte: AC nonelectrolyte: M and N Part B: Strong electrolyte: Nitric acid, Aluminum chloride and Calcium hydroxide Weak electrolyte: Carbonic acid and Methyl amine nonelectrolyte: Sucrose and Ethanol
16. Part A Determine whether each of the following compounds is soluble or insoluble: Drag the appropriate items to their respective bins. Part B Write the ions present in a solution of Na2CO3. Express your answers as chemical formulas separated by a comma. Offset subscripts and charges on each ion.
Part A: Soluble: Na2CO3 Insoluble: AlPO4, PbSO4, AgI Part B: Na+ and CO3^2−