Question 1 Which of the following are generally considered to be nonelectrolytes? A) Soluble ionic compounds B) Strong acids C) Weak acids D) None of the above
Question 2 Which of the following are generally considered to be strong electrolytes? A) Strong acids B) Soluble ionic compounds C) Weak acids D) Both A and B
Question 3 Compounds containing the nitrate ions are generally soluble with the exception of silver nitrate. A) True B) False
Question 4 Compounds containing the ammonium ion are generally soluble. A) True B) False
Question 5 A precipitate will form when a solution of silver nitrate is mixed with a solution of sodium bromide. A) True B) False
Question 6 Mixing which of the following pairs of substances in aqueous solution will result in a precipitate being formed? A) sodium nitrate and ammonium bromide B) sodium hydroxide and hydrochloric acid C) calcium chloride and sodium carbonate D) All of the above
Question 7 Which of the following types of substances should be represented as separated ions in an ionic equation? A) Insoluble ionic compounds B) Weak acids and bases C) Water D) Strong acids or soluble ionic compounds (strong electrolytes)
Question 8 Which of the following "rules" for assigning oxidation numbers is incorrect? A) The oxidation number of an elemental substance is determined by its group number. B) The oxidation numbers of the atoms in a polyatomic ion add up to zero. C) In an ionic compound, the oxidation number is equal to the subscript in the compound formula. D) All of the above are incorrect.
Question 9 If 2.000 mol of ethanol liquid (volume around 100 mL) is mixed with 1.000 L of water, the solution will be 1.000 M in ethanol. A) True B) False
Question 10 How many mL of 2.0 M hydrochloric acid would be required to prepare 200.0 mL of 1.0 M HCl? A) 50.0 mL B) 100.0 mL C) 400.0 mL D) Depends on how much of the 2.0 M hydrochloric acid you have available
Question 11 When calcium carbonate is placed in water, which of the following best describes what is present in the mixture? A) calcium carbonate molecules only B) calcium ions and carbonate ions only C) mostly calcium ions and carbonate ions and little undissociated calcium carbonate D) a few calcium ions and carbonate ions and a lot of undissociated calcium carbonate E) hydrated calcium and carbonate ions only
Question 12 Ammonium sulfide and mercuric bicarbonate are expected to be A) both soluble. B) soluble and insoluble. C) insoluble and soluble. D) both insoluble.
Question 13 Which of the following salts is expected to be soluble? A) Silver chloride B) Mercuric sulfate C) Silver chlorate D) Barium sulfate E) Lead iodide
Question 14 The equation Fe 3+ (aq) + 3OH - (aq) → Fe(OH) 3 represents A) a balanced molecular equation. B) a balanced ionic equation. C) a balanced net ionic equation. D) a dissociation reaction. E) an example of a redox reaction.
Question 15 Which of the following is not an acid/conjugated base pair? A) sulfuric acid / sulfate ion B) ammonia / ammonium ion C) water / hydroxide ion D) phosphoric acid / dihydrogen phosphate ion E) dihydrogen phosphate ion / hydrogen phosphate ion
Question 16 Which of the following species should be considered a weak Bronsted acid? A) HI B) OH- C) HNO 3 D) HClO 4 E) None of the above
Question 17 Which of the following species is not amphoteric? A) Al 2 O 3 B) H 2 O C) H 2 PO 4 - D) HPO 4 2- E) PO 4 3-
Question 18 In which of the following species is the oxidation number of manganese highest? A) MnO 2 B) Mn 2 (SO 4 ) 3 C) K 2 MnO 4 D) KMnO 4 E) MnO 3
Question 19 Which of the following equations does not represent a redox reaction? A) Cu + 2AgNO 3 → 2Ag + Cu(NO 3 ) 2 B) 2CrO 4 2- + 2H + → Cr 2 O 7 2- + H 2 O C) 2SO 2 + O 2 → 2SO 3 D) 2H 2 + O 2 → 2H 2 O E) All are redox
Question 20 A sample of oxalic acid (a diprotic acid of the formula H 2 C 2 O 4 ) is dissolved in enough water to make 1.00 L of solution. A 100.0 mL sample of this solution is titrated with a solution of sodium hydroxide of concentration 0.750 M and requires 20.0 mL of sodium hydroxide to reach the end point. Calculate the mass of the original oxalic acid sample. A) 6.75 g B) 0.675 g C) 1.35 g D) 13.5 g E) None of the above
23.48mL of a NaOH solution are needed to neutralize 0.5468g of KHP (MW 204.2 g/mol). What is the concentration of the base solution? 1. 0.1141M 2. 0.002678M 3. 1.14M 4. Can’t tell
Answer Key – Chapter 4 1. D 2. D 3. B 4. A 5. A 6. C 7. D 8. D 9. B 10. B 11. D 12. A 13. C 14. C 15. A 16. B 17. E 18. D 19. B 20. A