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Chapter 15 Review

Chapter 15 Review. Chemistry I Pre-AP Mr. Chuang. Question 1. Certain solutions are strongly basic due to the high concentration of. (A) oxide ions. (D) hydroxide ions. (B) potassium ions. (E) hydronium ions. (C) ammonium ions.

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Chapter 15 Review

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  1. Chapter 15 Review Chemistry I Pre-AP Mr. Chuang

  2. Question 1 Certain solutions are strongly basic due to the high concentration of (A) oxide ions. (D) hydroxide ions. (B) potassium ions. (E) hydronium ions. (C) ammonium ions.

  3. According to the Brønsted–Lowry concept of acid–base reactions, the acids in the equation are H2O + CO32– HCO3– + OH– Question 2 (A) H2O and OH– (D) CO32– and HCO3– (B) HCO3– and OH– (E) H2O and CO32– (C) H2O and HCO3–

  4. Question 3 What is the conjugate base of the acid H3PO4? (A) H3O+(aq) (C) H2PO4–(aq)   (B) H2O(l) (D) OH–(aq)

  5. Question 4 Which of these is a conjugate acid–base pair?   (A) NH4+, H2O (D) OH–, NH3   (B) NH4+, NH3 (E) HCl, NaOH (C) H2O, NH3

  6. Question 5 To prepare a buffer solution, which substance should be added to a 1.0 M solution of acetic acid, CH3COOH?   (A) HCl (D) CH3COONa (B) H2O (E) CH3OH (C) CaCl2

  7. Question 6 Which compound acts either as an acid or a base in solution? (A) NH3 (D) Ca(OH)2 (B) NaOH (E) HSO3– (C) H2SO4

  8. Question 7 Assuming complete ionization, the pH of a 0.01 M HCl solution would be (A) l (B) 2 (C) 3 (D) 4   (E) 0.5

  9. Question 8 What is the hydrogen–ion concentration, [H+], in an aqueous solution of pH 3? (A) 3 M (D) 103 M (B) 10–3 M (E) 10–14M (C) 10–2 M

  10. Question 9 How does the pH of the mixture change as hydrochloric acid, HCl, is slowly added to a solution of sodium hydroxide, NaOH?   (A) The pH decreases and may go below 7.   (B) The pH increases and may go above 7.   (C) The pH decreases to 7 and stops.   (D) The pH increases to 7 and stops.

  11. Question 10 What is the hydroxide ion concentration, [OH–] of a solution having a pH of 4? (A) 1x101 M (D) 1x10–10 M   (B) 4x100 M (E) 1x10–14 M   (C) 1x10–4 M

  12. Question 11 What is the OH– concentration in a solution whose H3O+ concentration is 2.0 x 10–5 M? (A) 2.0x10–10 M (D) 2.0x109 M (B) 2.0x10–5 M (E) 5.0 x 10–5 M (C) 5.0x10–10 M

  13. Question 12 Which of the following is the weakest base? (A) Cl- (D) NH3 (B) OH- (E) F- (C) C2H3O2-

  14. Question 13 The pOH of a 0.2 M solution of HNO3 will be _____ the pOH of a 0.2 M solution of HC2H3O2. (A) greater than (B) less than (C) equal to (D) impossible to tell

  15. Question 14 Which of the following will have the lowest pH? (A) 0.100 M HCl (D) 0.100 M NaOH (B) 0.100 M HF (E) 0.010 M NaOH (C) 0.0010 M HCl

  16. Question 15 Which of the following will have the highest pOH? (A) 1.0 M HF (D) 0.10 M HNO3 (B) 1.0 NaOH (E) 0.10 M NaOH (C) 1.0 M HNO3

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