CHEM Chapter 11 Quizlet

1) According to the Arrhenius concept, if NaOH were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydronium ions. D) a source of H- ions. E) a proton donor.

2) According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as A) a base. B) an acid. C) a source of hydroxide ions. D) a source of H- ions. E) a proton acceptor.

3) The name given to an aqueous solution of HBr is A) hydrogen bromide. B) hydrobromic acid. C) bromic acid. D) bromous acid. E) hypobromous acid.

4) The name given to an aqueous solution of HNO3 is A) nitric acid. B) nitrous acid. C) hydrogen nitrate. D) hydronitrogen acid. E) hyponitric acid.

5) The name given to an aqueous solution of HClO3 is A) chlorous acid. B) hypochlorous acid. C) chloric acid. D) hydrochloric acid. E) hypochloric acid.

6) Which one of the following is characteristic of a base? A) produces H3O+ in water B) has a sour taste C) has a slippery, soapy feel D) turns blue litmus red E) is insoluble in water

7) The correct formula for sulfuric acid is A) H2SO4. B) H2SO3. C) H2SO4-. D) H2SO3-. E) SO42-.

8) The name of Al(OH)3 is A) aluminum trihydroxide. B) monoaluminum trihydroxide. C) aluminum hydroxide. D) aluminum(III) hydroxide. E) aluminum oxygen hydride.

9) According to the Brønsted-Lowry definition, A) an acid is a proton acceptor. B) a base produces H+ ions in aqueous solutions. C) a base is a proton donor. D) a base is a proton acceptor. E) an acid acts as the solvent

10) Identify the Brønsted-Lowry acids in the following reaction. H2O + CO32- → HCO3- + OH- A) H2O/HCO3- B) CO32-/HCO3- C) OH-/HCO3- D) CO32-/OH- E) H2CO3/H2O

11) The conjugate base of HClO3 is A) HClO2. B) ClO3-. C) Cl(OH)2. D) ClO3. E) HClO.

12) The conjugate acid of HSO4- is A) SO42-. B) HSO4. C) H2SO4. D) H2SO4-. E) HSO3-.

13) Which of the following is the strongest acid? A) H3PO4 B) NH4+ C) NaOH D) H2CO3 E) HCl

14) The stronger the acid, the ________ the conjugate base. A) stronger B) weaker

15) Which of the following is the strongest base? A) H3PO4 B) NH3 C) NaOH D) NaCl E) HCl

16) Which of the following is correctly identified? A) NH3, strong acid B) NaOH, strong base C) HCl, weak acid D) H2CO3, strong acid E) Ca(OH)2, weak base

17) Ammonium hydroxide is a weak base because A) it is a dilute solution. B) it is only slightly soluble in water. C) it cannot hold on to its hydroxide ions. D) it dissociates only slightly in water. E) it is completely ionized in aqueous solution.

18) Which of the following is the strongest acid? A) HF (Ka for HF is 7.2 × 10-4) B) HCN (Ka for HCN is 4.9 × 10-10) C) HCNO (Ka for HCNO is 2 × 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 × 10-10)

19) Which of the following is the weakest acid? A) HF (Ka for HF is 7.2 × 10-4) B) HCN (Ka for HCN is 4.9 × 10-10) C) HCNO (Ka for HCNO is 2 × 10-4) D) H3BO3 (Ka for H3BO3 is 5.4 × 10-10)

20) The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is A) neutral in water solution. B) able to react with HCl. C) a weak acid. D) a strong acid. E) ionic.

21) Predict whether the equilibrium of the following reaction favors reactants or products: NH4+ + H2O ⇌ NH3 + H3O+ A) Reactants are favored. B) Products are favored. C) Neither side is favored.

22) For Kw, the product of [ H3O+] and [OH-] is A) 1.0 × 10-14. B) 1.0 × 10-7. C) 1.0 × 10-1. D) 1.0. E) 1.0 × 1014.

23) Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution? A) In acids, [OH-] is greater than [ H3O+]. B) In bases, [OH-] = [ H3O+]. C) In neutral solutions, [ H3O+] = [ H2O]. D) In bases, [OH-] is greater than [ H3O+]. E) In bases, [OH-] is less than [ H3O+].

24) What is the [ H3O+] in a solution with [OH-] = 1 × 10-12 M? A) 1 × 10-12 M B) 1 × 102 M C) 1 × 10-7 M D) 1 × 10-8 M E) 1 × 10-2 M

25) What is the [OH-] in a solution that has a [ H3O+] = 1 × 10-6 M? A) 1 × 10-2 M B) 1 × 10-6 M C) 1 × 10-8 M D) 1 × 10-10 M E) 1 × 10-12 M

26) What is the [OH-] in a solution that has a [ H3O+] = 2.0 × 10-4 M? A) 2.0 × 10-10 M B) 5.0 × 10-10 M C) 1.0 × 10-10 M D) 2.0 × 10-4 M E) 5.0 × 10-11 M

27) What is the [ H3O+] in a solution that has a [OH-] = 5.0 × 10-2 M? A) 2.0 × 10-12 M B) 2.0 × 10-2 M C) 1.0 × 10-14 M D) 2.0 × 10-4 M E) 5.0 × 10-12 M

28) A solution which has [ H3O+] = 6.7 × 10-8 M is A) acidic. B) basic. C) neutral.

29) A solution which has [OH-] = 4.6 × 10-6 M is A) acidic. B) basic. C) neutral.

30) A solution which has [OH-] = 3.4 × 10-12 M is A) acidic. B) basic. C) neutral..

31) A solution with a pH of 4 is A) extremely acidic. B) moderately acidic. C) neutral. D) slightly basic. E) extremely basic.

32) What is the pH of a solution with [ H3O+] = 1 × 10-9 M? A) 1.0 × 10-5 M B) -9.0 C) 5.0 D) -5.0 E) 9.0

33) What is the pH of a solution with [ H3O+] = 3.0 × 10-3 M? A) 3.0 × 10-3 B) 2.52 C) 3.0 D) -2.52 E) 9.0

34) What is the pH of a solution with [OH-] = 1 × 10-4 M? A) 10.0 B) -10.0 C) 4.0 D) -4.0 E) 1.0 × 10-10

35) What is the pH of a solution with [OH-] = 2.0 × 10-10 M? A) 9.70 B) -9.70 C) 4.30 D) -4.30 E) 2.0 × 10-10

36) The [ H3O+] of a solution with pH = 2 is A) 10 M. B) -10 M. C) 1 × 102 M. D) 1 × 10-2 M. E) 1 × 10-12 M.

37) In which of the following are the pH values arranged from the most basic to the most acidic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 11 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

38) In which of the following are the pH values arranged from the most acidic to the most basic? A) 1, 3, 6, 8, 11, 14 B) 2, 5, 7, 9, 10, 1.1 C) 14, 10, 7, 4, 3, 1 D) 14, 10, 7, 1, 3, 5 E) 7, 10, 14, 4, 3, 1

39) In a sulfuric acid solution, where the [ H3O+] is 0.01 M, what is the pH? A) pH = 12.0 B) pH = 2.0 C) pH = 3.0 D) pH = 11.0 E) pH = 5.0

40) The [ H3O+] of a solution with pH = 5.60 is A) 3 × 10-6 M. B) 2.5 × 10-8 M. C) 2.5 × 10-6 M. D) 4.0 × 10-6 M. E) 4.0 × 10-9 M.

41) The [OH-] of a solution with pH = 8.34 is A) 5 × 10-9 M. B) 4.6 × 10-9 M. C) 2.2 × 10-9 M. D) 3 × 10-6 M. E) 2.2 × 10-6 M.

42) When a piece of magnesium metal is added to hydrochloric acid, what gas is produced? A) oxygen B) chlorine C) nitrogen D) carbon dioxide E) hydrogen

43) An acid and base react to form a salt and water in a(n) ________ reaction. A) ionization B) dissociation C) oxidation D) neutralization E) reduction

44) In a neutralization reaction A) two acids react to form water. B) water and a salt react to form an acid and a base. C) an acid and a salt react to form water and a base. D) a base and a salt react to form water and an acid. E) an acid and a base react to form a salt and water.

45) Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 with Ca(OH)2? A) H3PO4 + Ca(OH)2 → CaHPO4 + 2H2O B) 3H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5H2O C) H3PO4 + Ca(OH)2 → Ca3(PO4)2+ H2O D) 2H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6H2O E) 4H3PO4 + 6Ca(OH)2 → 2Ca3(PO4)2 + 12H2O

46) The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula A) H2O. B) AlNO3. C) AlH2. D) Al(NO3)3. E) NO3OH.

47) How many moles of H2O are produced when 1 mole of Mg(OH)2 reacts with 1 mole of H2SO4? A) 1 B) 2 C) 3 D) 4 E) 5

48) In a neutralization reaction, how many moles of HClO4 react with 1 mole of Al(OH)3? A) 1 B) 2 C) 3 D) 4 E) 5

49) Which of the following is a neutralization reaction? A) KCl + NaNO3→ KNO3 + NaCl B) HNO3+ KOH → H2O + KNO3 C) H2O + SO3 → H2SO4 D) 4Na + O2 → 2Na2O E) 2NO2 → 2NO + O2

50) 25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is A) 0.212 M. B) 0.115 M. C) 0.500 M. D) 0.390 M. E) 0.137 M.

51) What is the molarity of a KOH solution if 25.0 mL neutralizes 35.0 mL of a 0.200 M HCl solution? A) 0.267 M B) 0.143 M C) 0.200 M D) 0.280 M E) 0.100 M

52) A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid? H3PO4 + 3NaOH →Na3PO4 + 3H2O A) 0.333 M B) 3.00 M C) 1.50 M D) 1.00 M E) 0.750 M

53) A 25.0 mL sample of H2SO4 requires 20.0 mL of 2.00 M KOH for complete neutralization. What is the molarity of the acid? H2SO4 + 2KOH → K2SO4 + 2H2O A) 2.00 M B) 2.50 M C) 0.800 M D) 1.60 M E) 1.25 M

54) A 10.0 mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is A) 0.207 M. B) 0.4141 M. C) 0.0708 M. D) 0.428 M. E) 0.142 M.

55) How many milliliters of 0.400 M NaOH are required to completely neutralize 20.0 mL of 0.200 M HCl? A) 50.0 mL B) 40.0 mL C) 0.100 mL D) 20.0 mL E) 10.0 mL

56) How many milliliters of 0.200 M NaOH are required to completely neutralize 5.00 mL of 0.100 M H3PO4? A) 7.50 mL B) 2.50 mL C) 0.833 mL D) 5.00 mL E) 15.0 mL

57) How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl? A) 100. mL B) 50.0 mL C) 25.0 mL D) 0.250 mL E) 0.50 mL

For the problem(s) that follow, consider the reaction in which magnesium reacts with an HCl solution . Mg(s) + 2HCl(aq) → MgCl2 (aq) + H2(g) 58) If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution? A) 1.65 M B) 80.0 M C) 8.00 M D) 0.823 M E) 3.29 M

59) The function of a buffer is to A) change color at the end point of a titration. B) maintain the pH of a solution. C) be a strong base. D) maintain a neutral pH. E) act as a strong acid.

60) The normal blood pH is about A) 6.8. B) 7.0. C) 7.2. D) 7.4. E) 7.6.

61) In a buffer system of HF and its salt, NaF, A) the HF neutralizes added acid. B) the HF neutralizes added base. C) the HF is not necessary. D) the F- neutralizes added H2O. E) the F- neutralizes added base.

62) Which of the following is a buffer system? A) NaCl and NaNO3 B) HCl and NaOH C) H2CO3 and KHCO3 D) NaCl and NaOH E) H2O and HCl

63) Which of the following could be a buffer? A) NaF B) HF + NaF C) HF + H2O D) NaF + H2O E) NaCl + HF

64) What is the name of the medical condition of an asthmatic patient with a blood pH of 7.30? A) respiratory acidosis B) respiratory alkalosis C) metabolic acidosis D) metabolic alkalosis E) diabetes mellitus

65) If a condition of hyperventilation occurs, the blood pH of the patient is expected to A) saturate. B) increase. C) decrease. D) stay the same. E) concentrate.

66) When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO2, the blood pH rises in a condition called A) metabolic acidosis. B) metabolic alkalosis. C) respiratory acidosis. D) respiratory alkalosis. E) pulmonary distress.

67) Which solution has the highest pH? A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

68) Which solution has the lowest pH? A) a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate B) a buffer made with 0.10 M acetic acid and 0.10 M sodium acetate C) a buffer made with 0.01 M acetic acid and 0.10 M sodium acetate D) a buffer made with 0.01 M acetic acid and 0.01 M sodium acetate E) All of the buffers have the same pH since they are all made with acetic acid and sodium acetate.

1) The name of HCl is________.

2) The conjugate acid of H2PO42- is ________.

3) Identify the conjugate acid-base pairs in the following reaction: HCl + NH3 → NH4+ + Cl-

4) Write the proper Ka expression for the ionization of acetic acid, HC2H3O2

5) If an acid has a Ka << 1, is it classified as a weak acid or a strong acid?

6) The pH of 0.0010 M HCl is ________.

7) The pH of 0.0001 M KOH is ________.

8) In a titration experiment, a student used 24.13 mL of 0.111 M sodium hydroxide to neutralize 20.00 mL of a hydrochloric acid solution. What was the molarity of the acid solution?

9) A student had 2.0 L of a sodium hydroxide solution that had a concentration of 0.4000 M. The student needed to make 500 mL of a 0.1000 M solution. How many mL of the concentrated solution was needed?

10) A student had 25.0 mL of 0.100 M H2SO4 solution. How many mL of a 0.100 M NaOH solution will the sulfuric acid neutralize?

11) What is the pH of a buffer made with 0.10 M acetic acid and 0.01 M sodium acetate?

1) HCl is hydrochlorous acid.

2) The conjugate base of HCl is Cl-.

3) HCl is a strong acid.

4) A strong acid is completely dissociated in water.

5) In any water solution, [H3O+][OH-] = 1.0 × 10-7.

6) The pH of 0.001 M HCl is 12.0.

7) A solution with a pH of 4.0 is more acidic than a solution with a pH of 6.0.

8) A solution with a pH of 4.0 is basic.

9) Magnesium metal is not attacked by sulfuric acid solutions.

10) For most reactions of acids with bases, the resulting products are a salt and water.

11) If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.

12) Alkalosis is the blood condition in which the blood pH is higher than normal.

13) A buffer is a solution that tends to maintain a neutral pH.

1) HCl

2) NaOH

3) NH3

4) H2SO4

5) CO32-

6) NaCl

7) CN-

8) H2CO3

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 9) acid

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 10) base

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 11) [H3O+] = 1.0 × 10-6 M

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 12) [H3O+] = 1.0 × 10-10 M

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 13) [H3O+] = 1.0 × 10-7 M

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 14) pH = 2

In the following solutions, is the [OH-] greater than, less than, or equal to the [H3O+]? 15) pH = 9

16) has a sour taste

17) has a pH = 4.5

18) turns blue litmus paper red

19) contains more hydronium ions than hydroxide ions

20) H2O

21) [H3O+] = 3.4 × 10-5 M

22) [OH-] = 2.8 × 10-2 M

23) Ca(OH)2

24) pH =9.0

25) [H3O+] = 1.0 × 10-7 M

1) Name the following acids: a) HCl

1) Name the following acids: b) H2SO3

1) Name the following acids: c) H3PO4

1) Name the following acids: d) HI

1) Name the following acids: e) HClO3

2) Write the conjugate base for each of the following acids (subtract H+): a) HNO3

2) Write the conjugate base for each of the following acids (subtract H+): b) H2SO4

2) Write the conjugate base for each of the following acids (subtract H+): c) HCl

2) Write the conjugate base for each of the following acids (subtract H+): d) H2CO3

3) Write the conjugate acid for each of the following bases (add H+): a) NO3^-

3) Write the conjugate acid for each of the following bases (add H+): b) HCN

3) Write the conjugate acid for each of the following bases (add H+): c) OH^-

3) Write the conjugate acid for each of the following bases (add H+): d) H2PO4^-

4) Identify the conjugate acid-base pairs in the following equation: HNO₂ (aq) + H₂O (l) --> H₃O⁺ (aq) + NO₂⁻ (aq)

5) Write an equation showing how the buffer system neutralizes an added acid (H₃O⁺)

6) What is the [OH⁻] of a solution if [H₃O⁺] is 6.2 x 10⁻⁸ M?

7) What is the [H₃O⁺] of a solution if [OH⁻] is 2.7 x 10⁻¹²?

8) Determine the pH of a solution with an [H₃O⁺] of 5.9 x 10⁻⁷.

9) Determine the [OH⁻] of a solution with a pH of 8.3

10) Determine the pH of a 0.600 g KOH in 0.340 L of solution