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Chemistry 2

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Name _________________________________ I.D. Number _______________________ Unit 3 Evaluation Evaluation 03 Chemistry 2 (SCIH 032 062) This evaluation will cover the lessons in this unit. It is open book, meaning you can use your textbook, syllabus, and other course materials. You will need to understand, analyze, and apply the information you have learned in order to answer the questions correctly. To submit the evaluation, follow the directions provided. Matching Match each of the following terms to its correct definition. a. acid dissociation constant b. diprotic acid c. hydrogen-ion donor d. Lewis acid e. pH _____ 1. can accept an electron pair _____ 2. acid with two ionizable protons _____ 3. Brønsted-Lowry acid _____ 4. negative logarithm of the hydrogen ion concentration _____ 5. ratio of the concentration of the dissociated to the undissociated form Multiple-Choice Select the response that best completes the statement or answers the question. _____ 6. When an acid reacts with a base, what compounds are formed? a. b. c. d. Unit 3 Evaluation a salt only water only metal oxides only a salt and water 103 SCIH 032 _____ 7. What is the formula for phosphoric acid? a. b. c. d. _____ 8. Which of the following is a property of an acid? a. b. c. d. _____ H2PO4 H3PO4 HPO4 H2PO3 sour taste nonelectrolyte strong color unreactive 9. What is a property of a base? a. b. c. d. bitter taste watery feel strong color unreactive _____ 10. The formula of the hydrogen ion is written as _________. a. b. c. d. OHH3O+ H+ NH4+ _____ 11. Which of these compounds yields the lowest concentration of hydroxide ions in aqueous solution? a. b. c. d. sodium hydroxide potassium hydroxide calcium hydroxide magnesium hydroxide _____ 12. What is an acid according to the Arrhenius definition? a. b. c. d. a substance that ionizes to yield protons in aqueous solution a substance that is a hydrogen ion a substance that accepts an electron pair in aqueous solution a substance that is a hydrogen ion acceptor _____ 13. Which of these compounds or ions is an Arrhenius base? a. b. c. d. Unit 3 Evaluation LiOH NH3 H3PO4 CH3COO- 104 SCIH 032 _____ 14. What is transferred between a conjugate acid-base pair? a. b. c. d. an electron a proton a hydroxide ion a hydronium ion _____ 15. A Lewis acid is a substance that can _________. a. b. c. d. donate a pair of electrons accept a pair of electrons donate a hydrogen ion accept a hydrogen ion _____ 16. Why would you use more than one indicator to determine the pH of a solution? a. b. c. d. Indicators generally change color over narrow ranges of pH. Indicators can only determine if a solution is acidic or basic. Indicators are not stable in solution so the pH must be rechecked. Most indicators are not very reliable so you need to use more than one. _____ 17. How does an indicator provide information about the pH of a solution? a. b. c. d. by reacting with acids or bases in solution and forming a colored complex by dissociating into ions that have a different color than the molecular form by reducing the number of free hydronium or hydroxide ions in solution by causing the acid or base in solution to dissociate into a colored form _____ 18. Which compound can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base? a. b. c. d. water ammonia sodium hydroxide hydrochloric acid _____ 19. How many moles of calcium hydroxide, Ca(OH)2, are needed to neutralize 2 moles of sulfuric acid, H2SO4? a. b. c. d. 1 2 4 8 _____ 20. Which of the following represents a Brønsted-Lowry conjugate acid-base pair? a. b. c. d. Unit 3 Evaluation SO3 and SO2 CO2 and CO3-2 HO- and H+ NH3 and NH4+ 105 SCIH 032 _____ 21. What is the charge on the hydronium ion? a. b. c. d. 2– 1– 0 1+ _____ 22. How much H3PO4 is needed to neutralize 1 liter of a 0.75M solution of NaOH? a. b. c. d. ____ 23. 0.25 mol 0.75 mol 1.0 mol 2.25 mol What is the best description for a solution with a hydroxide-ion concentration equal to 1 x 10-5 M? a. b. c. d. acidic basic neutral The answer cannot be determined. _____ 24. In a neutral solution, [H+] is _________. a. b. c. d. 10M zero 1 x 10-14 M equal to [OH-] _____ 25. What is pH? a. b. c. d. the positive logarithm of the hydrogen ion concentration the negative logarithm of the hydrogen ion concentration the negative logarithm of the hydroxide ion concentration the positive logarithm of the hydroxide ion concentration _____ 26. Which type of solution is one with a pH of 8? a. b. c. d. acidic neutral basic The type varies, depending on the solution. _____ 27. Which of these solutions is the most basic? a. b. c. d. Unit 3 Evaluation [H+] = 1 x 10-4M [OH-] = 1 x 10-4M [H+] = 1 x 10-14M [OH-] = 1 x 10-14M 106 SCIH 032 _____ 28. How can all indicators be described? a. b. c. d. oxidizing agent weak base or acid strong base or acid salt _____ 29. What characterizes a strong acid or base? a. b. c. d. polar covalent bonding complete ionization in water ionic bonding presence of a hydroxide or hydrogen ion _____ 30. The acid dissociation constant for an acid dissolved in water is equal to the _________. a. b. c. d. equilibrium constant equilibrium constant divided by the concentration of water equilibrium constant times the concentration of water equilibrium constant times the equilibrium constant of water _____ 31. In reference to solutions of strong acids and strong bases, the word strong refers to _________. a. b. c. d. normality molarity solubility degree of ionization _____ 32. What is another name for the acid dissociation constant? a. b. c. d. equilibrium constant ionization constant rate constant mole fraction Matching Match each of the following terms to its correct definition. a. salt hydrolysis b. end point c. titration d. equivalence point e. buffer capacity Unit 3 Evaluation 107 SCIH 032 _____ 33. process of adding a known amount of solution of known concentration to determine the concentration of another solution _____ 34. the number of moles of hydrogen ions equals the number of moles of hydroxide ions _____ 35. indicator changes color _____ 36. cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water _____ 37. the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs Multiple-Choice Select the response that best completes the statement or answers the question. _____ 38. Which combination of acid and salt in aqueous solution would form a buffer? a. b. c. d. hydrochloric acid and potassium chloride carbonic acid and sodium carbonate sulfuric acid and calcium sulfate nitric acid and magnesium nitrate _____ 39. Which phrase best describes a 0.012M solution of an acid that ionizes only slightly in water? a. b. c. d. concentrated and weak strong and dilute dilute and weak concentrated and strong _____ 40. Which of the following pairs of compounds consists of a weak acid and a strong base? a. b. c. d. sulfuric acid, sodium hydroxide acetic acid, ammonia acetic acid, sodium hydroxide nitric acid, calcium hydroxide _____ 41. A substance with a Ka of 1.8 x 10-5 would be classified as a _________. a. b. c. d. Unit 3 Evaluation strong acid weak acid strong base weak base 108 SCIH 032 _____ 42. A substance with a Kb of 1.8 x 10-5 would be classified as a _________. a. b. c. d. strong acid weak base strong base weak acid _____ 43. When will the acidity of a buffer solution consisting of ammonium ions and ammonia molecules increase? a. b. c. d. when the added acid exceeds the number of ammonia molecules available when the added acid exceeds the number of ammonium ions available when all of the water in the solution is converted to hydrogen ions when some of the water in the solution is converted to hydroxide ions _____ 44. Which pH value could represent the equivalence point of the titration of a strong base and a weak acid? a. b. c. d. pH 0 pH 5 pH 7 pH 9 _____ 45. Which acid has the greatest acid dissociation constant? a. b. c. d. nitric acid acetic acid carbonic acid boric acid _____ 46. Which of the following describes an aqueous solution of ammonium sulfate? a. b. c. d. weakly acidic neutral weakly basic strongly basic _____ 47. Which base has the smallest base dissociation constant? a. b. c. d. Unit 3 Evaluation potassium hydroxide sodium hydroxide calcium hydroxide ammonia 109 SCIH 032 _____ 48. A buffer is a solution that resists change in pH when a small amount of acid or base is added. a. true b. false _____ 49. In a titration, what happens when the number of moles of hydrogen ions equals the number of moles of hydroxide ions? a. b. c. d. The equivalence point has been reached. The end-point has been reached. The point of neutralization has been reached. The titration has failed. _____ 50. Which of the following describes an aqueous solution of potassium bromide? a. b. c. d. weakly acidic neutral weakly basic strongly basic Carefully check your answers on this evaluation and make any corrections you feel are necessary. When you are satisfied that you have answered the questions to the best of your ability, transfer your answers to an answer sheet. Please refer to the information sheet that came with your course materials. Unit 3 Evaluation 110 SCIH 032
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Explanation & Answer

Here are the answers, please tell me if you have any problem.

1.
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d.
b.
c.
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a.

6. d.
7. b.
8. a.
9. a.
10.c.
11.d.
12.a.
13.a.
14.b.
15.b.
16.a.
17.b.
18.a.
19.b.
20.d.
21.d.
22.a.
23.b.
24.d.
25.b.
26.c.
27.c.
28.b.
29.b.
30.a.
31.d.
32.b.

Lewis acid
diprotic acid
hydrogen-ion donor
pH
acid dissociation constant

a salt and water
H3PO4
sour taste
bitter taste
H+
magnesium hydroxide
a substance that ionizes to yield protons in aqueous solution
LiOH
a proton
accept a pair of electrons
Indicators genera...


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