acid base solutions eadms

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					1. A substance is dissolved in water and produces hydroxide ions. This substance is most likely a(n)
__________.

A acid           B base      C salt        D neutral



2. A student mixes salt with warm water until it dissolves. The salt solution is most likely to have which
characteristic, as compared with plain water?

A better electrical conductivity

B stronger chemical bonds

C a bitter taste

D more free hydrogen ions
3. How can a very strong acid be neutralized?

A Increase the temperature of the solution to 90 °C.

B Add a strong base to the solution.

C Add a salt to the solution.

D Decrease the temperature of the solution to 10 °C.


4. Phenolphthalein is added to a solution. The phenolphthalein turns pink. Which of the following can be
concluded about the solution?

A It is neutral.

B It is basic.

C It is a buffer.

D It is covalent.



5. Magnesium is added to a solution to check for acidity. If the solution is an acid, which of the following
occurs?

A The solution turns yellow.

B Carbon dioxide gas is liberated.

C The solution solidifies.

D Hydrogen gas is liberated



6. A student adds calcium carbonate to a solution. If the solution is an acid, which of the following occurs?

A A small amount of ice forms.

B Carbon dioxide gas is liberated.

C A blue flame forms above the solution.
D The solution turns dark red.
7. An unknown solution is found to have the ability to conduct an electrical current. When iron metal is
exposed to the solution, it reacts and produces an orange precipitate and hydrogen gas. This unknown
solution is best characterized as a (an)

A alcohol.

B base.

C salt.

D acid.


8. Which of the following statements describes a substance that can be characterized as a base?

A changes the color of blue litmus paper to red

B reacts with metals to produce hydrogen gas and a salt

C reacts with substances containing hydrogen ions to produce water and a salt

D neutralizes substances that contain hydroxide ions

9. Which of the following describes a substance that could be characterized as an acid?

A tends to taste bitter and feel slippery

B reacts with substances containing hydroxide ions to produce water and a salt

C changes the color of red litmus paper to blue

D neutralizes substances that contain hydrogen ions
10. You are given a solution from your instructor and asked to determine if it is an acid, base or salt
solution. You run two tests on the substance and in the duration of the tests you observe that it reacted with
certain metals to produce hydrogen gas, and it reacted with metal hydroxides to produce water and
salt. Based on these observations you determine that the solution is a(n) __________.

A acid      B base        C salt solution      D neutral
11. When an acid is mixed with a metal hydroxide you would expect __________.

A the solution to turn red      C hydrogen gas to be produced
B water and salt to be produced D no reaction to occur

12. In the presence of an acid you would expect __________.

A red litmus paper to turn blue C blue litmus paper to have no change
B blue litmus paper to turns red D red litmus paper to turn green
13. Based on the characteristic of taste alone, which of the following foods would you assume to be most
acidic?

A milk        B soda        C banana peel        D lemon
14. Which of the following is an observable property of an acid?

A changes red litmus paper blue

B reacts with compounds containing hydrogen to form water and salt
C tastes bitter

D reacts with zinc metals to form hydrogen gas

15. Which of the following is an observable property of a base?

A They have a sour taste.

B They feel slippery.

C They react with metal hydroxides forming salt and water.

D They react with zinc metals forming hydrogen gas.
16. Which of the following is formed when a base containing hydroxide ions reacts with an acid?

A hydrochloric acid       B hydrogen ions         C water and salt       D sulfuric acid
17. An aqueous solution of a base will cause an indicator to __________.

A break        B change color         C dissolve        D change direction
18. Which of the following is a familiar property of a base?

A slippery texture         B sour taste    C sweet taste          D rough texture

19. One observable property of a base is that it tastes __________.

A bitter          B sour      C salty      D sweet
20. An observable property of a basic solution would be a change in the color of litmus paper from red to
__________.

A pink       B blue        C white         D green
21. What are the chemical dyes in acids called that change color?

A designators         B alteration    C metamorphic ions         D indicators
22. Metals like zinc and magnesium will react with aqueous solutions of acids to produce __________.

A helium gas          B hydrogen gas       C hydroxide gas       D water vapor
23. All of the following are observable properties of bases EXCEPT __________.

A that bases taste bitter

B that bases conduct electricity when in solution

C that bases turn litmus paper from blue to red

D that bases react with acids to form salts and water

24. All of the following are observable properties of acids EXCEPT __________.

A that they conduct electricity when in solution

B that they taste sour

C that they turn litmus paper from red to blue

D they react with bases to form salts and water

25. Which of these BEST describes the way most bases feel?

A slimy         B gritty       C hot        D cold

26. Which of these BEST describes the taste of most acids?

A bitter      B sweet        C sour      D tasteless
27. According to the Brønsted-Lowry acid-base definition, what occurs if the base NH3 is added to water?

A The water molecules donate hydroxide ions to the NH3.

B The water molecules gain hydrogen ions from the NH3.

C The NH3 molecules donate hydroxide ions to the water.

D The NH3 molecules gain hydrogen ions from the water.
NH3 + H2O → NH4+ + OH-

28. The equation above describes an acid–base reaction. Which of the reactants serves as an acid according
to the Bronsted–Lowry acid–base definition?

A NH3 C OH–
B H2O D NH4+
29. In the equation: HBr(aq) + NH3(aq) → NH4 + (aq) + Br–(aq), the HBr serves as an acid because it is

A a hydrogen ion donor. C a hydroxide ion donor.
B a hydrogen ion acceptor. D a hydroxide ion acceptor.
30. Which of the following is a hydrogen ion donor?

A a strong acid       B a weak base       C a strong base     D both A and C
31. Which of the following are hydrogen–ion donating substances?

A acids only       B bases only          C both acids and bases     D salts
32. Which of the following, if any, are hydrogen–ion accepting substances?

A acids only C both acids and bases
B bases only D neither acids nor bases
33. Which of the following statements concerning the behavior of acids and bases is true?

A Acids and bases are both hydrogen–ion donating substances.

B Acids are hydrogen–ion donating and bases are hydrogen–ion accepting substances.

C Acids and bases are both hydrogen–ion accepting substances.

D Acids are hydrogen–ion accepting and bases are hydrogen–ion donating substances.

34. Adding a base to an acidic solution REDUCES the solution's concentration of which of the following?

A H+ ions

B OH- ions

C CO molecules

D CO2 molecules
35. A powder is added to water, forming an acidic solution. The concentration of which of the following
increased when the powder dissolved?

A H2 molecules C OH- ions
B H+ ions        D O3 molecules
36. In the balanced equation shown below, phosphoric acid reacts with lithium hydroxide to produce lithium
phosphate and water.




Which of the following statements accurately describes what happens in this reaction?

A Li3PO4 accepts hydrogen ions.

B LiOH accepts hydroxide ions.

C Li3PO4 donates hydroxide ions.

D H3PO4 donates hydrogen ions.
37. According to the Bronsted-Lowry acid-base definition, in a solution, hydrochloric acid will

A accept chloride ions.

B accept hydrogen ions.

C donate hydrogen ions.

D donate hydroxide ions.
38. Which is the acid in the chemical equation below?

HA + B- → A- + HB

A HA          B B-            C A-     D HB

39. Acetic acid is classified as a weak acid rather than a strong acid. Which property of acetic acid indicates
that it is a weak acid in an aqueous solution?

A It forms an excess of hydronium ions.

B It rapidly escapes into the gas phase.

C It partially dissociates.

D It reacts to form a new compound.
40. An electrolyte is a substance that dissolves in water to produce free ions. Which of the following would
make good electrolytes?

A strong acids         B weak acids        C strong bases       D Both A and C
41. Hydrogen fluoride is classified as a weak acid rather than a strong acid. Which property of hydrogen
fluoride causes it to be a weak acid in an aqueous solution?

A It rapidly escapes into the gas phase.

B It shows little dissociation.

C It forms an excess of hydronium ions.

D It reacts when forming a new compound.
42. Sodium hydroxide (NaOH) is classified as a strong base. For every mole of sodium hydroxide added to a
large volume of water, one mole of which of the following enters solution?

A H+ ions C H3O+ ions
B OH- ions D H2O2
43. A solution is prepared that contains one mole of nitrous acid (a weak acid) and one mole of sodium
hydroxide (a strong base). Which of the following statements regarding this solution is true?

A The sodium hydroxide will partially dissociate to form hydrogen ions.

B The nitrous acid will completely dissociate to form hydrogen ions.

C The sodium hydroxide will completely dissociate to form hydroxide ions.

D The nitrous acid will partially dissociate to form hydroxide ions.
44. Vinegar typically consists of a 5% acetic acid                            solution. The acetic acid in
vinegar is classified as a weak acid because

A it has a pH close to 7.                   C its concentration is low.
B it only partially dissociates.            D it is safer than most acids.
45. In regards to acids and bases, strong and weak refer to extent of __________.

A dissociation           B deletion           C retention          D dismantle
46. If less than 1% of ethanoic acid is ionized in an instant, ethanoic acid is
considered a __________ acid.

A strong           B hydrochloric            C sulfuric                                   D   weak
47. Acids and bases that are weak __________ in water.

A will fully dissociate                  C    will not dissociate
B will partially dissociate              D are classified as hydrochloric
48. What criteria is used in order to classify acids as strong or weak?

A      how they dissociate in water

B      how fast they dissolve material

C      the amount of sulfur present

D     the time it takes for sulfur ions to bond
49. A strong acid will __________ into ions when placed in water.

    not                      partially                   completely                    sometimes
A                        B                           C                             D
    dissolve                 dissolve                    dissolve                      dissolve




50. The data in this graph BEST support which statement about the pH of the substances?

A Sea water is a base.

B Milk is a strong acid.

C Ammonia is a neutral substance.

D Vinegar is a strong base.
51. The pH of blood is between 7.35 and 7.45, which means that it is __________.

A acidic       B neutral          C slightly basic       D slightly acidic
52. A scientist measures the pH of four solutions. Which pH level is the most acidic?

A 7         B 6        C 5       D 10

53. Which of the following lists pH values from least to most acidic?

A 0, 4, 5         B 8, 10, 12     C 12, 6, 3       D 0, 7, 14




54. In the table above, which pH value correctly matches the solution type?

A A

B B

C C

D All of the pH values correctly match the solution type.
55. A solution of ammonium hydroxide (NH4OH) has a pH of 10. The solution is __________.

A an acid         B a base      C a salt        D neutral

56. A solution of sodium hydroxide (NaOH) has a pH of 13. The solution is __________.

A a weak acid         B a strong base      C a weak base         D a salt

57. The pH of a base solution is __________.

A greater than or equal to 7 C less than 7
B equal to 7                 D greater than 7
58. The pH of an acid solution is __________.

A less than or equal to 7

B from 1 to 7

C less than 7

D greater than 7
59. A weak basic solution is most likely to have which pH?

A 14

B -1

C 0

D 8
60. Which of the following pH values is the most acidic?

A pH = -0.1

B pH = 0.0

C pH = 2.0

D pH = 4.0
61. Place the following solutions in order of increasing acidity.

Solution A has a pH of 11
Solution B has a pH of 4
Solution C has a pH of 9

A A, B, C         B B, C, A          C A, C, B       D B, A, C

62. The pH of pure water is approximately __________.

A –14        B 7        C 0       D 14
63. A gas tank holds a homogeneous mixture of 0.1 mol neon, 0.2 mol helium, 0.2 mol oxygen and 0.8 mol
Argon. Which of these gases is the solvent in this mixture?

A Neon, because it has the lowest concentration.

B Argon, because it has the highest concentration.

C Oxygen, because it is the most reactive.

D Helium, because it has the lowest mass percent.
64. Isopropyl alcohol, C3H7OH, is fully miscible in water, H2O. When mixed with water, isopropyl alcohol
__________.

A is never the solvent

B is never the solute

C is neither the solute or solvent

D may be either the solute or solvent
65. Which of the following is an example of a solid solute in a liquid solvent?

A air        B antifreeze         C salt water       D soda pop

66. A solvent is _________.

A a homogeneous mixture                            C the substance in which the solute is dissolved
B a polar substance in which a solute is dissolved D a liquid in which a substance can be dissolved
67. Water samples containing dissolved substances are aqueous

A solvents.        B solutions.        C solutes.       D hydrates.
68. A solute is __________.

A dissolved to form the solution C a homogeneous mixture
B always a solid                 D what the particles are dissolve in
69. Carbonated water is an example of which type of solute–solvent combination?

A gas in a liquid      B liquid in a gas    C solid in a liquid   D None of the above
70. A solution is known as a homogeneous mixture because __________.

A the solute fully dissolves in the solvent

B the solvent fully dissolves in the solute

C the solvent is always water

D the solvent particles are uniformly dissolved in the mixture

71. A student stirs 5 grams of powder into 1 liter of water. The powder separates so that each molecule that
originally formed the powder is surrounded by water molecules. The powder can be classified as which of the
following?

A a solute

B an ion

C a buffer

D a reagent
72. A solution is prepared by adding 5.0 g NaNO3 and 10.0 g CaCl2 to 25.0 g of H2O. Which of the following
correctly identifies the solute(s) and solvent(s) used in this mixture?

A NaNO3 and CaCl2 are solutes; H2O is the solvent

B NaNO3 and CaCl2 are solvents; H2O is the solute

C NaNO3 is the solute; CaCl2 and H2O are the solvents

D NaNO3 is the solvent; CaCl2 and H2O are the solutes
73. A solution is formed by mixing two liquids. We have 20 mL of Substance A and 100 mL of Substance B. It
appears that Substance A dissolved into substance B. From this observation, we know that Substance A is
definitely __________.

A an electrolyte        B a nonelectrolyte        C the solute        D the solvent

74. When you place a small amount of salt into a large bucket of water, the saltis __________.

A melted          B the solvent        C the solute      D the solution
75. A solid is placed in a liquid. A greater amount of the solid will dissolve if there is a strong attraction
between

A the molecules of the liquid.

B the molecules of the solid.

C the molecules of the solid and liquid.

D the atoms in the molecules of the solid.

				
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