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Chemistry > Unit 10 > Flashcards

Unit 10 Flashcards

1
Q

What are properties of acids?

A
  1. excess of hydrogen ions, H+
  2. pH below 7
  3. sour taste
  4. corrosive and poisonous
  5. react with active metals (activity series)
  6. neutralize bases
  7. turns blue litmus paper red
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2
Q

What are properties of bases?

A
  1. excess of hydroxide ions, OH-
  2. pH above 7
  3. bitter taste
  4. caustic (burns the skin)
  5. slippery
  6. neutralize acids
  7. turns red litmus paper blue
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3
Q

What are some examples of strong acids?

A
  1. HCl (hydrochloric/stomach acid)
  2. H₂SO₄ (sulfuric/car battery acid)
  3. Hl (hydroiodic acid)
  4. HNO₃ (nitric acid-used to make bombs/munitions)
  5. HClO₄ (perchloric acid)
  6. HBr (hydrobromic acid)
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4
Q

What are some examples of weak acids?

A
  1. Citric Acid (citrus fruits)
  2. Ascorbic Acid (Vitamin C)
  3. Acetic Acid (HC₂H₃O₂-Vinegar)
  4. Formic Acid (ant/bee stings)
  5. Acetylsalicylic Acid (aspirin)
  6. Carbonic Acid (H₂CO₃-all carbonated beverages)
  7. Tartaric Acid (grapes)
  8. Deoxyribonucleic Acid (DNA)
  9. Lactic Acid (milk/sore muscles)
  10. Phosphoric Acid (H₃PO₄-dark-colored carbonated drinks)
  11. Tannic Acid (tea)
  12. Malic Acid (apples)
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5
Q

Strong acids will ________ _______ in water. Weak acids do not.

A

completely ionize

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6
Q

What are some acids commonly used in industry?

A
  1. HCl: used to “pickle”/cure steel
  2. HNO₃: explosives
  3. H₂SO₄: car batteries
  4. HClO₄: cure steel
  5. H₃PO₄: fertilizers
  6. HC₂H₃O₂: make plastics/tape (vinegar)
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7
Q

acids that contain oxygen, such as sulfuric acid

A

Oxyacid

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8
Q

acids that contain a hydrogen and one other element, such as HCl

A

Binary Acids

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9
Q

What are some examples of strong bases?

A

(✩Made from some of the metals of Groups I and II)

  1. NaOH (“lye” used in drain cleaners/unclog drains)
  2. KOH
  3. LiOH
  4. Ca(OH)₂ (used to remove hair from cow hide before tanning)
  5. RbOH
  6. CsOH
  7. Sr(OH)₂
  8. Ba(OH)₂
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10
Q

What are some examples of weak bases?

A
  1. Mg(OH)₂: magnesium hydroxide (laxative)
  2. NaClO: sodium hypochlorite (bleach)
  3. NH₃: ammonia (glass cleaner/fertilizer)
  4. CaO: Lime (a fertilizer; also used to create “limelight” when burned at night)
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11
Q

According to Svante Arrhenius, acids are substances that, when placed in water, __________________________________. Bases produce an excess of ____________________.

A

the amount of hydrogen ions increases; hydroxide ions (increase the hydroxide concentration)

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12
Q

According to the Lewis theory of acids and bases, a Lewis Acid is a species that will ______ a lone pair of electrons. Lewis bases will ______ a lone pair of electrons.

A

accept, donate

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13
Q

Strong acids will ionized completely to produce the _________ ion when mixed with water.

A

hydronium

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14
Q

The Bronsted-Lowry theory of acids and bases says that acids are ______ ______ and bases are ______ _________.

A

proton (H+) donors, proton (H+) acceptors

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15
Q

Water can be classified as both an ____ or a ____ under the Bronsted-Lowry theory. This is termed ___________ or ___________.

A

acid or a base, Amphoteric or Amphoprotic

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16
Q

acids that have ONE ______ that they are capable of losing during ionization.

A

Monoprotic Acids

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17
Q

acids that have TWO or MORE _______ that they can lose at a time. (ex. sulfuric acid)

A

Polyprotic Acids

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18
Q

formed from the gain of a proton

A

Conjugate Acids

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19
Q

formed from the loss of a proton

A

Conjugate Bases

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20
Q

the process which occurs when an acid is added to a base. It produces a salt and water.

A

Neutralization

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21
Q

A salt forms from the ________ ___ of a base and the ________ ___ of an acid

A

positive ion, negative ion

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22
Q

What is an example of a basic salt with a pH above 7?

A

Sodium Bicarbonate/Baking soda

23
Q

strong acid + strong base =

A

neutral salt

24
Q

strong acid + weak base =

A

acidic salt

25
Q

weak acid + strong base =

A

basic salt

26
Q

pH is a measure of the ______________________________.

A

negative log of hydrogen ion concentration

27
Q

pH scale is from _ to __.

A

0 to 14

28
Q

_ is a very strong acid, __ is a very strong base, and _ is neutral.

A

0, 14, and 7

29
Q

pOH is the measure of the ___________ concentration in a substance. 14= pH + pOH

A

Hydroxide

30
Q

a process in which a measured amount of a solution of _______ concentration is added to a quantity of a solution of ___________ concentration. The point at which the solution is neutralized is the endpoint. the endpoint is signaled by a change in the ______ of the liquid indication that has been added to it.

A

Titration, known, unknown, color

31
Q

a substance which changes color in a certain pH range

A

Indicator

32
Q

Indicator that was used in lab that is colorless in acid, baby pink at the end point (or equivalence point), and magenta when the pH is around 10.

A

Phenolphthalein

33
Q

The _______ ______ allows you to calculate the concentration of the unknown.

A

titration formula

34
Q

Oxidation is the ____ of valence electrons. Most ______ undergo oxidation. Iron will ____, silver will _______.

A

loss, metals, rust, tarnish

35
Q

Since electrons are negative, the element becomes __________ charged when losing valence electrons.

A

positively

36
Q

Reduction is the ____ of valence electrons. Most _________ will undergo reduction.

A

gain, nonmetals

37
Q

If you have _ or less valence electrons, the element will usually undergo oxidation. _ to _ valence electrons will usually undergo reduction.

A

3, 5 to 7

38
Q

If you have oxidation, you must have ________.

A

reduction

39
Q

Oxidation is ____.

A

loss

40
Q

Reduction is ____.

A

gain

41
Q

a device in which a chemical reaction either produces or is carried out by an electric current.

A

Electrochemical Cell

42
Q

an electrochemical cell that uses electrical current to drive an otherwise non spontaneous reaction

A

Electrolytic Cell

43
Q

a gel or piece of paper soaked in a salt like potassium chloride is an example of a ____ ______. This allows ions to be exchanged but does not allow the two solutions to ___.

A

salt bridge, mix

44
Q

In an electrochemical cell, such as a battery, reduction occurs at the _______ and oxidation occurs at the _____.

A

cathode, anode

45
Q

If a Redox reaction occurs spontaneously and produces an electrical current, it is called _______ or ________.

A

Voltaic or Galvanic

46
Q

the amount of energy you can get from a battery (maximum) is stated in _____, (unit of electricity named after __________ _____ who developed the first but crude battery).

A

volts, Alessandro Volta

47
Q

found in a lot of batteries but don’t do well in COLD weather

A

Zn-C dry cell

48
Q

uses a paste of potassium hydroxide in addition to the items mentioned in the Zn-C cell. Performs better in cold weather.

A

Alkaline Battery

49
Q

Ni-Cd battery is ____________.

A

rechargeable

50
Q

battery used in pacemakers because of their low voltage and their ability to last up to 10 years (rechargeable, ex. cell phones)

A

Lithium-iodine

51
Q

car battery

A

Lead Storage Battery

52
Q

liquid hydrogen and oxygen used in spacecraft

A

fuel cell

53
Q

nonspontaneous reactions are called ____________ cells. These cells require a current for them to work. (Ex.: electroplating metals)

A

electrolytic

Chemistry (13 decks)

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