Module 3.3 Acids, Bases, and pH Flashcards

1
Q

What are acids and bases?

A

Chemical compounds that have specific properties and a certain number of hydrogen ions (H+) when dissolved in water.

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2
Q

Hydrogen atoms have

A

1 proton and 1 electron

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3
Q

Hydrogen ions have

A

lost its electron. Has only 1 proton.

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4
Q

Hydrogen ions are

A

positively charged

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5
Q

How does dissociation happen?

A

Sometimes one of the polar covalent bonds of water pulls the electrons so far towards the oxygen that the water molecule falls apart or dissociates

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6
Q

The equation for the dissociation of water is: ​

A

H2O → OH- + H+ ​

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7
Q

Rarely during dissociation, H+ is

A

quickly picked up by a passing water molecule to become H3O+ aka a hydronium ion

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8
Q

When a hydronium ion is made, it results in a

A

a hydroxide ion left (OH-)

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9
Q

What happens during the dissociation of water?

A

Water dissociates into hydroxide ions (OH-) and hydrogen ions (H+).

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10
Q

What is the chemical equation for the dissociation of water?

A

H2O → OH- + H+

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11
Q

What is a hydronium ion?

A

H3O+, formed when H+ is picked up by a passing water molecule.

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12
Q

How often does the hydrogen ion get picked up during dissociation?

A

1 in 1x10^7 molecules of water in neutral water

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13
Q

What is the official chemical name of H+?

A

Hydrogen ion.

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14
Q

How is H+ read

A

H plus

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15
Q

The hydrogen atom has

A

1 proton and 1 electron

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16
Q

When the electron is lost in the hydrogen ion, the only part of the hydrogen atom left is the

A

proton

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17
Q

What defines an acid in biological terms?

A

A molecule that can donate H+.

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18
Q

An acid increases the hydrogen ions in

A

a solution

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19
Q

An acidic solution is a solution that has a

A

high concentration of H+ or hydronium ions

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20
Q

What is the difference between strong acids and weak acids?

A

Strong acids completely dissociate; weak acids do not.

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21
Q

Give examples of strong acids.

A
  • Sulfuric acid
  • Hydrochloric acid
  • Nitric acid
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22
Q

Give examples of weak acids.

A
  • Carbonic acid
  • Citric acid
  • Acetic acid
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23
Q

What defines a base?

A

Atoms or molecules that can accept H+.

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24
Q

What is a characteristic of a basic solution?

A

Low concentration of H+ or high concentration of OH-.

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25
Q

Bases decrease

A

H+ concentrations in a solution

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26
Q

Weak bases do not

A

dissociate completely

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27
Q

Give examples of weak bases.

A
  • Ammonia (NH3)
28
Q

What defines strong bases?

A

They dissociate completely and create OH- ions that can pick up hydrogen ions indirectly.

29
Q

Strong bases dissociate

A

completely

30
Q

Give examples of strong bases.

A
  • Sodium hydroxide
  • Sodium phosphate
  • Sodium carbonate
31
Q

What are some properties of acids?

A
  • Taste sour
  • Are corrosive
  • Conduct electricity
32
Q

Strong acids nearly completely

A

dissociate

33
Q

Weak acids do not do what well?

A

Dissociate

34
Q

What percentage of weak acids dissociate

A

usually only 5%​

35
Q

What is the pH scale?

A

A measure of the acidity or basicity of an aqueous solution.

36
Q

Hydronium is more common in

37
Q

The pH scale goes from

38
Q

pH stands for

A

The Power of Hydrogen or the Power of Hydronium

39
Q

Another way to look at pH is as a measure of

A

the concentration of H+ in an aqueous solution

40
Q

Neutral substances

A

are neither acidic nor basic​ (ex NaCl and distilled water)

41
Q

What is the neutral pH value?

42
Q

The numbers on the scale range from 0 to 14 and reflect

A

the concentration of H+ and OH- in the solution

43
Q

A fluid is assigned a number according to

A

the number of H+ ions present in a liter of that fluid

44
Q

What does a lower pH number indicate?

A

Higher concentration of H+ ions and the LOWER the OH- concentration​.

45
Q

What does a higher pH number indicate?

A

Lower concentration of H+ ions and higher concentration of OH- ions.

46
Q

What is the pH of an acidic solution?

47
Q

What is the pH of a basic or alkaline solution?

48
Q

Low pH is

A

acidic. It has more H+ ions and fewer OH- ions

49
Q

High pH is

A

basic and has more OH- ions and fewer H+ ions

50
Q

The pH scale is a what kind of scale

A

logarithmic scale

51
Q

A logarithmic scale is a base

52
Q

A change of one whole pH number represents

A

a ten-fold (10X) change in the number of H+ ions

53
Q

What happens to proteins if the pH changes too much?

A

They can denature or fall apart.

54
Q

What are buffers?

A

Substances that resist sudden changes to the original pH of a solution.

55
Q

Give an example of a buffer in human blood.

A

Carbonate-bicarbonate buffer.

56
Q

What is the formula for the carbonate-bicarbonate buffer?

A

H2CO3 ↔ HCO3- + H+​

57
Q

Normal pH of blood

58
Q

What do buffers do when pH becomes too acidic?

A

Act like a base and accept H+ ions.

59
Q

What do buffers do when pH becomes too basic?

A

Act like an acid and accept OH- ions.

60
Q

STRONG acids and bases can

A

neutralize each other

61
Q

What is neutralization?

A

A reaction where H+ of an acid combines with OH- of a base to form water.

62
Q

What are salts?

A

Substances that dissociate into cations and anions in water, neither of which are H+ or OH-.

63
Q

How are salts formed?

A

In a neutralization reaction.

64
Q

Strong acids and strong bases react to form

A

water and a salt​. They make neutral products.

65
Q

What are electrolytes?

A

Salts dissolved in water that conduct electricity.

66
Q

Examples of electrolytes

A

Na+​
Cl-​
K+​
Ca2+​
Mg2+

67
Q

What are some functions of electrolytes?

A
  • Maintaining salt/water balance
  • Maintaining acid/base balance
  • Involved with nerve function and parts of bone and teeth