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ccp 3.1 > MIDTERM - Acids, Bases, pH, and Equilibria in Acid-Base Solutions > Flashcards

MIDTERM - Acids, Bases, pH, and Equilibria in Acid-Base Solutions Flashcards

1
Q

stands for power/potential of hydrogen

quantitative measure of the acidity and alkalinity of liquid solutions.

It is measured on a scale of 0 to 14.

A

pH

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2
Q

Low pH corresponds to ____ concentrations of 𝑯+ and high pH values correspond to ___ concentration of 𝑯+.

A

high
low

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3
Q

It is also directly related to the ratio of 𝑯+ and π‘Άπ‘―βˆ’ in solutions.

A

pH

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4
Q

increasing acidity

A

pH<7

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5
Q

increasing basicity

A

pH>7

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6
Q

acidity is inversely related to ____

the higher the H+ ion concentration, the ___ the pH

A

pH

lower

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7
Q

The pH of the human body ranges between ____ to ____, with the average at 7.40, in the absence of pathological
states.

A

7.35 - 7.45

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8
Q

caused by an overproduction
of acid that builds up in the blood or
excessive loss of bicarbonate from the
blood (metabolic acidosis) or by a buildup
of carbon dioxide in the blood the results
from poor lung function or depressed
breathing (respiratory acidosis).

A

Acidosis

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9
Q

condition in which the
body fluids have excess base (alkali).
This is opposite of excess acid
(acidosis).

Decreased carbon dioxide
(an acid) level) or increased
bicarbonate (a base) makes the body
too alkaline.

A

Alkalosis

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10
Q

an increase in the hydrogen ion concentration of the blood, resulting in a decrease in pH.

A

Acidemia

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11
Q

a decrease in the hydrogen ion concentration in the blood, resulting in an increase in pH.

A

Alkalemia

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12
Q

The pH level can be measured by using:

A

a. pH strips/paper
b. pH indicators
c. pH meter

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13
Q

2 Methods of pH Determination:

A

a. Electrometric Method
b. Colorimetric method

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14
Q

based on the property of acid-base indicator dyes, which produce color depending on the pH of the sample.

The color change can be measured as an absorbance change spectrophotometrically.

A

Colorimetric Method

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15
Q

a chemical added in a small amount to a solution that causes a color change depending on the pH.

An indicator doesn’t shift color at a precise pH or hydrogen ion concentration. Instead, the color change occurs over a range of hydrogen ion concentration.

A

pH indicator or acid-base indicator

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16
Q

Titrate a WEAK ACID using an indicator that changes under SLIGHTLY ALKALINE solutions.

A

Titrate a WEAK BASE using an indicator that changes color at a SLIGHTLY ACIDIC pH.

When titrating strong acids or bases, aim for a pH indicator that displays color change near a neutral pH.

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17
Q

method used to determine the pH level of a sample using ion-sensitive electrodes.

A

Electrometric Method

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18
Q

a laboratory equipment being used to measure the acidity or alkalinity of a solution. It measures the concentration of hydrogen ions using an ion sensitive electrodes.

It is the most reliable and convenient method for measuring pH.

A

pH meter

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19
Q

a species that produces 𝑯+ ions in water
solution.

A

Arrhenius acid

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20
Q

a species that produces π‘Άπ‘―βˆ’ ions in water
solution.

A

Arrhenius base

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21
Q

a species that accepts an electron pair.

A

lewis acid

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22
Q

species that donates an electron pair.

A

lewis base

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23
Q

proton (𝑯+π’Šπ’π’) donor

A

bronsted-lowry acid

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24
Q

a proton (𝑯+π’Šπ’π’) acceptor

A

bronsted-lowry base

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25
Q

The species formed when a proton is removed from an acid is referred to as the __________ of that acid.

A

conjugate base

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26
Q

The species formed when a proton is added to a base is called the ________ of that base.

A

conjugate acid

27
Q

LEWIS:

acid =
base =

A

electron-pair acceptor
electron-pair donor

28
Q

BRONSTED-LOWRY

acid =
base =

A

H+ donor
H+ acceptor

29
Q

ARRHENIUS

acid =
base =

A

H+ donor
OH- donor

30
Q

Strong and weak acids differ in the extent of their ______ in water.

A

ionization

31
Q

Strong acids ionize _______, forming 𝑯+ ions and anions.

A

completely

32
Q

Weak acids are _____ ionized to 𝑯+ ions in water.

A

partially

33
Q

The acidic and basic properties of aqueous solutions are dependent on the

A

equilibrium that involves the water, solvent.

34
Q

pH increases by 1 unit when the concentration of 𝐻+ decreases by a power of 10!

A
35
Q

WEAK ACIDS (BRONSTED-LOWRY REACTION)

Most weak acids fall into one of two categories:

A
  1. Molecules containing an ionizable H atom.
  2. Cations.
36
Q

Thousands of molecular weak acids (most of them are organic in nature).

Among the molecular inorganic weak acids is nitrous acid:

A
  1. Molecules containing an ionizable H atom
37
Q

The ammonium ion behaves as a weak acid in water; a 0.10 M solution of 𝑁𝐻4𝐢𝑙 has a pH of about 5.

The process by which the 𝑁𝐻4+ ion lowers the pH of water can be represented by the equation:

A
  1. Cations
38
Q

Many metal cations act as weak acids in water solutions.

A
39
Q

The weaker the acid, the smaller the value of πΎπ‘Ž.

A

The weaker the acid, the higher the value of π‘πΎπ‘Ž.

40
Q

The π‘πΎπ‘Ž value is used to indicate the

A

strength of an acid.

41
Q

depends on the concentration of weak acid, increasing as the acid is diluted

A

Percent Ionization

42
Q

[𝐻+]

A

concentration ionized or equilibrium concentration of hydrogen ion

43
Q

[𝐻A]

A

original concentration or concentration of weak acid

44
Q

Certain weak acids are _________

they contain more than one ionizable
hydrogen atom.

The acid equilibrium constant becomes smaller with each successive step.

A

polyprotic

45
Q

WEAK BASES (Bronsted-Lowry Reaction)

Most weak bases fall into one of two categories:

A
  1. Molecules (most are organic compounds, amines).
  2. Anions (An anion derived from a weak acid is itself a weak base.)
46
Q

Kb =

A

base equilibrium constant

47
Q

[π΅βˆ’] =

A

molar concentration of weak base

48
Q

[𝐻𝐡] =

A

molar concentration of conjugate acid

49
Q

The weaker the base, the smaller the
value of 𝐾b

A

The weaker the base, the higher the value of 𝑝𝐾𝑏.

50
Q

The π‘πΎπ‘Ž value is used to indicate the

A

strength of a base.

51
Q

The larger the value of 𝐊𝐚, the _____ the value of πŠπ› and vice versa.

A

smaller

52
Q

From the general relation between πΎπ‘Ž of a weak acid and 𝐾𝑏 of its conjugate weak base, these two quantities are _______ related to each other.

A

inversely

53
Q

Any solution containing appreciable amounts of both a weak acid and its conjugate base is highly resistant to changes in pH brought about by addition of strong acid or strong base.

has a pH close to the 𝒑𝑲𝒂 of the weak acid.

A

BUFFERS

54
Q

Choosing A Buffer System

The pH of the buffer depends on two factors:

A
  1. The acid equilibrium constant of the weak acid, 𝑲𝒂.
  2. The ratio of the concentrations or amounts of 𝑯𝑨 and π‘¨βˆ’
55
Q

Effect of Added 𝑯+or π‘Άπ‘―βˆ’on Buffer Systems:

The pH of a buffer does change slightly on addition of moderate amounts of a strong acid or strong base.

A

Addition of 𝐻+ ions converts an equal amount of a weak baseπ΅βˆ’ to its conjugate acid HB:

56
Q

By the same token, addition of π‘‚π»βˆ’ ions converts an equal amount of weak acid to its conjugate base π΄βˆ’

A
57
Q

A buffer has a limited capacity to react with 𝐻+ or π‘‚π»βˆ’ ions without undergoing a drastic change in pH.

A
58
Q

the capacity of a buffer to absorb added π‘‚π»βˆ’ or 𝐻+ ions is _______ related to the slope of the curve.

A

inversely

59
Q

the pH range over which the buffer is effective.

It is related to the ratio of concentrations of the weak acid and its conjugate.

A

buffer range

60
Q

An acid-base indicator is useful in determining the ____________ of an acid-base titration.

This is the point in which reaction is complete; equivalent quantities of acid and base have reacted.

A

equivalence point

61
Q

If the indicator is chosen properly, the point at which it changes color (its end point) CONINCIDES with the equivalence point.

A

To understand how and why an indicator changes color, we need to understand the equilibrium principle involved.

62
Q

The color that you see when a drop of indicator solution is added in
an acid-base titration depends on the

A

ratio

63
Q

Strong acids ionize completely in water to form _____ ions

strong bases dissolve in water to form
____ ions.

A

H3O+

OH-

64
Q
A

ccp 3.1 (4 decks)

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