Chapter 16 (sections 1-3) Flashcards

1
Q

Define buffer

A

A solution containing significant amounts of both a weak acid and its conjugate base (or a weak base and its conjugate acid) that resists pH change by neutralizing added acid or added base

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2
Q

A buffer resists pH change by _____ added acid or base.

A

neutralizing

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3
Q

A buffer contains significant amounts of …?

A

both a weak acid AND its conjugate base (or a weak base and its conjugate acid)

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4
Q

Buffers ____ pH change.

A

resist

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5
Q

A____ contains significant amounts of both a weak acid and its conjugate base

A

buffer

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6
Q

In a buffer the weak acid ____ added base until the concentration of the base…?

A

neutralizes

exceeds the concentration of the weak acid

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7
Q

In a buffer, the conjugate base ____ the added acid until the concentration of the acid …?

A

neutralizes

exceeds the concentration of the conjugate base

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8
Q

Define common ion affect

A

The tendency for a common ion to decrease the solubility of an ionic compound or to decrease the ionization of a weak acid or weak base

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9
Q

Using the approximation that x is small we can consider the equilibrium concentrationd of HA and A- to be essentially …?

A

identical to the initial concentrations of HA and A-

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10
Q

To determine the concentration of [H₃0⁺] for any buffer solution, we…?

A

multiply Ka by the ratio of the concentrations of the acid and the conjugate base
[H₃0⁺] = Ka [HA]/[A⁻]

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11
Q

In a buffer solution where the concentrations of the acid and conjugate base are equal what is [H₃0⁺] equal to?

A

Ka

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12
Q

When calculating the pH of a buffer, adding a small amount of strong acid to a buffer converts the stoichiometric amount of the _____ to the _____ ____

A

base

conjugate acid

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13
Q

When calculating the pH of a buffer, adding a small amount of strong base to a buffer converts the stoichiometric amount of the _____ to the _____ ____

A

acid

conjugate base

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14
Q

Define buffering action

A

The way a buffer solution reacts with small amounts of acid or base to maintain a fairly constant pH

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15
Q

pKa + pKb =..?

A

14

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16
Q

When is a buffer most effective?

A

When the concentrations of the acid and conjugate base are equal

17
Q

A buffer becomes less effective as the difference in relative amounts of acid and conjugate base ______.

18
Q

In order for a buffer to be reasonably effective, the relative concentrations of acid and conjugate base should not differ by more than a factor of _____.

19
Q

A buffer is most effective (most resistant to pH changes) when the concentrations of acid and conjugate base are ____.

20
Q

Lowest pH for effective buffers occurs when the base is one-tenth as concentrated as the acid. What is this in equation format?

A

pH = pKa -1

21
Q

Highest pH for effective buffer occurs when the base is 10 times as concentrated as the acid. What is this in equation format?

A

pH = pKa + 1

22
Q

The effective range for a buffering system is…?

A

one pH unit on either side of the pKa

23
Q

Define buffer capacity

A

the amount of acid or base that can be added to a buffer without destroying its effectiveness

24
Q

The buffer capacity increases with ____ absolute concentrations of the buffer components

A

increasing

25
Overall buffer capacity increases as the relative concentrations of the buffer components become...?
more similar to each other
26
As the ratio of the buffer components gets closer to one, the overall capacity of the buffer becomes _____.
greater