5.1.3 - Acids, Bases & pH. Flashcards

1
Q

What is a Brønsted-Lowry Acid?

A

A proton donor.

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2
Q

What is a Brønsted-Lowry Base?

A

A proton acceptor.

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3
Q

How are conjugate acid-base pairs related?

A

The conjugate acid donates a proton (H+) to make the conjugate base; the base accepts the proton (H+) to make the acid.

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4
Q

What is the Conjugate Base of these below?
* HNO3.
* H20.
* H2SO4.
* HCl.

A
  • NO3-.
  • OH-.
  • HSO4-.
  • Cl-.
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5
Q

What is the Conjugate Acid of these below?
* OH-.
* H20.
* SO42-.
* Br-.

A
  • H20.
  • H3O+.
  • HSO4-.
  • HBr.
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6
Q

Explain what each of the below are and give 1 example of each.
1. Monobasic Acid.
2. Dibasic Acid.
3. Tribasic Acid.

A
  1. An acid which only has 1 H+ ion to donate to its conjugate base (HCl).
  2. An acid which only has 2 H+ ions to donate to its conjugate base (H2SO4).
  3. An acid which only has 3 H+ ions to donate to its conjugate base (H3PO4).
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7
Q

What is the DEFINITION of a Weak Acid? Give a general equation for this?

A
  • A weak acid only partially dissociates it’s H+ ions in aqueous solution.
  • [HA] ⇌ [H+] + [A-] which leads to [H+] ∼ [A-].
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8
Q

What is the DEFINITION of a Strong Acid?

A
  • A strong acid fully dissociates all of it’s H+ ions in aqueous solution.
  • [HA] ∼ [H+].
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9
Q

Write the Ka expression for a general weak acid HA.

A

Ka = [H+][A-]/ [HA].

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10
Q

Which equation gives pH from [H+]?

A

pH = -log[H+].

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11
Q

Which equation gives pKa from Ka?

A

pKa = -log(Ka).

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12
Q

Which equation gives [H+] from pH?

A

[H+] = 10-pH.

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13
Q

What simplified Ka expression can we use for weak acids?

A

Ka = [H+]2/ [HA].

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14
Q

How does the simplified Ka expression Ka = [H+]2/ [HA] rearrange to solve for [H+]?

A

[H+] = √(Ka x [HA]).

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15
Q

What is the expression for the ionic product of water?

A

Kw = [H+][OH-].

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16
Q

What is the value of Kw for neutral pH7 at 25°C?

A

1.00 x 10-14 mol2 dm-6.

17
Q

Which equation gives Ka from pKa?

A

Ka = 10-pKa.

18
Q

Does a larger Ka value mean a stronger or weaker acid?

A

Stronger - The acid dissociation equilibrium lies further to the right.

19
Q

Does a larger pKa value mean a stronger or weaker acid?

A

Weaker - Trend follows the reverse of Ka due to -ve sign in -log(Ka).

20
Q

What two approximations are made when calculating pH of weak acids?

A
  • [HA]eqm = [HA]start.
  • [H+] = [A-].
21
Q

When does the approximation that [H+] = [A-] for a weak acid break down?

A

For very dilute or very weak solutions of acid as the H+ from water dissociation is significant compared to the H+ from the acid.

22
Q

What is the Kw expression in pure water?

A

[H+] = [OH-] so Kw = [H+]2, therefore [H+] = √Kw.