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Chemistry Module 1 > Acid - Base equilibria > Flashcards

Acid - Base equilibria Flashcards

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1
Q

What is a bronsted acid

A

Proton donor

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2
Q

What is a bronsted base

A

Proton acceptor

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3
Q

For the reaction NH3 + H2O ⇌ NH4+ + OH- , what are the conjugate acid base pairs?

A
  1. NH3 accepts a proton to become NH4+, NH3 acts as a brØnsted Lowry base
  2. H2O donates a proton, thus acting as a brØnsted Lowry acid
  3. NH3 and NH4+ are a conjugate acid base pair
  4. H2O and OH- are a conjugate acid base pair
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4
Q

What is a strong acid

A

Fully dissociates in solution, can be mono, di or tribasic

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5
Q

What is mono/di basic

A

monobasic - donates 1 proton per molecule of acid

di - donates 2 protons per molecule of acid

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6
Q

What is a weak acid ?

A

Partially dissociates in solution

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7
Q

What is the formula for pH?

A

pH = -log[H+]

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8
Q

What does [H+] equal

A

[H+] = antilog(-pH)

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9
Q

Draw out the table for converting between [acid] [H+] and pH

A

on page

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10
Q

What is the ionic product of water?

A

Kw = [H+][OH-]
units of mol^2dm^-6
At 25ºC , Kw = 1 x10 -14

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11
Q

What is Kw in pure water?

A

in pure water [H+] = [OH-] therefore Kw = [H+]^2

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12
Q

What is the table for converting between pH of strong alkalis

A

on page

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13
Q

What are the equations for pKw, pOH,

A

pKw = -log Kw pKw = 14.00 at 25ºC
pOH = -log[OH-]
pH + pOH = pKw

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14
Q

What is the general acid dissociation for a weak acid?

A

HA ⇌ H+ + A-

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15
Q

What is Ka

A

Ka = [H+][A-]
————-
[HA]
Always has units of moldm^-3

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16
Q

What does a higher Ka suggest

A

A higher Ka suggests a ‘stronger’ weak acid

17
Q

What is the table for converting between a weak acid and pH?

A

on page

18
Q

What happens when an acid or alkali is neutralised or diluted?

A

The concentration of the ions in solution changes

19
Q

What is the formula for working out concentration of a diluted solution?

A

on page

20
Q

What is the formula for working out The neutralisation

A

on page

21
Q

What is a buffer?

A

A solution that resists small changes in pH on addition of small amounts of acid or alkali

22
Q

What is the buffering action represented by?

A

HA ⇌ H+ + A-

23
Q

What is the buffering action when extra acid is added

A
  1. Extra Hydrogen ions are added
  2. The anion in the buffer reacts with the H+
    ( H+ + A- →HA )
  3. The extra H+ ions are removed
  4. This maintains [H+] and maintains pH
24
Q

What happens on the addition of alkali

A
  1. Extra hydroxide ions are added
  2. These react with the undissociated acid in the buffer solution (HA + OH- → A- + H2O)
  3. Extra OH- ions are removed
  4. This maintains [H+] and maintains pH
25
Q

What is the henderson-Hasselbalch equation?

A

on page

26
Q

Draw out the four different titration curves, state what the reaction is between and suggest a suitable indicator.

A

in book

27
Q

What is the pH range for phenolphthalein and what titrations is it suitable for?

A

8.3 to 10.0
Strong - Strong
Weak - Strong

28
Q

What is the pH range for methyl orange and what titrations is it suitable for?

A

3.1 - 4.4
Strong - Strong
Strong - Weak

29
Q

What is the pH range for methyl red and what titrations is it suitable for?

A

4.4 - 6.2
Strong - Strong
Strong - Weak

30
Q

What is salt hydrolysis?

A

When all or some of the H+ ions in an acid are replaced with positive ions

31
Q

What are the four things that salts can be made from and what is the solution (acidic or alkaline)

A
  1. Strong acid - Strong base e.g. NaCl and solution is neutral
  2. Strong acid - Weak base e.g. NH4NO3, solution is acidic
  3. Weak acid - Strong base e.g. CH3COONa, solution is alkaline
  4. Weak acid - Weak base e.g. CH3COONH4, either acidic or alkaline
32
Q

For the previous question, for 1, 2 and 3 what happens in water.

A
  1. Neither of the ions from the salt react with water
  2. The positive ion react with water donating a H+ to form the acidic hydronium ion
  3. The negative ion reacts with water, the water donates a H+ leaving OH- ions in solution

Chemistry Module 1 (10 decks)

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