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1.1 Chemistry > pH > Flashcards

pH Flashcards

1
Q

What are electrolytes?

A

Ionic salts

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2
Q

What are electrolytes used for?

A

They conduct electrical impulses within the body

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3
Q

What are acids and bases in relation to electrolytes?

A

They are a special subset of electrolytes

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4
Q

What are the three characteristic properties of acids?

A

Sour taste

Turns litmus red

Eats away active metals by reacting to produce H2

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5
Q

What are the three characteristic properties of bases?

A

Bitter taste

Turns litmus blue

Produces slippery aqueous solutions to the touch

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6
Q

What are indicators?

A

They indicate acids and bases by colour changes

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7
Q

Give some examples of indicators.

A

Litmus

Cabbage juice

Some flowers

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8
Q

What is a neutral sibstance?

A

Something that exhibits neither an acid nor a base behaviour

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9
Q

What do electrolytes do?

A

They conduct electric currents

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10
Q

What do nonelectrolytes do?

A

They do not conduct electric currents

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11
Q

Give some examples of electrolytes.

A

Acetic acid
Hydrogen chloride
Sulfuric acid

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12
Q

Give some examples of nonelectrolytes.

A

Acetone
Carbon dioxide
Ethanol

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13
Q

What are ions?

3

A

Mobile charged particles in solution

Carry currents in electrolyte solutions

Formed by dissociation of ionic salts

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14
Q

What forms ions?

A

The dissociation of ionic salts

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15
Q

What is dissociation?

A

The splitting of ionic compounds to individual charged components

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16
Q

What are acids?

A

Compounds that can give hydrogen ions hence increasing the concentration of hydronium ions

17
Q

What form are protons in in water?

A

Form of hydronium ions

18
Q

What is the Bronsted-Lowry definition of an acid?

A

Any substance that can donate a proton

19
Q

List three strong acids.

A

Sulfuric acid - H2SO4

Nitric acid - HNO3

Hydrochloric acid - HCL

20
Q

List two weak acids.

A

Ethanoic acid - CH3COOH

Carbonic acid - H2CO3

21
Q

What are bases?

2

A

Bases are compounds that can accept hydrogen ions

They produce hydroxide anions (OH-) in water -> they increase the hydroxide ion concentration while decreasing the hydrogen ion concentration

22
Q

What is the Bronsted Lowry definition of a base?

A

Any substance that can accept a proton

23
Q

List three strong bases.

A

Sodium hydroxide - NaOH
Potassium hydroxide - KOH
Lithium hydroxide - LiOH

24
Q

List three weak bases

A

Calcium hydroxide - Ca(OH)
Ammonia - NH3
Carbonate - CO3

25
Q

What happens to both strong acids and bases in water?

2

A

They are essentially 100% ionized in water

They are completely dissociated in aqueous solution

26
Q

What happens to both weak acids and bases in water?

A

They are much less ionized

27
Q

What is Ka?

A

The acid ionisation constant

28
Q

What is Kb?

A

The base ionisation constant

29
Q

What does a large value of Ka mean?

A

It means there are many H+ ions in solution -> a strong acid

30
Q

What does a large Kb value mean?

A

It indicates many OH- ions -> a strong base

31
Q

what does a small Ka value indicate?

A

A weak acid

32
Q

What does a small Kb value indicate?

A

A weak base

33
Q

What is the pH equation?

A

pH = -log10 [H+]

34
Q

What is the pOH equation?

A

pOH = -log to the base 10 [OH-]

35
Q

What is the equilibrium constant for water equation?

A

Kw = [H+] x [OH-] = 10^-14

36
Q

What is the H+ concentration equation?

2

A

Square root of (Ka x Macid)

Where Macid is the concentration in moles per litre

37
Q

What is the OH concentration equation?

A

Square root of (Kb x Mbase)

Where Mbase is the concentration in moles per litre

38
Q

What is the equation for the acid dissociation constant?

A

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

Ka = [H30+][A-]/[HA]

39
Q

What is the equation for the base dissociation constant?

A

Kb = [Hb+][OH-]/[B]

1.1 Chemistry (19 decks)

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