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acids and bases Flashcards

1
Q

polyprotic acid/ (polybasic acid)

A

acid that donates more than one proton

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2
Q

polybasic species

A

bases that accept more than one proton

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3
Q

example of a monoprotic acid

A

HNO3
1 mole of HNO3 will produce one mole of H+ ions

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4
Q

example of a triprotic acid

A

H3PO4
1 mole of H3PO4 will produce 3 moles of H+ ion

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5
Q

Bronsted lowry acids

A

proton donors

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6
Q

Bronsted lowry bases

A

proton acceptors

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7
Q

Explain what Arrhenius’ proton and hydroxide ion theory was (1884) AND THE PROBLEM WITH IT

A

acids donate protons and bases release hydroxide ions

when an acid an base react they form a salt

PROBLEM: doesn’t explain why chemicals like ammonia are bases because ammonia does NOT contain hydroxide ions, so
it does not fall under the Arrhenius’ umbrella.

− ammonia does not produce OH- ions directly in solution, but rather accepts protons to form ammonium ions (NH4+).

Therefore ammonia is a bronsted lowry base and not an arrhenius base (since it does not contain hydroxide ions (OH-) and does not release them directly when dissolved in water. Instead, it reacts with water to form hydroxide ions.

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8
Q

metal + acid

A

salt + hydrogen

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9
Q

metal oxide + acid

A

salt + water

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10
Q

metal hydroxide + acid

A

salt + water

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11
Q

metal carbonate + acid

A

salt + co2 + water

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12
Q

Conjugate Acid-Base Pair

A

a pair of compounds that transform into each other by the transfer of a proton.

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13
Q

conjugate acid

A

species that has gained a proton

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14
Q

conjugate base

A

species that has lost a proton

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15
Q

water reacts with acids to form a conjugate acid:

A

H3O+

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16
Q

water reacts with a base to form a conjugate base:

A

OH-

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17
Q

is the forward or backward reaction favoured in the equilibrium equation of ethanoic acid (and other cooh)?

A

backward reaction favoured so not many protons produced

ethanoic acid is a weak acid

18
Q

is the forward or backward reaction favoured in the equilibrium equation of a strong acid (HCL, H2SO4, HNO3)?

A

forwards reaction favoured strongly.
Lots of H+ produced.

19
Q

is the forward or backward reaction favoured in the equilibrium equation of a strong base (NAOH, KOH)?

A

forward reaction favoured strongly. Lots of OH- ions produced.

20
Q

is the forward or backward reaction favoured in the equilibrium equation of a weak base (ammonia)?

A

backwards reaction favoured so not many OH- ions produced.

21
Q

What are buffer solutions?

A

Solutions which resist changes in pH when small quantities of acid or alkali are added.

22
Q

What is an acidic buffer?

A

A buffer with pH < 7, consisting of a weak acid and its sodium or potassium salt.

23
Q

What is an example of an acidic buffer?

A

Ethanoic acid and sodium ethanoate.

24
Q

What is an alkaline buffer?

A

A buffer with pH > 7, consisting of a weak base and its chloride.

25
Q

What is an example of an alkaline buffer?

A

Ammonia and ammonium chloride.

26
Q

Why is pH stability important in biological systems?

A

It is essential for processes to work properly, as most enzymes function best at particular pH values.

27
Q

What is the normal pH of blood?

A

About 7.4.

28
Q

What can happen if blood pH varies by 0.5?

A

It can lead to unconsciousness and coma.

29
Q

What role do hydrogencarbonate ions play in blood pH regulation?

A

They remove excess H+ ions.

30
Q

What is the equilibrium reaction involving carbon dioxide in blood?

A

CO2(aq) + H2O(aq) ⇌ H+(aq) + HCO3¯(aq).

31
Q

What is the dissociation reaction of a weak acid in an acidic buffer?

A

CH3COOH(aq) ⇌ CH3COO¯(aq) + H+(aq).

32
Q

What happens when acid is added to an acidic buffer?

A

H+ is removed by reacting with CH3COO¯ ions to form CH3COOH.

33
Q

What happens when alkali is added to an acidic buffer?

A

OH¯ ions react with H+ ions, shifting the equilibrium to produce more H+ ions.

34
Q

What is necessary for an acidic buffer solution to function effectively?

A

A large concentration of both CH3COOH and CH3COO¯.

35
Q

What is the formula for calculating the pH of an acidic buffer solution?

A

pH = - log10 [H+].

36
Q

What is the Ka expression for a weak acid HA in a buffer solution?

A

Ka = [H+(aq)][A¯(aq)] / [HA(aq)].

37
Q

How do you calculate [H+] in a buffer solution?

A

[H+] = [HA] * Ka / [A¯].

38
Q

What is the pH when 500cm3 of 0.10 mol dm-3 weak acid is mixed with 500cm3 of 0.20 mol dm-3 of its salt?

A

pH = 4.699 (4.7).

39
Q

What is the equilibrium reaction for an alkaline buffer?

A

NH3(aq) + H2O(l) ⇌ OH¯(aq) + NH4+(aq).

40
Q

What is needed for an alkaline buffer to work effectively?

A

A large concentration of both OH¯(aq) and NH4+(aq).

41
Q

What components are used to create an alkaline buffer?

A

Ammonia (a weak base) and ammonium chloride (its salt).

chemistry (4 decks)

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