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Chemistry module 5 > 5.1.3 Acids, Bases and Buffers > Flashcards

5.1.3 Acids, Bases and Buffers Flashcards

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1
Q

acids dissociate and release ….

A

H+ ions

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2
Q

Alkalis dissociate and release…..

A

OH- ions in solution

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3
Q

Bronsted-Lowry Acid

A

a species that donates a proton

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4
Q

Bronsted- Lowry base

A

species that accepts a proton

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5
Q

conjugate acid-base pairs

A

an acid and a base that can become each other through the transfer of a H+ /proton

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6
Q

Hydronium ion

A
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7
Q

monobasic

A

when one mole of acid dissociates to form one mole of H+ ions/protons

acids that release one proton into solution. Has one H that can be replaced.

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8
Q

example of mono basic acids

A

HCl, CH3COOH

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9
Q

dibasic acid, example

A

when one mole of acid dissociates to form 2 moles of H+/ protons

An acid that contains two replaceable hydrogen atoms per molecule of the acid - produces 2 H+ ions

H2CO3, H2SO4

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10
Q

tribasic

A

when one mole of acid dissociates to form 3 moles of H+/protons

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11
Q

why is CH3COOH mono basic ?

A

organic acids don’t replace any hydrogen atoms from the carbon chain

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12
Q

acid + carbonate

A

salt and water and co2 (carbonates are bases)

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12
Q

acid + metal

A

salt + hydrogen

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13
Q

why is solid carbonate included in the ionic equation?

2H+ + CuCO3 (s) —> Cu 2+ (aq) + H20(l) + CO2 (g)

A

it changes state to a gas, which is included in an ionic equation

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14
Q

what does pH measure?

A

the concentration of H+ ions in solution

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14
Q

hydrogen ion concentrations have a large range of values, what method makes it a more manageable scale?

A

negative log (10^-)

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15
Q

equation to find pH from H+ concentration

A

pH = -log (H+)

16
Q

equation to find H+ ion concentration from pH value

A

[H+] = 10 to the minus pH

17
Q

how does a change in pH by 1 affect H+ ion concentration?

A

x 10 difference

18
Q

How would you dilute a solution from 1 to 4 pH?

A

changes by pH of 3 so dilute by 10x10x10 = 1000 times

19
Q

How many more H+ ions does a solution of pH 1 have compared to ph 14?

A

10 to the power of 13

20
Q

when calculating pH of a strong, monobasic acid, why is H+ equal to the concentration of the acid?

A

amount of H + ions determines concentration and if strong acids completely dissociate their H+ ions , thats equal to concentration

21
Q

What is the version of the equilibrium constant used in acid-base equilibria?

A

acid dissociation constant (Ka)

22
Q

What does the Ka value measure?

A

the amount a weak acid dissociates. strong acids fully do.

23
Q

formula of Ka?

A

Ka = concentration of products / concentration of reactants

24
Q

what does a larger Ka value mean? and why?

A

more dissociation so stronger acid, because for equilibrium to be further right, number at top (concentration of ions) needs to be bigger than bottom (concentration of acid)

25
Q

what factor changes equilibrium constant Ka?

A

temperature - affects all equilibrium constants

26
Q

Ka values are hard to compare, so what negative algorithm value is used?

A

pKa

27
Q

pKa =

A

-log Ka

28
Q

How can you find ka from pKa?

A

10 to the -pKa

29
Q

compare the size of ka and pKa in a strong acid

A

stronger the acid, larger Ka value because more dissociation, smaller the pKa

30
Q

compare the size of Ka and pKa in a weak acid

A

weaker the acid, smaller the Ka, bigger the pKa

31
Q

water acts as both an acid and as a abase, show its acid base equilibrium

A

H20 + H20 —> H30+ + OH-

32
Q

what is the acid dissociation constant for water?

A

Ka = [H+ (aq)] [OH- (aq)] / [H2O(l) ]

32
Q

weak acids partially dissociate, how is that shown?

A

through arrow going both ways (equilibrium arrow)

33
Q

What is Kw?

A

Ionic product of water - the ions in water H+ and OH- multiplied together

34
Q

equation for Kw?

A

Kw = [H+][OH-]

35
Q

in aqueous solution there will always be both H+ and OH- ions in solution. However, when there are more H+ ion, it is …

A

acidic

36
Q

in an acid solution with pH 4, what is the concentration of OH- ions?

A

10 to the power of -10 because concentrations of H+ and OH- add up to -14 (kw value)

37
Q

How do you find the pH of a strong base?

A

use kw - find H+ concentration and ionic product of water value to find OH-

38
Q

How is finding the pH of a mono basic base and dibasic base different?

A

have to multiply number of OH+ ions by 2 because its a dibasic base so produces two moles of OH- ions

39
Q

when there are two acids in a reaction, How do you know which acids as a base or acid?

A

the strongest acid will act as the acid (bigger Ka value etc ) and other as the base

Chemistry module 5 (1 decks)

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