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chemistry-A2 (physical) > Acids and Bases > Flashcards

Acids and Bases Flashcards

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1
Q

What is a Bronsted-Lowry acid defined as?

A

a proton donor

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2
Q

What is a Bronsted-Lowry base defined as?

A

a proton acceptor

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3
Q

what is the product of the reaction between an Acid and a base

A

Salt + Water

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4
Q

how can we determine the concentration of an acid or a basse

A

titration

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5
Q

what is the name of the reaction between acid and base

A

neutralisation reaction

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6
Q

what is the pH of an acid

A

pH<7

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7
Q

what is the pH of a base

A

pH>7

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8
Q

what are alkalis

A

bases that are soluble in water

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9
Q

what does an acid-base equilibria involve

A

the transfer of protons

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10
Q

what is a strong acid?

A

when they dissolve in water
it competely dissociates into ions. (protons)

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11
Q

what is a weak acid?

A

when they dissolve in water
it slightly dissociates into ions

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12
Q

what is produced when acids disscoiate

A

protons

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13
Q

what is produced when bases dissociates

A

hydroxides

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14
Q

what is defined as a strong base

A

it completley dissociates into OH-
(hydroxides)

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15
Q

what is defined as a weak base

A

it slightly dissociates to hydroxide ions

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16
Q

how do we calculate the pH

A

pH = - log [H+]

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17
Q

what happens when we increase the concentration of an acid

A

it increases the acidity
pH decreases

17
Q

why does the pH decrease when we increase the concentration

A

more H+ is produced
concentration increases
when the acid dissociates

18
Q

what happens to the pH when we dilute an acid with wateer

A

increase in pH

19
Q

what happens to the concentration of the acid when its diluted by water

A

concentration decreases

20
Q

what happens to the [H+] when we dilute an acid in water

A

[H+] decreases

21
Q

what happens to the pH when we add a solid base to an acid solution

A

it will increase

22
Q

what happens to the volume of the solution when we add a solid base to the acid solution

A

volume stays the same

23
Q

what does the pH scale measure?

A

the [H+] in a solution

24
Q

what does a high [H+] suggest

A

more hydrogen ions
lower pH

24
Q

what does a low [H+] suggest

A

less hydrogen ions
higher pH

25
Q

what can water slightly dissociate into

A

H+
OH-

26
Q

what is the equation when water slightly dissociates

A

H2O -> H+ + OH-

27
Q

what type of reaction is the slight dissociation of water

A

endothermic reaction

28
Q

what does the reaction of the dissociation of water reach

A

dynamic equilibrium

29
Q

where is kw derived from

A

from the Kc of the dissociation of water

29
Q

what is the pH of water at room temperature

A

7

30
Q

what is the kw expression

A

Kw = H+ ][OH-(aq) ]

31
Q

why is pure water neutral

A

H+ = OH-

32
Q

what happens to Kw when we increase the temperature?

A

the temperature increases

33
Q

why does the value of kw increase when we increase the temperature?

A

when temperature increases the equilibrium will move to the right.
(cause the dissociation of water is endothermic)
therefore more products are formed (OH- & H+)

34
Q

what are the units for Kw

A

mol2 dm-6

35
Q

what is the value for Kw at room temperature?
298K + 25 degrees

A

1.00 x 10-14 mol2 dm-6

36
Q

Explain why the expression for Kw does not include the concentration of water. (2 marks)

A

the concentration of water is really high
concentration of water is constant

37
Q

Explain why the value of Kw increases as the temperature increases? (2 marks)

A
  1. Dissociation is endothermic
  2. Equilibrium moves to the right to oppose the increase in temperature. 9counteract change)

chemistry-A2 (physical) (2 decks)

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