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Chemistry GCSE > Topic 4 - Acid and Alkali > Flashcards

Topic 4 - Acid and Alkali Flashcards

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1
Q

acidic pH

A

less than 7

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2
Q

alkali pH

A

more than 7

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3
Q

neutral pH

A

7

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4
Q

how can you find the pH of a solution

A

using indicators

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5
Q

indicator

A

a substance that changes colour depending on the pH

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6
Q

name common acids

A
  • hydrochloric acid (HCl)
  • sulfric acid (H2SO4)
  • nitric acid (HNO3)
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7
Q

name a common alkali

A
  • sodium hydroxide (NaOH)
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8
Q

what ion does acids contain

A

H+

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9
Q

what ion does alkalis contain

A

OH-

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10
Q

what ion does neutral solutions contain

A

even concentration of H+ and OH- ions

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11
Q

concentrated solution

A

contains a lot of dissolved solute per unit volume

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12
Q

dilute solution

A

contains only a small amount of solute

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13
Q

difference in concentration of H+ ions in acid pH

A

each time (each number) you go down in pH the concentration of H+ ions i increases by 10x

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14
Q

concentration equation

A

amount dissolved / volume of solution

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15
Q

bases

A

substances that neutralise acids to form a salt and water only

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16
Q

base + acid reaction

A

base + acid -> salt + H20 (BASH20)

17
Q

during neutralisation reactions explain why the pH becomes neutral

A

the hydrogen ions combine with oxide ions to form water; this removes the’” hydrogen ions ans so the pH increases

18
Q

during neutralisation reactions explain how is a salt produced

A

salts are produced by replacing the hydrogen ions with metal ions

19
Q

method to prepare a solute

A

1) add excess of base
2) gently warm the mixture to speed up reaction
3) filter to remove the untracked solid from the solution
4) heat to evaporate water and concentrate the salt solution
5) leave to evaporate water slowly for crystallisation to occur

20
Q

what’s the difference between base and an alkali

A

base is insoluble, alkali is soluble

21
Q

what happens in a titration

A
  • acid is added from à burette to a fixed volume of alkali in a conical flask “)
  • a few drops of indicator are added to the alkali so you can follow the reaction
  • eventually the solution will reach end-point
22
Q

end-point

A

when the indicator changes colour

23
Q

how to make a pure dry salt

A
  • carry out a titration
  • note the exact volume of acid needed to neutralise the alkali
  • use the burette to add the correct volume of acid without the indicator
  • evaporate the water from the solution formed
24
Q

general equation for reaction of metal and an acid

A

metal + acid -> salt + H2 (MASH2)

25
Q

general equation for reaction of metal carbonate and an acid

A

metal carbonate + acid -> salt + H20 + CO2 (CASH2OCO2)

26
Q

precipitation reaction

A

in a precipitation reaction is one in which a soluble substance in a solutions* i cause an insoluble precipitate to form

27
Q

precipitate

A

cause (a substance) to be deposited in solid form from a solution

28
Q

what is the test for carbon dioxide

A

limewater

29
Q

what happens to the hydrogen ions in neutralisation?

A

They combine with oxide ions to form water. This removes the hydrogen ions instead of pH increases.

30
Q

Difference between single indicator and universal indicator

A

Single indicator only tells if substance is acidic or basic however universal indicator provides a more detailed indication of how acidic or basic substances by displaying a variety of colours of the pH scale

31
Q

spectator iron

A

An ion from the acid that does not change during a reaction

32
Q

Oxidation

A

Loss of electrons in a reaction

33
Q

reduction

A

gain of electrons in a reaction

34
Q

how do you work at the ionic equation?

A

Crossover method

35
Q

what happens when two solutions containing soluble cells react together?

A

The endings swap
e.g. Copper sulphate + potassium carbonate -> copper carbonate + potassium sulphate

36
Q

how to prepare insoluble salts

A
  • mix the two solutions in a beaker, then filter the mixture
  • Rinse the beaker with a little distilled water and pour this through the funnel
  • Pour a little distilled water over the precipitate in the funnel
  • Carefully remove the food paper containing the precipitate and dry in a warm oven
37
Q

What chloride are in soluble water?

A

Silver, lead chlorides

38
Q

What sulphates are in soluble in water?

A

Lead barium calcium sulphate

39
Q

what nitrates are insoluable water?

A

all of them

Chemistry GCSE (8 decks)

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