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Chemistry 🧪 > Topic 8 Acids, Bases And Salts > Flashcards

Topic 8 Acids, Bases And Salts Flashcards

1
Q

Universal indicator at acidic, neutral and alkaline

A

Acidic - red
Neutral - green
Alkaline - purple

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2
Q

Phenolphthalein indicator at acidic, neutral and alkaline

A

Acidic - colourless
Neutral - colourless
Alkaline - pink

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3
Q

Methyl Orange indicator at acidic, neutral and alkaline

A

Acidic - red
Neutral - orange
Alkaline - yellow

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4
Q

Red litmus paper at acidic, neutral and alkaline

A

Acidic - red
Neutral - red
Alkaline - blue

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5
Q

Blue litmus at acidic, neutral and alkaline

A

Acidic - red
Neutral - blue
Alkaline - blue

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6
Q

Where are strong acids on the PH scale

A

0-2. Examples are hydrochloric, sulfuric or nitric acid

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7
Q

Where are weak acids on in the pH scale

A

3-6. Examples are ethanoic or carbonic

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8
Q

Where is neutral on the pH scale

A

7

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9
Q

Where are weak alkalis on the pH scale?

A

8-11. Examples are ammonia

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10
Q

Where are strong alkalis on the pH scale

A

12-14. Examples are sodium hydroxide or potassium hydroxide

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11
Q

What do acids produce when dissolved?

A

H+ (aq) ions. The higher the concentration of hydrogen ions, the lower the pH of the acid is

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12
Q

What do alkalis produce when dissolved?

A

OH- (aq) ions

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13
Q

What do weak acids and alkalis do in water?

A

Only partially ionise

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14
Q

What do strong acids and alkalis do in water?

A

Completely ionise

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15
Q

Dilute

A

contains a Small number of particles dissolved per unit volume

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16
Q

Concentration

A

A measure of the number of moles of acid/alkali molecules dissolved in 1dm3 of water. Measured in mol/dm3. The higher the concentration the more acid/alkali molecules that have been dissolved

17
Q

Neutralisation

A

The reaction between an acid and an alkali which produces salt and water

18
Q

What is the ionic equation for neturalisation

A

H+ (aq) + OH- (aq) = H2O (l)

19
Q

Is neutralisation an exothermic reaction?

A

Yes

20
Q

Base

A

Metal oxide/hydroxide which neutralises an acid

21
Q

Alkali

A

A soluble

22
Q

Acid + metal =

A

Salt + hydrogen

23
Q

Acid + base =

A

Salt + water

24
Q

Acid + alkali =

A

Salt + water

25
Q

What are bases and alkali?

A

Oxides/hydroxides

26
Q

Acid + carbonate =

A

Salt + water + carbon dioxide

27
Q

Acid + hydrogencarbonate =

A

Salt + water + carbon dioxide

28
Q

Acid + ammonia =

A

Ammonium salt

29
Q

Salt

A

A compound formed when some or all of the hydrogen ions in an acid are replaced by metal/ammonium ions

30
Q

How to test for hydrogen gas

A

Apply a lighted splint - if hydrogen is present there will be a popping sound

31
Q

How to test for carbon dioxide?

A

Limewater will turn from colourless to milky/cloud ly if carbon dioxide is present there

32
Q

Facts about group 1 and 2 salts

A

Most group 1 and 2, aluminium and zinc salts are white. Dissolved in water they give colourless solutions.

33
Q

What are transition metals? What do they look like?

A

They are metals between groups 2 and 3 and are generally coloured

34
Q

How do you prepare a salt from an acid and base?

A
  1. Measure 25cm3 of dilute acid and place in beaker
  2. Warm dilute acid. Do not allow to boil
  3. Add the base and stir. Continue adding until there is no further reaction and the unreacted base is in excess at the bottom of the beaker
  4. Allow to cool then filter the mixture and collect the filtrate in an evaporating basin
  5. Heat the filtrate in the evaporating basin until half of it has evaporated (to make it more concentrated)
  6. Allow basin to cool and crystals will form
  7. When crystals have formed,very between 2 pieces of filter paper/desiccator/low temperature oven
35
Q

What is the first method to prepare a salt from an acid and alkali (soluble base)?

A
  1. Fill burette with acid
  2. Using pipette and pipette filler place 25cm3 of alkali solution into a conical flask
  3. Add 3 drops of phenolphthalein into the conical flask until solution turns pink
  4. Add acid from the Buee the into the conical flask, swirl gently
  5. Stop adding acid when indicator turns colourless
  6. Record volume by reading burette
  7. The reaction is repeated for a more accurate result, then again without indicator and using the more accurate result of acid
  8. Pour solution into evaporating basin
  9. Heat gently until half of the solution remains
  10. Leave to cool and crystallise, remove crystals and dry
36
Q

What is the second method to prepare a salt from an acid and alkali (soluble base)?

A

Follow steps 1-5 of first method:
1. Fill burette with acid
2. Using pipette and pipette filler place 25cm3 of alkali solution into a conical flask
3. Add 3 drops of phenolphthalein into the conical flask until solution turns pink
4. Add acid from the burette into the conical flask and swirl gently
5. Stop adding acid when indicator turns colourless

Then:
6. Add 2 spatulas of decolourising charcoal to conical flask
7. Heat gently - do not boil
8. Allow to cool slightly, then filter mixture into evaporating basin
9. Heat again until half of the solution remains
10. Leave to cool and crystallise, remove crystals and dry

Chemistry 🧪 (7 decks)

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