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Chemistry > Acids, Bases and Salts > Flashcards

Acids, Bases and Salts Flashcards

1
Q

what colour is produced by litmus paper when in acidic solution?

A

red

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2
Q

what colour is methyl orange in alkali?

A

yellow

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3
Q

what colour is phenolphthalein in acid?

A

colourless

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4
Q

what colour is methyl orange in acid?

A

red

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5
Q

what colour is litmus paper in alkali?

A

blue

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6
Q

what colour is phenolphthalein in alkaline?

A

pink

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7
Q

what colour is a universal indicator in acid?

A

red

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8
Q

what colour is universal indicator in alkaline?

A

blue

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9
Q

what is the word equation for metals reacting with acid?

A

metal + acid ⇒ salt + hydrogen

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10
Q

what is the word equation for acids reacting with bases?

A

acid + base ⇒ salt + water

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11
Q

what does hydrochloric acid form?

A

chloride

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12
Q

what does nitric acid form?

A

nitrate

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13
Q

what does sulphuric acid form?

A

sulphate

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14
Q

what is the word equation for acid reacting with metal oxide?

A

acid + metal oxide ⇒ salt + water

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15
Q

what is the word equation for acid and metal hydroxide reacting together?

A

acid + metal hydroxide ⇒ salt + water

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16
Q

what is the word equation for acid reacting with metal carbonate?

A

acid + metal carbonate ⇒ salt + water + carbon dioxide

17
Q

describe how to prepare salts from neutralisation reactions ( i.e. dilute acid reacting with excess metal oxide or metal carbonate)

It can also be seen in terms of H+ and OH-

A

acid + base => salt + water

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

18
Q

explain how to carry out an acid-alkali titration

A

Method

  • Use the pipette and pipette filler to add 25 cm3 of alkali to a clean conical flask.
  • Add a few drops of an indicator and put the conical flask on a white tile (so you can see the colour of the indicator more easily).
  • Fill the burette with acid and note the starting volume.
  • Slowly add the acid from the burette to the alkali in the conical flask, swirling to mix.
  • Stop adding the acid when the end-point is reached (the appropriate colour change in the indicator happens). Note the final volume reading.
  • Repeat steps 1 to 5 until you get consistent readings
  • The same method works for adding an alkali to an acid - just swap around the liquids that go into the conical flask and burette.
19
Q

what is an acid?

A

a substance that produces hydrogen ions ( H+) when dissolved in water

20
Q

what is a base?

A

bases are substances that react with acids and neutralises them

21
Q

explain the term weak and strong, as applied to acids

A

Strong acids

In aqueous solution, a strong acid is one that completely dissociates (splits up) into ions.

Example: hydrochloric acid.

HCl(g) + H2O(l)→H+(aq) + Cl-(aq)

This is not a reversible reaction, and 100% of the HCl molecules dissociate into ions.

Other strong acids include nitric acid and sulphuric acid.

Weak acids

In aqueous solution, a weak acid is one that only partially dissociates into ions. As a result, a state of equilibrium is produced.

22
Q

explain the term weak and strong, as applied to bases

A

Strong bases

In aqueous solution, a strong base is one that completely ionises.

Example: sodium hydroxide.

NaOH(s) + H2O(l)→Na+(aq) + OH-(aq)

This is not a reversible reaction, and 100% of the NaOH(s) splits into free ions.

Weak bases

In aqueous solution, a weak base is one that only partially ionises. Just as with weak acids, a state of equilibrium is produced.

23
Q

hydrochloric acid + sodium carbonate => sodium chloride + water + carbon dioxide (add metal carbonates to give salt + water + carbon dioxide)

A

2HCl + Na2CO3 => 2NaCl + H2O + CO2

24
Q

sulfuric acid + calcium carbonate => calcium sulfate + water + carbon dioxide

A

H2SO4 + CaCO3 => CaSO4 + H2O + CO2

25
Q

nitric acid + calcium carbonate => calcium nitrate + water + carbon dioxide

A

2HNO3 + CaCO3 => Ca(NO3)2 + H2O + CO2

26
Q

hydrochloric acid + copper oxide => copper chloride + water (acids react with metal oxide to form salt + water)

A

2HCl + CuO => CuCl2 + H2O

27
Q

sulfuric acid + zinc oxide => zinc sulfate + water

A

H2SO4 + ZnO => ZnSO4 + H2O

28
Q

nitric acid + copper oxide => copper nitrate + water

A

2HNO3 + CuO => Cu(NO3)2 + H2O

29
Q

what salts are soluble in water?

A

potassium, sodium & ammonium (soluble carbonates), nitrates, most chlorides (except silver chloride), most sulfates (except barium and calcium sulfate)

30
Q

what does the rate of reaction depend on?

A

temperature, concentration (or pressure for gases), catalyst & size of particles (or surface area)

31
Q

how do you find the rate of reaction?

A

rate of reaction = amount of reactant used or amount of product formed / time

Chemistry (12 decks)

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