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CHEMISTRY > SC4 - ACIDS AND ALKALIS > Flashcards

SC4 - ACIDS AND ALKALIS Flashcards

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1
Q

acids contain ___ ions

A

hydrogen ions H+

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2
Q

alkalis contain ___ ions

A

hydroxide ions OH-

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3
Q

hydrochloric acid formula

A

HCl

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4
Q

sulphuric acid formula

A

H2SO4

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5
Q

nitric acid formula

A

HNO3

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6
Q

ways of measuring pH (2)

A
  • using an indicator and comparing the colour with the pH scale (less accurate)
  • using a digital pH meter (more accurate, to the decimal point)
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7
Q

pH of acids

A

pH 1-7

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8
Q

pH of a neutral substance eg. water

A

pH 8

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9
Q

pH of alkalis

A

9-14

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10
Q

UNIVERSAL INDICATOR: colour in acid

A

red / orange / yellow

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11
Q

UNIVERSAL INDICATOR: colour in neutral

A

green

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12
Q

UNIVERSAL INDICATOR: colour in alkali

A

purple / blue

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13
Q

PHENOLPHTHALEIN: colour in acid

A

colourless

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14
Q

PHENOLPHTHALEIN: colour in alkali

A

pink

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15
Q

METHYL ORANGE: colour in acid

A

red

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16
Q

METHYL ORANGE: colour in alkali

A

yellow

17
Q

give the names of 3 indicators

A
  • universal indicator
  • phenolphthalein
  • methyl orange
18
Q

concentrated acid definition

A

containing a large amount of acid than water in the solution

19
Q

dilute acid definition

A

containing a small amount of acid than water in the solution

20
Q

strong acid definition

A
  • all of the acid splits up into H+ ions (dissociates) when dissolved in water
  • high concentration of H+
    -low pH
21
Q

weak acid definition

A
  • only some of the acid splits up into H+ ions when dissolved in water
  • lower concentration of H+
  • higher pH (still acidic)
22
Q

the concentration of hydrogen ions decreases by a factor of __ every time the pH is increased by _

A

decreases by a factor of 10 every time the pH is increased by 1

23
Q

base definition

A
  • a metal oxide or hydroxide eg. CuO or Ca(OH)2
  • bases can neutralisé acids to give salt and water only
24
Q

general equation for base + acid

A

BASHO
base + acid -> salt + water

25
Q

salts formed by hydrochloric acid (HCl)

A

chlorides

26
Q

salts formed by sulphuric acid (HSO4)

A

sulphates

27
Q

salts formed by nitric acid (HNO3)

A

nitrates

28
Q

describe how to make a salt by reacting a base with an acid eg. copper sulphate from copper oxide + sulphuric acid

A
  • add EXCESS BASE to acid to neutralise all the acid
  • FILTER off the excess base
  • EVAPORATE the water from the solution to get crystals of the salt
  • dry the crystals in an oven
29
Q

alkali definition

A

a base that is soluble in water

30
Q

describe how to do a titration experiment

A
  • using a PIPETTE transfer a known volume of alkali into a CONICAL FLASK
  • add a few drops of INDICATOR (methyl orange or phenolphthalein)
  • add acid from a BURETTE slowly until you are near the indicator changing colour
  • add the acid drop-wise until the indicator changes colour
  • record the volume of acid used
31
Q

general equation for metal + acid

A

MASH
metal + acid -> salt + hydrogen

32
Q

test for hydrogen gas

A

when a lit splint is added to the test tube, it makes a squeaky pop

33
Q

general equation for metal carbonate + acid

A

CASHOCO
metal carbonate + acid -> salt + water + carbon dioxide

34
Q

test for carbon dioxide gas

A

lime water turns milky when carbon dioxide is bubbled through it

35
Q

describe precipitation reactions

A
  • salts that are insoluble can be made using precipitation reactions
  • the metal and non-metal part of two compounds swap round to give two new compounds
  • if one of these is insoluble it forms a precipitate
36
Q

SOLUBLE SALTS

A
  • sodium carbonate, potassium carbonate, ammonium carbonate
  • all nitrates
  • all chlorides except lead chloride, silver chloride
  • all sulphates except calcium sulphate, lead sulphate, barium sulphate
  • all ammonium salts
  • all group 1 metal salts
37
Q

INSOLUBLE SALTS

A
  • all carbonates except sodium carbonate, potassium carbonate, ammonium carbonate
  • lead chloride, silver chloride
  • calcium sulphate, lead sulphate, barium sulphate

CHEMISTRY (13 decks)

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