Folding Notes – How to Use
Print the following two pages back to back and follow the cutting instructions to create your folding notes.
The answers to the blanks are given below in order of appearance.
Chemical reactions:
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Higher
Requires
Cold
Lower
Releases
Hot
pH:
Law of the Conservation of Mass:
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Equal
Balanced
1
16
1
16
Acids:
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Hydrogen ions
Neutral
Indicators
Basic
Acidic
Acidic
Basic
Bases:
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Hydrogen ions
7
Sour
Metals
Red
CH3COOH
HNO3
Hydrochloric
H2SO4
Neutralisation reactions:
Hydroxide ions
7
Bitter
Slippery
Blue
NH3
Sodium hydroxide
Acid + metals reactions:
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Salt
Colourless
Odourless
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Base
Water
Positive
Negative
Acid + carbonate reactions:
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Carbonate
Carbon dioxide
Oxygen
As a word equation, chemical reactions are written like:
Reactants  Products
In endothermic reactions products are _____________
energy than the reactants so the reaction ___________
energy. Endothermic reactions are hot/cold (circle one).
“The mass of the products in a chemical reaction must
________ the mass of the reactants”.
When written in symbol form, chemical equations must
be _____________. An example of this is:
2 H2 + O2  2 H2O
In exothermic reactions products are _______________
energy than the reactions so the reaction ___________
energy. Exothermic reactions are hot/cold (circle one).
The atomic mass of: hydrogen = ____, oxygen = ____.
So the mass on the reactant and product side is equal:
(2 x 2 x _____) + (2 x _____) = 38
pH stands for “potential of Hydrogen” and is a measure
of how many ___________________ exist in a solution.
pH ranges from 1 – 14, where a pH of 7 is ___________.
Acids produce ____________________ in solution.
1 2 3 4 5 6 7 8 9 10 11 12 13 14

acidic


basic
We can measure pH using ________________.
Common examples include:
- universal indicator (produces a pH rainbow)
- litmus paper (blue =__________, red =___________)
- phenolphthalein (colourless =______, purple =______)
Bases produce ____________________ in solution.
For example:
NaOH  Na + OH
+
-
Properties of bases:
- have a pH greater than ___
- taste _________
- feel ___________ (imagine holding a wet bar of soap)
- turn red litmus paper ___________
Common bases: ammonia (______), bleach, soap and
______________________________ (NaOH).
HCl  H+ + Cl-
For example:
Properties of acids:
- have a pH less than ___
- taste ______ (an example is vinegar - acetic acid)
- corrode ____________
- turn blue litmus paper ___________
Common acids: acetic acid (______), nitric acid (____),
____________ acid (HCl) and sulfuric acid (______).
When an acid and a _______ react they form a neutral
salt (ionic compound) and _____________.
Acid + Base  Salt + Water
The water forms because H+ + OH-  H2O. The salt is
the combination of the ______________ ion from the
base and the _______________ ion from the acid.
An example neutralisation reaction is:
hydrochloric acid
sodium chloride
HCl + NaOH  NaCl +
H2O
sodium hydroxide
When an acid and a metal (other than gold, silver or
copper) react they form a ______ and hydrogen gas.
water
When an acid and a carbonate or hydrogen _________
react they form a salt, water and _________________.
Acid + Metal  Salt + Hydrogen gas
Acid + CarbonateSalt + Water + Carbon dioxide
To identify hydrogen gas which is ______________ and
______________ we can use the pop test.
An example acid and metal reaction is:
The carbonate (CO32-) loses one _____________ atom
to form the rest and then becomes the carbon dioxide.
An example acid and carbonate reaction is:
hydrochloric acid
magnesium chloride
2 HCl + Mg  MgCl2 +
magnesium metal
H2
hydrogen gas
hydrochloric acid
dioxide
calcium chloride
carbon
2 HCl + CaCO3  CaCl2 + H2O + CO2
calcium carbonate
water
Law of
Conservation
of Mass
This is the back side of the notes
Chemical
reactions
 Cut along these dotted lines 
and fold the tabs to the other side
Acids
You may glue this blank surface to
your workbook if you wish
pH
Neutralisation
reactions
Bases
Acid +
carbonate
reactions
Acid + metal
reactions