Properties of Acids & Bases
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Transcript Properties of Acids & Bases
PROPERTIES OF ACIDS &
BASES
WEEK OUTLINE:
Monday: Properties of Acids & Bases
Tuesday: Acid Precipitation
Wednesday: Properties of Acids & Bases Lab
Stations
Thursday: Neutralization Reactions
Friday: Acid/Base Quiz
Making an Indicator – Acids & Bases at Home Lab
NEXT WEEK:
Monday (Dec 14): Review Class
Tuesday (Dec 15): Chemistry Test
Wednesday- Friday (Dec 16-18) Start Climate
Change Unit
WHAT DO YOU THINK?
Page 265: True or False?
Stomach acid can dissolve metals like a coin in a
child’s stomach?
We all contribute to the production of acid
precipitation?
Even diet soda drinks can cause tooth decay?
Medications for heartburn work by cooling the
stomach?
All acids are dangerous?
Soft drinks can be used to make spilled drain
cleaner safer?
PROPERTIES OF ACIDS AND BASES
Young children like to explore by putting things
in their mouths
Occasionally objects get swallowed!
Coins are the most common object to be
swallowed
Once in the stomach, the coin in bathed in a
corrosive mixture that includes hydrochloric acid
(HCl (aq)) and other digestive juices
The concentration of HCl in your stomach is
about the same as ones we have used in class what do you think happens to the coin?
PROPERTIES OF ACIDS
Chemists
classify substances by their
properties
Acids - are substances that react with metals
and carbonates, conduct electricity, turns
blue litmus red, and neutralize bases
Acids also taste sour, but you should never
taste chemicals in a lab!
Very useful in food industry - act as
preservatives (vinegar and lemon juice)
PROPERTIES OF ACIDS
Reaction
with Metals
Acids react with metals to produce
hydrogen gas
Ex. hydrochloric acid + zinc → hydrogen
gas + zinc chloride
2HCl (aq) + Zn (s) → H2 (g) + ZnCl2
(aq)
PROPERTIES OF ACIDS
Reaction
with Carbonates
Acids react with carbonates to produce
carbon dioxide gas
Ex. acetic acid + sodium hydrogen
carbonate → carbon dioxide + water +
sodium acetate
HC2H3O2 (aq) + NaHCO3 (aq) → CO2
(g) + H2O (l) + NaC2H3O2 (aq)
PROPERTIES OF ACIDS
Electrical
Conductivity
Many acids are good conductors of
electricity
A solution can only conduct electricity if it
contains ions
Since acids are molecular compounds
they do not contain ions
PROPERTIES OF ACIDS
Electrical
Conductivity (Continued)
However, collisions with water molecules
break acid molecules apart to form cations
(hydrogen ions) and anions
Ex. Hydrochloric acid forms hydrogen and
chloride ions:
HCl (aq) → H+ (aq) + Cl- (aq)
CHEMICAL FORMULAS OF ACIDS
All acids produce hydrogen ions when dissolved
in water
Hydrogen ions give acids their properties
The chemical formula of an acid begins with an H
and is usually followed by an “(aq)”
This is because an acid shows its properties
when dissolved in water
Hydrogen chloride - gas that would dissolve in
water in lungs when inhaled = forming highly
corrosive hydrochloric acid
NAMES OF ACIDS
Two
common groups of acids:
Binary Acids (Table 1 Page 269)
Acid Name
Chemical Formula
Hydrofluoric acid
HF (aq)
Hydrochloric acid
HCl (aq)
Hydrobromic acid
HBr (aq)
Hydrosulfuric acid
H2S (aq)
NAMES OF ACIDS
Oxyacids – related to polyatomic ions (Table 2
Page 269)
Acid
Chemical
Formula
Related
polyatomic ion
Polyatomic ion
name
Acetic acid
HC2H3O2 (aq)
C2H3O2- (aq)
Acetate
Nitric acid
HNO3 (aq)
NO3- (aq)
Nitrate
Carbonic acid
H2CO3 (aq)
CO3-2 (aq)
Carbonate
Sulfuric acid
H2SO4 (aq)
SO4 -2 (aq)
Sulfate
Phosphoric acid
H3PO4 (aq)
PO4 -3 (aq)
Phosphate
PROPERTIES OF BASES
Bases - conduct electricity, change the colour of
acid-base indicators, feel slippery and taste bitter
PROPERTIES OF BASES
Electrical Conductivity
Bases are electrolytes, meaning their solutions
are good conductors of electricity
Ex. NaOH (sodium hydroxide) is an electrolyte
because in water it separates into ions as it
dissolves
NaOH (s) → Na+ (aq) + OH- (aq)
Many common bases are ionic compounds - they
are made up of ions (unlike acids)
As they dissolve in water, their ions are released
NAMES AND CHEMICAL FORMULAS
OF BASES
Table 4 Page 271
Base
Chemical Formula
Sodium hydroxide
NaOH (aq)
Calcium hydroxide
Ca(OH)2 (aq)
Ammonium hydroxide
NH4OH (aq)
Magnesium hydroxide
Mg(OH)2 (aq)
Aluminum hydroxide
Al(OH)3 (aq)
Sodium hydrogen carbonate
(baking soda)
NaHCO 3 (aq)
COLOUR WITH ACID-BASE
INDICATORS
A substance that changes colour depending on
the acidity or basicity of the solution is known as
an acid-base indicator
COLOURS OF COMMON SYNTHETIC
ACID-BASE INDICATORS
Table 3 Page 270
Indicator
Colour in Acid
Colour in Base
Bromothymol blue
Yellow
Blue
Phenolphthalein
Colourless
Pink
Pheol Red
Yellow
Red/pink
Litmus
Red
Blue
Methyl orange
Red
Orange/Red
THE PH SCALE
pH scale - a numerical scale of all the possible
values of pH from 0 to 14
pH is a measure of how acidic or basic a solution
is
A solution with a pH of 7 is considered neutral
A solution with pH of less than 7 is considered
acidic
A solution with pH of greater than 7 is
considered basic
THE PH SCALE CONTINUED
Solutions with highest hydrogen ion
concentration are near zero on pH scale
Solutions with highest concentrations of
hydroxide ions are near 14 on pH scale
Can use the words “acidity” or “basicity” to
describe the properties of acids or bases
ACID AND BASE HOMEWORK
Page 271 #1-5