Acids and Bases

Conjugate acid of $NH_3$

Conjugate base of $NH_3$

Conjugate acid of $H_2O$

Conjugate base of $H_2O$

Oxygen atom

Hydrogen atom

Lone pair of electrons

Metal atom

$H_3O^+$

$OH^-$

$H_2O$

$H_4O^{2+}$

Oxygen

Hydrogen

Carbon dioxide

Nitrogen

$0.1\text{ mol dm}^{-3}$ $CH_3COOH$

$0.1\text{ mol dm}^{-3}$ $HCl$

$0.1\text{ mol dm}^{-3}$ $NH_3$

Pure distilled water

Ammonium ethanoate

Sodium ethanoate

Ammonium nitrate

Methyl ethanoate

2 times

10 times

20 times

100 times

pH 0

pH 1

pH 7

pH 14

$1.0 \times 10^{-4}\ mol\,dm^{-3}$

$1.0 \times 10^{-7}\ mol\,dm^{-3}$

$1.0 \times 10^{-10}\ mol\,dm^{-3}$

$1.0 \times 10^{-14}\ mol\,dm^{-3}$

Hydrofluoric acid ($HF$)

Hydrobromic acid ($HBr$)

Hydroiodic acid ($HI$)

Perchloric acid ($HClO_{4}$)

Partial dissociation in water

High electrical conductivity

Slippery feel to the touch

Turns universal indicator purple

$CO_{2}$

$HCl$

$HBr$

$SO_{3}$

Plant respiration

Volcanic eruptions

Glacial melting

Animal migration

They neutralize the acids

They provide a surface for reactions and act as catalysts

They prevent the sun from reaching the ground

They absorb all the moisture in the air

Hydrochloric acid

Calcium carbonate

Sodium sulfate

Nitric acid

$Al^{3+}$

$BCl_{3}$

$NH_{3}$

$FeCl_{3}$

They both donate electron pairs

They both accept electron pairs

They both donate protons

They both accept protons

$Cl^{-}$

$SnCl_{2}$

$SnCl_{3}^{-}$

Tin metal

$9.0$

$5.0$

$14.0$

$1.0 \times 10^{-9}$

Concentration of the acid

Presence of a catalyst

Temperature

Initial pH of the solution

$1.00$

$1.30$

$2.00$

$0.05$

3

7

11

13

Only Phenolphthalein

Only Methyl Orange

Both Bromothymol Blue and Phenolphthalein are usually suitable

Only Alizarin Yellow

The point where pH is 7

The point where half the volume of base to reach equivalence has been added

The point where the indicator changes color

The point where the acid is completely neutralized