Acids, Bases and Alkalis Cheat Sheet by fongrsy

Metal + Acid  Salt + Hydrogen Gas
Metal Carbonate + Acid  Salt + Water + Carbon Dioxide
Metal Oxide + Acid  Salt + Water
Metal Hydroxide + Acid  Salt + Water
Base + Acid  Salt + Water (Neutr­ali­sation)
Alkali + Acid  Salt + Water (Neutr­ali­sation)
Alkali + Ammonium Salt  Salt + Water + Ammonia Gas
Alkali + Salt  Metal Hydroxide + Salt

Acidic solutions have pH values < 7.
They contain more H⁺ ions and fewer OH^- ions.
Neutral solutions have pH values = 7.
They contain equal amounts of H⁺ ions and OH^- ions.
Alkaline solutions have pH values > 7.
They contain more OH^- ions and fewer H⁺ ions.

1. Acids are corrosive.
2. Acids have a sour taste.
3. Acidic solutions conduct electr­icity. (Elect­rol­ytes)
4. Acids change the colour of indica­tors.

Litmus Paper: Blue to Red
Methyl Orange Solution: Orange to Red
Universal Indicator Paper: Orange to Red
Universal Indicator Solution: Green to Red

1. Alkalis have a soapy feeling and a bitter taste.
2. Alkaline solutions conduct electr­icity. (Elect­rol­ytes)
3. Alkalis change the colour of indica­tors.

Litmus Paper: Red to Blue
Methyl Orange Solution: Orange to Yellow
Universal Indicator Paper: Orange to Violet
Universal Indicator Solution: Green to Violet

Step 1: Write down the chemical equation.
Step 2: List down the atoms (or polyatomic ions) involved in both sides.
Step 3: Count the number of atoms on both sides.
Step 4: Compare both sides and change the coeffi­cients (not subscr­ipts) so that the atoms on the left side are equal to the atoms on the right side.
(Tip: Balance the Metals first, then the Non-Metals, and then the Oxygen atoms and Hydrogen atoms.)
Step 5: Double check both sides to make sure the atoms on both sides are equal.

1. For solid samples, weigh the solid and dissolve in a known volume of solution (usually 100cm³).
2. Use a pipette to measure a known volume of the solution (e.g 10cm³) and empty into an Erlenmeyer flask.
3. Add a few drops of indicator into the solution.
4. Put the second chemical into a burette. This other solution will react with the synthe­sised chemical sample in the flask. Often the solution in the burette is an acid or alkali, and it must be of a precise, known concen­tra­tion.
5. Drop by drop, mix the chemical in the burette into the Erlenmeyer flask until the end point is reached. A colour change indicates the correct amount has been added to react completely with the chemical in the sample.
6. Take note of the volume of the solution added from the burette.