Acids and Bases
Madison Scott -& Selenia Lemly
Acids
A Lewis acid is an electron pair accepter
A Arrhenius acid, when added to water increases the number of ions in water.
Strong acids are completely ionized. Some examples are:
- hydrochloric acid
- sulfuric acid
- hydrobromic acid
Weak acids are only partly ionized
- formic acid
- hydrofluoric acid
- nitrous acid
Physical and Chemical properties of acids are:
- Physical: sour taste, soluable in water, pH levels less than 7, most acid solutions are corrosive, all acids diluted can conduct electricity
- Chemical: reacting with reactive metals to form salt and hydrogen gas, react with metal carbonates to form salt, carbon dioxide and water, reacts with bases(Alkali) to form saltwater
2 examples that you can tell if a substance is:
- When dissolving in water, if hydrogen ions go up, it is an acid
- Blue litmus paper turns red
Bases
A Lewis base donates pairs of electrons
A Arrhenius base when added to water increases the number of OH- ions in water
Strong bases are fully ionic, some examples are:
- Sodium Hydroxide
- Potassium Hydroxide
- Borium Hydroxide
Weak bases are not fully ionic, some examples are:
- Ammonia
- Pyridine
- Methylamine
Physical and Chemical Properties of bases are:
- Physical: bitter taste, slippery touch, conduct electricity,
turns red litmus paper blue
- Chemical: pH higher than 7, react with acidic substances
Reactions
Measurement
measure strength of acids and bases with the pH scale
- acid: 1-6
- neutral: 7
- base: 8-14