Classifying Compounds

Ionic Compounds: Acids, Bases & Salts Ionic compounds are classified into 3 categories: Acids Bases Salts Acetic acid, amino acids and nucleic acid (DNA) is covalent Note: some covalent compounds can be acids or bases as well

Formulas usually start with “H” Acids Any compound that: Turns blue litmus paper red Tastes sour Reacts with some metals to produce H2 gas Conducts electricity when dissolved in water Produce H+ ions when dissolved in water e.g. HCl hydrochloric acid (stomach acid) H2SO4 sulphuric acid (battery acid) Whip scorpion – called vinegaroon smalls like vinegar and sprays acetic acid in self defense Sulfuric acid – used to clean metals & in car batteries -ate becomes ic acid -ite becomes ous acid H3C6H5O7 citric acid (lemons, oranges, etc.) HCH3COO acetic acid (vinegar) Also can be written as CH3COOH or HC2H3O2 Formulas usually start with “H”

Formulas usually end with “OH” Bases Any compound that: Turns red litmus paper blue Has a bitter taste Feels slippery Conducts electricity when dissolved in water Produce OH- ions when dissolved in water e.g. NaOH sodium hydroxide (drain cleaner) KOH Potassium hydroxide (used in batteries) Eggs & baking soda are bases AlOH3 or magnesium hydroxide - antacid NH4OH Ammonium hydroxide (household cleaner) Al(OH)3 Aluminum hydroxide (antacid) Formulas usually end with “OH”

Neutralization reactions When acids react with bases they form salts and water Acid + Base  Water + Salt e.g. HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq) HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq) This is called a NEUTRALIZATION reaction In a neutralization reaction, the properties of the acid and base are lost as water and a salt are formed. Testing pH measures concentration of H ions

Indicators Some dyes can help classify acids and bases; they change different colours in the presence of either acids or bases. These dyes are called INDICATORS ACID BASE e.g. Litmus Red Blue Phenolphthalein Colourless Pink (fuchsia) Bromothymol blue Yellow Blue (See p. 224 or your data booklet for a more detailed listing)

Salts Any ionic compound which is not an acid nor a base. e.g. NaCl sodium chloride (table salt) MgF2 magnesium fluoride CuSO4 copper(II) sulphate Salts are formed in many ways: Acids react with Bases (Neutralization) H2SO4 + Mg(OH)2  MgSO4 + 2 H2O Acid Base Salt water Salts are made of a positive ion from a base and a negative ion from an acid.

Salts continued Salts can also be formed from oxides, carbonates or metals reacting with acids. Acids + metals 2 HCl(aq) + Mg(s)  MgCl2(aq) + H2(g) Salt hydrogen gas Acids + carbonates H2SO4(aq) + CaCO3(s)  CaSO4(aq) + H2O(l) + CO2(g) Salt Oxide – compound with at least one oxygen w/ one or more elements ex. Na2O Metals w/ acids usually releases hydrogen gas Carbon dioxide trapped in rocks – carbonate rocks, limestone deposits can neutralize acid rain H2SO4 (sulfuric acid) carbonates neutralize acids protect lakes and ecosystems from acid rain

Assignment In Class: Homework: Acid / Base Worksheet Workbook Pages 91 & 92