5.2 Salts Not just a flavour! Can be formed several ways • • • Acid – Base Neutralization Oxides and carbonates reacting with acid Metal reacting with acid Salts have many uses • Table Salt: NaCl Aluminum Sulfate: Al2(SO4)3 Making batteries, explosives, fertilizers, multivitamin and mineral tablets, blood and urine, tree sap Magnesium acetate: Mg(CH3COO)2 Salts - Neutralization • • • • • • A Salt results when an acid reacts with a base. Both are neutralized. The H+ and OH- ions combine to form water. The non-metallic ions of the acid and the metal ions of the base form the salt. Acid + Base ----> Salt + Water HCl + NaOH ----> NaCl + H2O H2SO4 + Ca(OH)2 ----> CaSO4 + H2O Metal and non-metal oxides Chemically combined with oxygen. Metal oxide: a metal combined with oxygen • • Solution becomes basic when dissolved in water Na2O(s) + H2O (l) 2NaOH (aq) Non-metal oxide: a non-metal combined with oxygen • • Solution becomes acidic when dissolved in water SO3 (g) + H2O (l) H2SO4 (aq) Acids and Metals The most reactive metals appear on the extreme left of the periodic table • • When metals react with acids, they usually release hydrogen gas 2HCl (aq) + Mg (s) MgCl2(aq) + H2 (g) online metals in acid demo Acids and Carbonates Carbonate is a combination of carbon and oxygen • Carbonate (CO3) is trapped in rocks When carbonate rocks react with acids, the carbonates help neutralize the acid Liming is a process that people do to help neutralize acidic lakes. Liming adds calcium carbonate (CaCO3) to the lake. Very expensive. Carbonates reacting with acid release CO2 • H2SO4 + CaCO3 • • • • CaSO4 + H2O + CO2 The Naked Egg The chemistry of removing an egg shell Eggshells are made up of calcium carbonate • CaCO3 • CH3COOH • 5% acetic acid 95% water Vinegar is also called acetic acid (5% solution) The chemical reaction is: 2CH3COOH + CaCO3 • Ca(CH3COO)2 + H2O + CO2 The eggshell has been removed leaving the thin membrane called a semi-permeable membrane which water can pass through. • What were the bubbles on the surface of the egg? • Think about the impact of acid rain on shells in nature! The Naked Egg Bubbles of CO2 Osmosis: water traveling through a membrane from a high concentration to a low concentration. 5.2 Salts • Salts are ionic compounds formed when acids and bases react. Salts are also produced when oxides or carbonates react with acids or when metals react with acids. • Table salt, NaCl, is found in sea water, salt lakes or rock deposits. Salt was once very valuable as a commodity. Iodine is now added to salt to minimize goiter (a disease of the thyroid). • NaCl is only one kind of salt. A salt is made up of a positive ion from a base and a negative ion from an acid. Salts are found in many things: In batteries, explosives and fertilizers In multivitamins In many living cells Salt crystals in Death Valley See pages 234 - 235 (c) McGraw Hill Ryerson 2007 Acid-Base Neutralization, and Metal Oxides and Non-Metal Oxides • Neutralization reactions occur when an acid and a base react to produce a salt and water. HCl(aq) + NaOH(aq) NaCl(s) + H2O(l) acid base salt water • Metal oxides react with water to form bases. Na2O(s) + H2O(l) 2NaOH(aq) • Non-metal oxides react with water to form acids SO2(g) + H2O(l) H2SO3(aq) Non-metal oxides are formed from the burning of fossil fuels. Acid added to water in the atmosphere = acid precipitation. The effects of acid rain on a forest See pages 236 - 237 (c) McGraw Hill Ryerson 2007 Acids and Metals, and Acids and Carbonates • Acids and Metals The most reactive metals, at the bottom of groups 1 and 2 on the periodic table, react vigorously with water and acids. All other metals are less reactive than those in groups 1 and 2. When metals do react with acids, H2 gas is usually released. 2HCl(aq) + Mg(s) MgCl2(s) + H2(g) • Acids and Carbonates Carbonates neutralize acids, protecting locations with natural carbonate supplies from acid precipitation. H2SO4(aq) + CaCO3(s) CaSO4(s) + H2O(l) + CO2(g) sulphuric acid calcium carbonate calcium sulphate water carbon dioxide See pages 238 - 239 Take the Section 5.2 Quiz (c) McGraw Hill Ryerson 2007