Acids and Bases Unit 13

Acids

1) Acids start with hydrogen, and some react with active metals to liberate hydrogen gas. Ba (s) + H 2 SO 4(aq) BaSO 4 (aq) + H 2(g)

Properties of Acids 2) Acids change the color of dyes known as “acid-base indicators” Acids turn litmus paper turns red.

Properties of Acids 1) Acids have a sour taste.

Properties of Acids 4) Acids react with bases to produce salt and water. This is a neutralization reaction. Mg(OH) 2 + HCl --> MgCl 2 + HOH

5) Acids conduct electrical currents in an aqueous solution. Acids are electrolytes.

6) Acids produce hydrogen ions when dissolved in water.

Bases

1) End with (OH) hydroxide

2) Change the color of acid- base indicators litmus paper: red  blue

3) Bases feel slippery.

Properties of Bases 4) Bases react with acid to produce salt and water. This is called neutralization reaction. 5) Bases are electrolytes. What?

6) Bases produce hydroxide ions when dissolved in water. 6) Bases produce hydroxide ions when dissolved in water.

Names and Formulas of Acids If acid is binary & ends with –ide: 1)hydro-(stem)-ic acid If the acid is TERNARY: (no HYDRO!) 2) If anion ends with –ite: (stem)-ous acid 3) If anion ends with –ate: (stem)-ic acid

Names and Formulas of Acids To write formulas for acid: To write formulas for acid: Balance the charges Balance the charges (Use criss-cross method).

Practice – A. H 3 PO 4 :_________________ – B. H 2 S:____________________ – A. Hydrobromic acid:_______________ – B. Nitrous acid:___________________

Names and Formulas of Bases 1. Bases are compounds that produce hydroxide ions when dissolved in water.-ALKALINE 1. Bases are compounds that produce hydroxide ions when dissolved in water.-ALKALINE 2. Ionic compounds that are bases are named like ionic compounds 2. Ionic compounds that are bases are named like ionic compounds

Naming Bases Name metal then add hydroxide Name metal then add hydroxide Base Examples Base Examples Ca(OH) 2 : Ca(OH) 2 : NaOH: NaOH:

Write the formula from the name for the following bases. Aluminum hydroxide = Aluminum hydroxide = Ammonium Hydroxide = Ammonium Hydroxide =

Neutralization Reactions A reaction between traditional acids (hydrodium ions) and bases (hydroxide ions) produces water and one of a class of compounds called salts A reaction between traditional acids (hydrodium ions) and bases (hydroxide ions) produces water and one of a class of compounds called salts H 3 O+(aq) + OH−(aq)  2H 2 O(l) H 3 O+(aq) + OH−(aq)  2H 2 O(l)

Acid Base Reactions 1. Salt- ionic compound composed of a OH - from an Arrhenius base and an H 3 O + from an Arrhenius acid 1. Salt- ionic compound composed of a OH - from an Arrhenius base and an H 3 O + from an Arrhenius acid 2HNO 3 + Ca(OH) 2 Ca 2+ (NO 3 - ) 2 + 2HOH 2HNO 3 + Ca(OH) 2 Ca 2+ (NO 3 - ) 2 + 2HOH H 2 S + 2NaOH Na 2 + S HOH H 2 S + 2NaOH Na 2 + S HOH Double Replacement Double Replacement

Uses of Common Acids Sulfuric acid: H 2 SO 4 is used in car batteries, paper manufacturing and many other manufacturing processes. Sulfuric acid is the #1 industrial chemical produced in the world.

Uses of Common Acids Phosphoric acid: H 3 PO 4. Fertilizers and animal feed Sour taste, not toxic Flavoring agent: Coca Cola ® Cleaning agent Manufacturing of detergents and ceramics

Hydrochloric acid:HCl 1. Stomach produces HCl to aid in digestion. 2. In the industries, it’s used for “pickling” iron and steel to remove impurities. 3. General cleaning agent, used in food processing, activation of oil wells, recovery of magnesium from sea water and production of other chemicals. 4. Dilute HCl, commonly known as muriatic acid, is used to correct acidity in swimming pools and cleaning masonry. 5. Used in toilet bowl cleaners

Acetic Acid: HC 2 H 3 O 2 1. Synthesizes chemicals used in making plastics. 2. Raw material in producing food supplements- lysine, an essential amino acid 3. Used as a fungicide 4. White vinegar contains 4-8% acetic acid 5. Used to produce food products such as pickles

Acid Rain Normal rain pH of 5.3 Normal rain pH of 5.3 Acid rain pH of Acid rain pH of

Acid Rain Man-Made Causes Man-Made Causes – Burning of fossil fuels (coal production – yucky!) –carbon dioxide + water => carbonic acid

4. Results of acid rain- changes ecosystems a) kills aquatic life a) kills aquatic life b) deteriorates statues and buildings and bridges b) deteriorates statues and buildings and bridges

Traditional Acid  Definition: An Arrhenius acid is a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solution.  HNO 3 + H 2 O  H 3 O + + NO 3 -

B. Acid- Base reactions- Arrhenius (traditional) Acid – Base Reactions 1. An acid-base reaction occurs in aqueous solution between a strong Arrhenius acid that completely dissociates to produce H 3 O +, and a strong Arrhenius base that completely dissociates to produce OH − 1. An acid-base reaction occurs in aqueous solution between a strong Arrhenius acid that completely dissociates to produce H 3 O +, and a strong Arrhenius base that completely dissociates to produce OH − HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l) HCl(aq) + NaOH(aq)  NaCl(aq) + H 2 O(l)

 c. Their water solutions are known as aqueous acids. All pure aqueous acids are electroytes.  HNO3(l) + H2O(l) H3O+(aq) + NO3−(aq)  HCl(g) + H2O(l) H3O+(aq) + Cl−(aq)

Traditional Bases Arrhenius base is a substance that contains hydroxide ions (OH - ) and dissociates to produce hydroxide ions (OH-) into solutions Arrhenius base is a substance that contains hydroxide ions (OH - ) and dissociates to produce hydroxide ions (OH-) into solutions NaOH(s) Na+(aq) + OH−(aq) NaOH(s) Na+(aq) + OH−(aq)