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Acids and Bases

Acids and Bases. Acids. A compound that produces hydrogen ions: H+(aq) when it dissolves in water. Aqueous solutions of acids conduct electricity because of the ions in the solution. This process is called ionization. EG. HCl(aq) --> H+(aq) + Cl-(aq). Naming Binary Acids.

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Acids and Bases

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  1. Acids and Bases

  2. Acids • A compound that produces hydrogen ions: H+(aq) when it dissolves in water. • Aqueous solutions of acids conduct electricity because of the ions in the solution. This process is called ionization. • EG. HCl(aq) --> H+(aq) + Cl-(aq)

  3. Naming Binary Acids • Binary acids are made of hydrogen and a non-metal. • To name a binary acid: • 1. Write the roote of the non-metal name • 2. Add the prefix hydro- to the root name. • 3. Add the ending -ic acid to the root name.

  4. Naming Oxoacids • Made of hydrogen, oxygen, and another element. • EG. An oxoacid can form with hydrogen and a polyatomic ion that contains oxygen. • 1. Write the name of the anion, without the -ate or -ide ending. • 2. If the anion name ended in -ate replace it with -ic at the end of the name.

  5. 3. If the anion name ended in -ite, replace it with -ic on the end. • 4. Add the word acid. • Note: acid names for sulfur, use sulfur- instead of just sulf- • Note: acids named with phosphorus, use the root phosphor-

  6. Examples…

  7. Writing the Formula… • 1. Determine if it is a binary or oxo- acid. • If it ends in -ic acid it is a polyatomic ion • If it starts with -hydro, it is a binary acid. • 2. Identify the chemical formula for the polyatomic ion or the ion just by itself • 3. Determine how many H+ ions are needed so the net charge is zero.

  8. Example: carbonic acid. • 1. Ends in -ic so it must be? • Polyatomic (oxoacid) • 2. Chemical formula: • CO3(aq) (2-) • 3. Hydrogen charge = +1, carbonate charge = -2. So the formula is? • H2CO3(aq) • You try it! P. 223 #3, P. 224 #1, 2.

  9. Bases • Most bases are compounds that contain hydroxide ions (OH-) • Bitter taste, slippery feel, can cause bad chemical burns. • Aqueous solutions conduct electricity because when in water, the compound dissociates into the separate ions.

  10. Naming bases • It’s easy! You just use the same method as you would for ionic compounds: • NaOH? • Sodium hydroxide • Formula for aqueous potassium hydroxide? • KOH(aq) • You try it! P. 227 #1, 2. P. 228 #1-8

  11. The pH Scale • Is a scale that ranges from 0 to 14 and is used to classify whether a solution is acidic, basic or neutral. • Acidic: anything below pH of 7. It means there are more H+ ions than OH- ions. The lower the pH, the more acidic it is. • Basic: anything above pH of 7. It means there are more OH- ions than H+ ions. The higher the pH, the more basic it is. • Neutral: when pH = 7.

  12. The concentration of hydrogen ions associates with a value on the pH scale differs from the value above it or below by a power of 10. • pH of 9 is 10 times more basic than a pH of 8. • pH of 3 is 100 times more acidic than a pH of 5. A pH indicator is a substance that changes colour to show the concentration of H+ to OH- ions in a solution.

  13. Types of indicators • EG: Litmus paper: blue litmus paper turns red in acid, red litmus paper turns blue in a base. • Universal: strip of paper that turns a different colour for each pH level. • Methyl orange • Methyl red • Bromothymol blue • Phenophthalein • Indigo carmine

  14. Acid-Base Neutralization • When you mix an acid and base, they can neutralize each other • It forms a salt and water. • EG: HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq) • This is a type of double displacement • Try this! P. 246 # 1, 4. Review: p. 252 # 1 - 16, 18 - 21, 28, 29.

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