Acids and Bases Chapter 19. Arrhenius Acids- hydrogen containing compounds that ionize to yield H + ions in an aqueous solution Begins with H Bases- compounds.

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Presentation transcript:

Acids and Bases Chapter 19

Arrhenius Acids- hydrogen containing compounds that ionize to yield H + ions in an aqueous solution Begins with H Bases- compounds that ionize to yield hydroxide (OH - ) ions in an aqueous solution End in OH

Hydronium Ion Hydrogen ions do not stay present in an aqueous solution Hydrogen bonds to water molecules to form hydronium ions (H 3 O + )

Naming Acids Follow the chart on the back of the periodic table! Naming Bases Name it the same as you would any other ionic compound Will end in hydroxide

Practice H 2 Se Ca(OH) 2 RbOH H 3 P B(OH) 3 HNO 2 H 2 C 4 H 4 O 6

pH Scale Introduced by Danish chemist Soren Sorensen in 1909 “Power of Hydrogen” Logarithmic scale

pH Scale

0-6 is Acidic 7 is Neutral (Pure Water) 8-14 is Basic

Br Ø nsted-Lowry Acid- A hydrogen ion donor Base- A hydrogen ion acceptor

Neutralization Reaction Neutralization: a reaction in which the pH of an acid is raised by combining with a base, or the pH of a base is lowered by combining with an acid; complete neutralization results in a pH of 7

Neutralization Reaction Double replacement reaction Follows the formula: Acid + Base  Water + Salt *Salt means any ionic compound

Example HCl (aq) + NaOH (aq)  H 2 O (l) + NaCl(aq)

Predict and Balance…. 1. ____HBr + ____ NaOH  2. ____H 2 S + ____ Ba(OH) 2  3. ____ H 3 PO 4 + ____ Ca(OH) 2  4. ____ H 2 SO 4 + ____ KOH  5. ____ HNO 3 + ____ NH 4 OH  6. ____ HC 2 H 3 O 2 + ____ AgOH 

Another Review…. How do you solve for molarity?

Solve A volume of a 37 mL of 0.36 M KCN neutralizes a 75 mL sample of HClO solution. What is the concentration of HClO? What volume of 6.0 M HCl is needed to neutralize a 45.0 mL sample of 3.0 M NaOH?

Buffers Buffer- a solution in which the pH remains fairly constant when small amounts of acid or base are added. How do they work? A buffer solution contains components that react with the hydrogen ions and another component that reacts with the hydroxide ions

Buffers Different buffers have different capacities- which is the amount of acid or base that can be added to a buffer solution before a significant pH change occurs.