H+ Ion 6.0

Day 2

 SWBAT utilize experimental data to illustrate and explain the pH Scale to characterize acidic and basic solutions  SWBAT compare and contrast the strengths of various common acids and bases.

Today we will be covering the following topics 1.Acid Base Theory 2.Arrhenius Acids 3.Arrhenius Bases 4.Dissociation of Water 5.Calculating pH 6.H+ concentration

Acid Base Theory:  Acids are substances which produce hydrogen ions in solution.  Bases are substances which produce hydroxide ions in solution.

Arrhenius Acids: a substance that when added to water increases the number of H+ ions in the water. Example: HCl (hydrochloric acid)

Arrhenius Bases: a substance that when added to water increases the number of OH- ions in the water. Example: NaOH (Sodium Hydroxide)

Example of what happens to acids and bases when placed in water

-Dissociation of Water: Water has the ability to split into an H+ ion and an OH- ion. -Water can act like an acid when it donates a H+ ion -Water can act like a base by accepting an OH- ion.

1. HCl - hydrochloric acid 2. HNO 3 - nitric acid 3. H 2 SO 4 - sulfuric acid 4. HBr - hydrobromic acid 5. HI - hydroiodic acid 6. HClO 4 - perchloric acid

1. LiOH - lithium hydroxide 2. NaOH - sodium hydroxide 3. KOH - potassium hydroxide 4. RbOH - rubidium hydroxide 5. CsOH - cesium hydroxide

 As the hydrogen ion concentration INCREASES the pH DECREASES  A change of 1 pH unit means the hydrogen ion concentration changed by a factor of 10

For example, if one solution has a pH of 1 and a second solution has a pH of 2, the first solution is not twice as acidic as the second—the hydrogen ion concentration increased by a factor of ___________. 10

Formula: [H + ] = 10 -pH My Example: Find [H+] if pH = 8.5

Calculate the hydrogen ion concentration of a solution with a pH of 4.5 Answer

Calculate the hydrogen ion concentration of a solution with a pH of 6.8 Answer

Calculate the hydrogen ion concentration of a solution with a pH of 12.2 Answer

Complete the worksheet it will be stamped &collected TODAY Work SMART

1.Give an example of an Arrhenius acid? 2.Give an example of an Arrhenius base? 3.As the pH decreases, the hydrogen ion concentration ___________. 4.What is the H+ concentration of a solution with a pH of 3? 5.Solution A has a pH of 3 and solution Z has a pH of 6. How many times greater is the H+ concentration in solution A than the H+ concentration in solution Z? a.100b.2c.1000d. 3

1.Give an example of an Arrhenius acid? HCl 2.Give an example of an Arrhenius base? NaOH 3.As the pH decreases, the hydrogen ion concentration increases. 4.What is the H+ concentration of a solution with a pH of 3? Solution A has a pH of 3 and solution Z has a pH of 6. How many times greater is the H+ concentration in solution A than the H+ concentration in solution Z? a.100b.2c.1000d. 3

STUDY YOUR NOTES FROM THIS WEEK IN PREPARATION FOR A POSSIBLE QUIZ NEXT WEEK