Unit 5 Review Notes #18-21

Groups Group 1: Sophia, Evan, Mac Group 2: Brandon, Hunter, Harrison Group 3: Haley, Chase, Nick Group 4: Brooks, Austin, Nathan Group 5: Amanda, Blake, Patrick Group 6: Parker, Matt, Drew, Madison Groups

Directions Every group participates in every question. Each question is timed. You can “re-do” your answer as long as it fits into the time limit. Your answer must be written on a piece of paper. Winning group gets extra credit on test. Directions

1 Point 1 Extra Define Acid and Base using Arrhenius’ definition. Extra: Give one example of an Arrhenius acid and one example of a Arrhenius base. 1 Point 1 Extra

2 Points Define acids and bases using 1) Bronsted Lowry definition and 2)Lewis definition 2 Points

For the following reaction, identify the acid and base using bronsted lowry definition: HNO3 + H2O  H3O+ + NO3- 2 Points

For the following reaction, identify the conjugate acid and base using the standard notation. (Connecting using lines) HNO3 + H2O  H3O+ + NO3- 2 Points

What does Kw mean? 1 point

What are the concentrations of [H+] and [OH-] of pure water (At room temp)? HINT: Why is water neutral? 1 Point

T/F If the [H+] is greater than 1.0 x 10-7, the solution is basic. YOU NEED TO MEMORIZE THESE 1 point

[H+] < 1.0 x 10-7 = basic [H+] > 1.0 x 10-7 = acidic MEMORIZE

Is this solution acidic or basic? [OH-] = 3.5 x 10-10 2 Points

What is the hydrogen ion concentration of a solution with the pH of 5 2 points

What is the hydroxide ion concentration of a solution with a pH of 9.5? 3 Points

Why do weak acids have a small Ka compared to strong acids Why do weak acids have a small Ka compared to strong acids. Use the equation to explain your answer. 1 Point

When a 1.5M solution of benzoic acid partially ionizes , the concentration of hydrogen ions at equilibrium is [H+] = 4.6 x 10-2 M. What is the Ka for this weak acid? 3 Points

Predict the products of this neutralization reaction and balance it: H2SO4 + LiOH  H+1 , SO4-2 , Li+1 , OH-1 2 Points

3 Points Using the previous equation… H2SO4 + LiOH  What is the molarity of lithium hydroxide if 15 mL of lithium hydroxide is neutralized by 17.6 mL of 2M sulfuric acid? 3 Points

3 Points Using Bronsted Lowry Definition: 1) What is the conjugate base of H2SO4? 2) What is the conjugate acid of H2O? 3) What is the conjugate acid of NO3-? 3 Points

When dealing with acid base reactions, why is water unlike any other acid or base? 1 Point

Calculate the pH of a solution with a hydrogen ion concentration of [H+] = 2.2 x 10-4. 2 Points

Calculate the pH of a solution that contains a hydroxide ion concentration of [OH-] = 1 x 10-4 2 Points

What is a buffer? 1 Point

How could you create a buffer solution? 1 Point

T/F Buffers are always neutral (pH=7). Explain why or why not 1 Point

Describe one application of acid base chemistry in the real world (outside of the classroom). 2 Points