Acid/Base Unit Review

Acid/Base Unit Review

Topics to Know for the Exam

• pH scale (how to read, what the scale is based on)

• Calculate pH, pOH, H⁺ and OH^- concentration

• Identify Acids, Bases, Conjugate Acids, and Conjugate Bases

• Use ICE Tables to calculate the pH of a solution

• Use Titrations to determine the concentration or volume of a solution

pH Scale

Multiple Choice

A substance is described as a strong base. Which of the following is the most likely pH?

• 3

• 1

• 11

• 13

Multiple Choice

Which of the following graphs best represents pH?

Multiple Choice

The function for pH is 1/10^x. Using this formula, choose the best explanation for pH.

• As the H+ concentration increases, the pH increases

• As the H+ concentration decreases, the pH decreases

• As the H+ concentration increases, the pH decreases

• As the H+ concentration increases, the pH remains constant

Multiple Choice

Solutions that have many free H+ ions would be described as...

• Acidic

• Basic

• Neutral

• Tasty

Multiple Choice

Which of the following terms is not interchangeable?

• Hydrogen ion

• Proton

• H₃O⁺(Hydronium)

• Hydroxide ion

Identifying Acids and Bases

Multiple Choice

What is the easiest way to identify an acid?

• It will typically have one or more hydrogen at the front

• It will typically have one or more hydrogen at the end

• It will typically have one or more hydroxide at the front

• It will typically have one or more hydroxide at the end

Multiple Choice

A Bronsted Lowry Base is a compound that....

• Donates a proton

• Accepts a proton

• Donates a hydroxide ion

• Accepts a hydroxide ion

Multiple Choice

The Bronsted Lowry Base, PO₄^-3 accepts two protons. Identify the molecule that will be produced.

• H₂PO₄^-3

• H₂PO₄^-1

• H₂PO₄^-2

• H₂PO₄

Multiple Choice

Identify the Bronsted Lowry Acid in the reaction below:

H₂PO₄^-1 + H₂O -> H₃PO₄ + OH^-

• H₂PO₄^-1

• H₂O

• H₃PO₄

• OH^-

Calculating pH, pOH, [H⁺], [OH^-]

Multiple Choice

Calculate the pH of a solution with a .014M H⁺ concentration.

• pH = 1.85

• pH = .014

• pH = 12.15

• pH = 5.82

Multiple Choice

A solution is found to have a pH of 5.4. Calculate the [H+].

• [H+] = 4M

• [H+] = 3.98 x 10^-6M

• [H+] = 4 x 10⁶M

• [H+] = 8.2M

Multiple Select

Which of the following can be used to calculate pOH?

• pH

• [H⁺]

• [OH^-]

• Knowing whether it is strong or weak.

Multiple Choice

A solution with an [H⁺] concentration of .00000003M can be described as...

• A weak base

• A strong base

• A weak acid

• A strong acid

Titrations

Multiple Choice

In our titration formula, where can the value for "n" be found?

• By calculating the volume of the base

• By checking the balanced reaction

• By calculating the concentration of the acid

• The value for "n" will always be given.

Multiple Choice

100ml of NaOH are required to neutralize 40ml of .25M HCl. Calculate the concentration of the NaOH.

• .1M

• 10M

• .75M

• 2M

Multiple Choice

35ml of HCl are required to neutralize 86ml of NaOH. What can be said about this scenario?

• The acid is stronger than the base

• The base is stronger than the acid

• The acid and base are equal concentrations

• There is not enough information to draw a conclusion.

Multiple Choice

What volume of .25M KOH will be needed to neutralize 50ml of .5M H₂SO₄?

• 200ml

• 25ml

• 50ml

• 100ml

ICE Tables

Multiple Choice

How will the concentration of the conjugate acid and conjugate base change throughout the course of a reaction?

• They will increase by X

• They will decrease by X

• They will remain constant

• They will increase initially, but then decrease

Multiple Choice

Calculate the pH of a .003M hydrocyanic acid solution.

• pH = 5.91

• pH = 3.27

• pH = 8.44

• pH = 11.39