Acids & Bases Review

Acids & Bases Review

By Leslie Dunham

Water breaks into ions
H₂O --> H⁺ + OH^-

Acids have more H⁺ ions
Bases have more OH^- ions
Neutral have equal amount of both

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Acid or base?

Acids have a pH of less than 7
Other characteristics include sour taste, reacts with metals to form hydrogen gas, conduct electricity

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Characteristics of acids

Acids have a pH of greater than 7
Other characteristics include bitter taste, slippery feeling, conduct electricity

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Characteristics of bases

Multiple Choice

Milk is a very weak acid. What might its pH value be?

• 6.5

• 7.8

• 4.2

• 12.2

Multiple Choice

Which of the following are properties of acids?

• They conduct electricity when dissolved in water

• They taste sour

• They react with metals to produce hydrogen gas

• All of the answer choices are correct

Multiple Choice

Which of the following is a property of a base?

• bitter taste

• reacts with metals

• salty

• sour taste

Multiple Choice

The strongest bases have pH values close to

• 0

• 14

• 7

• 5

Acids release H⁺ in solution
Bases release OH^- in solution

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Arrhenius acids & bases

Acid - a substance that can donate an H⁺ (proton)
Base - a substance that can accept an H⁺ (proton)

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Bronsted Lowry Acid and Base

Conjugate Acid - formed from a base by addition of an H⁺ (proton)
Conjugate Base - formed from an acid by loss of an H⁺ (proton)

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Conjugate acid and base

Multiple Choice

A hydrogen ion, H⁺, is the same as a(n):

• neutron
• electron
• proton
• hydroxide ion

Multiple Choice

According to the Arrhenius theory, an acid is a substance that

• changes litmus from red to blue

• changes phenolphthalein from colorless to pink

• produces hydronium ions as the only positive ions in an aqueous solution

• produces hydroxide ions as the only negative ions in an aqueous solution

Multiple Choice

An arrhenius base

• produces H⁺ ions

• produces OH^- ions

• is insoluble

• has an i of 2

Multiple Choice

A Bronsted Lowry acid:

• donates H+ to another substance

• accepts H+ from another substance

• produces H+

• produces OH-

Multiple Choice

A Bronsted Lowry base:

• donates H+ to another substance

• accepts H+ from another substance

• produces H+

• produces OH-

Multiple Choice

In the equation below, what is the Bronsted Lowry acid (donates H⁺)?

HCl + NH₃ → Cl^- + NH₄⁺

• HCl

• NH₃

• Cl^-

• NH₄⁺

Multiple Choice

In the equation below, what is the Bronsted Lowry base (accepts H⁺)?

HCl + NH₃ → Cl^- + NH₄⁺

• HCl

• NH₃

• Cl^-

• NH₄⁺

Strong acids and bases ionize COMPLETELY in solution
Weak acids and bases DO NOT ionize completely in solution

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Weak vs strong acids & bases

Measure of the strength of acids and bases
pH = power of hydrogen
Determined by concentration of H⁺ ions

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pH scale

Measures strength of OH^-
pH + pOH = 14

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pOH scale

Reactions between an acid and a base that eliminate acid/base properties
Acid + Base --> Salt + H₂O

Always neutralize using a strong acid or base

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Neutralization

Multiple Choice

HBr is a strong acid and HF is a weak acid. Which of the following statements is true?

• HBr would partially dissociate.

• They both have the same pH.

• HBr has a lower pH than HF.

• HBr has a higher pH than HF.

Multiple Choice

The following solution represents a...

• strong acid

• strong base

• weak acid

• weak base

Multiple Choice

The following solution represents a...

• strong acid

• strong base

• weak acid

• weak base

Multiple Choice

Which of the following is the correct definition for a strong acid?

• Partially dissociates into ions when dissolved in water and the change is not reversible

• Fully dissociates into ions when dissolved in water and the change is not reversible

• Fully dissociates into ions when dissolved in water and the change is reversible

• Partially dissociates into ions when dissolved in water and the change is reversible

Multiple Choice

A  pH and a pOH will add up to:

• 0
• 7
• 14
• 1.0 x 10^-14

Multiple Choice

If the pH of a solution is 5.6 the pOH is

• 6.5
• 12.4
• 8.4
• 5.6

Multiple Choice

What are the products to a neutralization reaction?

• H₂ + Ionic Salt
• H₂O + Ionic Salt
• H₃O⁺ + Ionic Salt
• OH^- + Ionic Salt