Strength of Acids

​Chart found

on page 739

Multiple Choice

Which acid is stronger?

• HF

  K_a = 6.8 x 10^-4

• HClO

  K_a = 2.9 x 10^-8

Multiple Choice

The H 3 O+ concentrations of three solutions at room temperature are as follows. Which solution is acidic?

• [H₃O⁺] = 1 x 10^-3 M

• [H₃O⁺] = 1 x 10^-7 M

• [H₃O⁺] = 1 x 10^-9 M

​potential of hydrogen or pH

Multiple Choice

As the p H of a solution increases (gets higher), what happens to the acidity of the solution?

• The acidity increases.

• The acidity decreases

• The acidity remains constant.

Multiple Choice

Which pH number below reflects a weak acid?

• 1

• 6

• 8

• 13

Multiple Choice

Which pH number below reflects a weak base?

• 1

• 6

• 8

• 13

Multiple Choice

Which pH number below reflects a strong base?

• 1

• 6

• 8

• 13

Multiple Choice

Which pH number below reflects a strong acid?

• 1

• 6

• 8

• 13

Multiple Choice

Mixing equal portions of an acid and a base should give us a mixture with a pH near

• 3

• 10

• 7

• 0

Multiple Choice

pH stands for:

• Potency of hydrogen

• Plurality of hydrogen

• Potential of hydrogen

• Pleurisy of hydrogen

Multiple Choice

Pure water is _______ on the pH scale.

• Acid

• Base

• Neutral

Multiple Choice

What is the range of pH values in an alkali (basic) solution?

• 0-6

• 8-14

• 15-239058204958

• pH = 7

Multiple Choice

Which is the stronger acid?

• pH 1

• pH 4

• pH 8

• pH 13

Multiple Choice

Which of the following substances is basic?

• Apple juice

• Ginger ale

• Baking soda

• Distilled water

Multiple Choice

True or false: bases are sometimes called alkaline.

• True

• False

Multiple Choice

The ion that every acid donates

• Hydrogen ions

• Hydroxide ions

• Hydrogen atoms

• Hydrogen molecules

Multiple Choice

The ion that every alkali donates.

• Hydrogen ions

• Hydroxide ions

• Hydroxide atoms

• water

Multiple Choice

A chemical dye that can be added to a substance that changes colour depending on whether the substance is acidic, neutral or alkaline.

• A poison

• An alkali

• An acid

• An indictor

Multiple Choice

A measure of the acidity of a substance. It identifies if a substance is acidic, neutral or alkaline.

• Ph scale

• table of ions

• periodic table

• pH scale

Multiple Choice

A substance that dissolves in water.

• acids

• insoluble salts

• soluble salts

• alkalis

Multiple Choice

An acid that fully dissociates in solution to produce a high concentration of hydrogen ions.

• a weak acid

• a strong acid

• a weak alkali

• a strong alkali

Multiple Choice

An acid that only partially dissociates in solution forming only a low concentration of hydrogen ions.

• a strong acid

• a strong alkali

• a weak acid

• a weak alkali

Multiple Choice

The pH scale is a range from:

• 1-7

• 0-14

• 1-14

• 1-20

Multiple Choice

A(n) ______ is a substance with a pH less than 7

• Acid

• Alkaline

• Base

• Buffer

Multiple Choice

A(n) _______ is a substance with a pH greater than 7.

• Base

• Acid

• Buffer

• Water

Multiple Choice

Which solution releases H+ in solution?

• Base

• Acid

• Buffer

• Water

Multiple Choice

This substance releases OH- into solution

• Acid

• Base

• Neutral

Multiple Choice

The pH of a solution is 8.43. What is the hydroxide ion OH^- concentration?

• 3.7 x 10^-9 M

• 2.7 x 10^-6 M

• antilog (-pH)

• 1.0 x 10^-14/-pH

Multiple Choice

What is the pH of a solution with a hydrogen ion concentration of 6.2 x 10^-5?

• 5

• 4.2

• 1.6

• 10.9

Multiple Choice

Hydrogen ion concentration is also written as:

• [H₂O]

• [H₃O⁺]

• [OH^-]

• [H⁺]

Multiple Choice

What is the concentration of H⁺ in a solution with a pH of 3?

• 1.0 x 10^-3

• 3.0 M

• 10.3 M

• 10³ M

Multiple Choice

Which of the following is the hydrogen ion concentration of an acid?

• 9.2 x 10^-14

• 2.4 x 10^-7

• 1.0 x 10^-8

• 5.7 x 10^-11

Multiple Choice

Which of the following is the [H⁺] concentration of a base?

• 9.2 x 10^-3

• 8.3 x 10^-6

• 3.4 x 10^-9

• 1.7 x 10^-7

Multiple Choice

Which of the following is the [H⁺] concentration of a base?

• 9.2 x 10^-3

• 8.3 x 10^-6

• 3.4 x 10^-9

• 1.7 x 10^-7

Multiple Choice

If [OH-] = 1 x 10^-4 M, what is the pH of the solution?

• -4

• 10

• 4

• -10

Multiple Choice

What is the [OH^-] of a solution whose pH = 5.43 ?

*K_w = [H+][OH-] or 1.0 x 10^-14*

• 8.57

• 2.69 x 10^-9 M

• 3.72 x 10^-6 M

• 269153

Multiple Choice

A certain solution has a pH of 1.93. Calculate its [H⁺] and [OH⁻].

• [H⁺] = 1.2 x 10 ^-2 M ; [OH⁻] = 8.3 x 10 ^-13 M

• [H⁺] = 1.2 x 10 ² M ; [OH⁻] = 8.3 x 10 ¹³ M

• [H⁺] = 8.3 x 10 ¹³ M ; [OH⁻] = 1.2 x 10 ² M

• [H⁺] = 8.3 x 10 ^-13 M ; [OH⁻] = 1.2 x 10 ^-2 M

Multiple Choice

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

• 4.60

• 5.0

• 2.5

• 7

Multiple Choice

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

• -1.14

• 2.0

• 1.14

• 7.3

Multiple Choice

What is the [H+] if the pH is 4.0?

• 1.0 x 10-10  M

• 1.0 x 10-4  M

• 1.0 x 10-14  M

• 1.0 x 10-7  M

Multiple Choice

What is the pOH of a solution that has a pH of 2?

• 10

• 12

• 14

• 1

Multiple Choice

What is the [OH-] if the pH is 4.9?

• 7.94 x 10-10 M

• 1.0 x 10-4  M

• 7.94 x 10-14 M

• 4.9 x 10-10 M

Multiple Choice

For a solution, pH + pOH =

• 7

• 1.0 x 10^-14

• -log (1.0 x 10 ^-14)

• 14

Multiple Choice

If the [H₃O⁺] of a solution is 9.3 x 10^-3 M, the pOH of the solution will be

• 2.03

• 11.97

• 1.02

• 12.98