Module 7

Question 1

pH =

Answer 1

-log ([H₃O+])

Question 2

K_w =

Answer 2

[H3O+] • [OH-] = 1 X 10-14 M²

Question 3

the value of the water ionization constant is exact;

Answer 3

Thus you can treat it as if it has an infinite number of significant figures.

Question 4

pOH =

Answer 4

-log ([OH^-])

Question 5

pH + pOH =

Answer 5

14

This 14 is exact for sig fig purposes

Question 6

HCl

Answer 6

Hydrochloric Acid

Question 7

HBr

Answer 7

Hydrobromic acid

Question 8

HI

Answer 8

Hydrogen Iodide

Question 9

HNO₃

Answer 9

Nitric Acid

Question 10

HClO₄

Answer 10

perchloric acid

Question 11

H₂SO₄

Answer 11

Sulferic Acid

Question 12

If an amphiprotic substance is in the presence of an acid that is stronger than its own acid srengh, the amphiprotic substance

Answer 12

acts as a base. If it is in the presence of a base that is stronger than its own base strength, it acts as an acid.

Question 13

Ka • Kb =

Answer 13

K_w

Only for a conjugate acid base pair.

Question 14

When a strong acid or a strong base is used, the reaction will usually be

Answer 14

a complete reaction. When both the acid and base are weak, the reaction will usually be an equilibrium.

Question 15

If an acid is strong, its conjugate base is weak. If an acid it weak, its conjugate base is strong.

Answer 15

If a base is strong, its conjugate acid is weak. If a base is weak, its conjugate acid is strong.

Question 16

When the conjugate of a diprotic or triprotic weak acid is 20 or more times weaker than the original acid,

Answer 16

you need not consider it when calculating pH.

Question 17

Arrhenius definition of acids and bases

Answer 17

An acid is any substance that increases the concentration of H₃0+ in water, and a base is any substance that increases the OH- concentration of water.

Question 18

Lewis definition of Acids and Bases

Answer 18

Acids are substances that accept a lone pair of electrons, while bases are substances that donate a lone pair of electrons.