Exam 2

Question 1

Arrhenius Acid

Answer 1

a compound that increases the concentration of hydrogen ions (H+)

Question 2

Arrhenius base

Answer 2

a compound that increases the concentration of hydroxide ions (OH-)

Question 3

Bronstead-Lowry Acid

Answer 3

a proton (H⁺) donor

Question 4

Bronstead-Lowry Acid

Answer 4

a proton acceptor

Question 5

Lewis Acid

Answer 5

any species that can accept a pair of electrons (Lewis is coordinate covalent bond)

Question 6

Lewis Base

Answer 6

a species that can donate a pair of electrons to an electron acceptor

Question 7

Strong Acids 6

Answer 7

hydrobromic (HBr), hydrochloric (HCl), hydroiodic (HI), nitric (HNO3), perchloric
(HClO4), and sulfuric (H2SO4 )

Question 8

Weak Acids 8

Answer 8

acetic (HC2H3O2), formic (HCOOH), hydrofluoric (HF), hypochlorous (HClO), nitrous
(HNO2), carbonic (H2CO3), oxalic (H2C2O4), and phosphoric (H3PO4)

Question 9

Conjugate acid-base pairs in an acid-base reaction.

Answer 9

two molecules or ions that differ by only one proton (H+) where one acts as an acid by donating the proton, and the other acts as a base by accepting that proton; essentially, they are related by the gain or loss of a single hydrogen ion in a chemical reaction.

Question 10

pH equal pKa when

Answer 10

concentrations are equal

Question 11

pH equation

Answer 11

pH=pka+log [base/acid]
pKa=-log(Ka)
pH=-log[H+]

Question 12

Find Ka from pH

Answer 12

10^-pH

Question 13

To find pH of a mixture of solutions given molarity and volume

Answer 13

Use m1v1… and calculate ph from conventration

Question 14

Relation of Kw and Ka and b

Answer 14

Kw=KaKb

Question 15

Find Ksp

Answer 15

Ksp=[anion][cation]