Acids & Bases

1. Identify each of the following as an Arrhenius acid (a), Arrhenius base (B), or salt (s).

a. NaCl

b. KOH

c. HCl

2.

a. H2O + H2O ↔ H3O+ + OH-

b. H2SO4 + OH- ↔ HSO4- + H2O

c. HSO4- + H2O ↔ SO42- + H3O+

d. OH- + H3O+ ↔ H2O + H2O

e. NH3 + H2O ↔ NH4+ + OH-

In Bronsted-Lowry Acids and Bases we know that after on acid has given up its proton, it is capable of getting back that proton and acting as a base, conjugate base is whatis left after an acid gives up a proton. The stronger the acid, the weaker the conjugate base. The weaker the acid, the strongerthe conjugate base.

3. Fill in the blanks in the table below.

Acid / Base / Equation
a / H2SO4 / HSO4- / H2SO4↔H+ + HSO4-
b / H3PO4
c / F-
d / NO3-
e / H2PO4-
f / H2O
g / SO4-2
h / HPO4-2
i / NH4+
j / H2O

pH and pOH

Since [H+] [OH-] = 10-14 at 25 ˚C, if [H+] is known, the [OH-] can becalculated and vice versa.

pH = - log [H+] So if [H+] = 10-6 M, pH = 6.

pOH = - log [OH-] So if [OH-] = 10-8 M, pOH = 8.

Together,pH + pOH = 14.

4. Fill in the appropriate blanks.

[H+] / pH / [OH-] / pOH / Acidic or Basic
a / 10-5 M / 5 / 10-9 M / 9 / Acidic
b / 7
c / 10-4 M
d / 10-2 M
e / 11
f / 12
g / 10-5 M
h / 10-11 M
i / 13
j / 6

5. Directions: Write the balanced chemical equation for the following neutralization equations. Name the products

a. __H2SO4(aq) + __KOH(aq)  ______

b. ___H3PO4(aq) + ___LiOH(aq)  ______

c. ___H2CO3(aq) + __Mg(OH)2(aq)  ______

d. ___H(C2H3O2)(aq) + __ NaOH(aq) ______

e. __HNO3(aq) + __Ca(OH)2 ______

f. __HBr(aq) + __KOH(aq)  ______