Acid/Base
Solubility
Electrochemistry
Kinetics
100

Name four strong acids.

HCl, HI, HBr, HClO4, HNO3, H2SO4

100
The Ksp expression for solubility of AgCl

Ksp = [Ag+][Cl-]

100

Compare a Galvanic cell and an electrolytic cell.

Galvanic cell - spontaneous. Electrolytic - not spontaneous

100

How do you find the reaction order from order of the reactants?

Sum the exponents of the reactants in the rate law.

200

Order the acid/base definitions from most general to most specific.

Lewis, Bronsted-Lowry, Arrhenius

200

Which way does solubility equilibrium shift during formation of a complex ion. How does this affect molar solubility?

Shifts right, increases solubility

200

If a metal is ______ on the activity series, it is more likely to be oxidized.

Higher

200

What is the unit for k in a 2nd order reaction?

1/M*time

300

Calculate the pH of 6.50 x 10-3 M KOH solution.

pOH = -log[OH-] = -log(6.50 x 10-3) = 2.187
pH = 14.000 – pOH = 14.000 – 2.187 = 11.813

300

Determine whether PbF2 would be more soluble in acidic solution

Yes, it contains a basic anion

300

How do you know which half reactions go in the anode/cathode?

Oxidation goes in the anode, reduction goes in the cathode

300

What is the integrated rate law for a 1st order reaction?

ln[A]t = -kt + ln[A]0

400

How does adding sodium acetate CH3COONa affect the pH of a solution?

Increases pH (makes it more basic)

400

Write the equation to calculate the solubility of PbCl2 in pure water. Ksp PbCl2 = 1.7 x 10-5

Ksp = (s)(2s)2 → s = 0.0162 M.

400

In a Galvanic cell containing copper and zinc, write and balance the two half reactions.

Zn (s) --> Zn2+ (aq) + 2e-

Cu 2+ (aq) + 2e- --> Cu (s)

400

The activation energy of a reaction is 56.80 kJ/mol and the frequency factor is 1.5 x 1011 /s. Calculate the rate constant at 25 Celsius.

K = Ae-Ea/RT = (1.5E11) *e-56.8 kJ/mol*1000 J/kJ / 8.314J*298.15K = 17/3

500

Titrate 25.0 mL of 0.100 M CH3COOH with 0.100 M NaOH (at 25 °C). Ka(CH3OOH) = 1.80 × 10–5. What is the pH after 30.0 mL NaOH is added?

CH3COOH: .025L * .1M = .0025 mols

NaOH: .03L * 0.1M = .003 mols

After eq point

.055L total volume

.0005  mol base

[OH-] = mol base/ V = .0005 mol base/.055L = .0091 M

pH = 14 +log ([OH-]-[HA])

pH = 14 + log ([0.0091]) = 11.96 

500

Write the equation to calculate the solubility of PbCl2 in 0.25 M MgCl2. Ksp PbCl2 = 1.7 x 10-5

Ksp = (s)(0.50 + 2s)2 →  6.80 E-5.

500

Calculate the equilibrium constant for a Zn/Cu cell at standard conditions. Reduction of copper: 0.34 V. Reduction of Zinc: -0.76 V anode

Zn (s) → Zn2+ (aq) + 2e- 0.76

Cu2+ (aq) + 2e- → Cu (s) 0.34

Zn (s) + Cu2+ (aq) → Cu (s) + Zn2+ (aq) = 1.1 V 

E standard cell = 0.0592/n * logK

1.1  = 0.0592/2 * logK

1.45 x 1037 = K 

500

For the reaction 2NO (g) + O2 (g) --> 2NO2 (g) with rate = k[NO]2[O2], explain why the following mechanism does not work.

1. 2NO (g) --> N2O2 (g) slow

2. N2O2 (g) + O2 (g) --> 2NO2 (g) fast


Rate law based on slow step is rate = k[NO]2, which does not match experimental rate law.

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