practice quiz

practice quiz

The following equations might be useful:
The following equations will be given:
pH = -log [H+] pOH = -log [OH-] 14.00 = pH + pOH
[H+] = antilog(pH) or 10-pH [OH-] = antilog(pOH) or 10-pOH Kw = [H+][OH–]= 1.0 x 10-14
Kw = Ka Kb for conj. pair
\textrm{pH} = \textrm{pK}_{a}+ \log \left ( \frac{[\textrm{A}^-]}{[\textrm{HA}]} \right )\textrm{pH} = \textrm{pK}_{a}-\log \left ( \frac{[\textrm{HA}]}{[\textrm{A}^-]} \right ).Weak acids in water: Ka = [H+][A-] / [HA]init Weak bases in water: Kb = [-OH] [BaseH] /[Base]init % ionization = [H+] / [HA]init x 100 % % ionization = [A-] / [HA]init x 100 %

1. Be able to apply differences between Arrhenius, Bronsted-Lowry, and Lewis definitions for acids and
bases to species in a chemical equation.
2. Choose the correct pair that represents conjugates
3. Determine strength of acids
4. Determine acidity of salts
5. Identify the type of acid: monoprotic, diprotic, polyprotic, hydrohalic, oxyacid, carboxylic.
6. Amphoteric and autoionization properties of water. Be able to calculate Kw, [H+] or [OH-].
7. Be able to interconvert between pH, pOH, [H+] or [OH-] 8. Be able to interconvert between pH, pOH, [H+] or [OH-] 9. Be able to interconvert between pH, pOH, [H+] or [OH-] 10. Strong acids and bases. Be able to calculate ion concentrations given equation and Ka, Kb.
11. Weak acids and weak bases. Be able to calculate ion concentrations given equation and Ka, Kb.
12. Percent ionization problem.

Practice Quiz Section: Please show all work for full credit on this assignment.

1. Choose the Bronsted-Lowry acids and bases in the following equation:

H2O + NH2- ßà NH3 + OH-
2. Write the conjugate acid for a-e and the conjugate base for f-j.
a. Cl- b. OCl- c. SO42- d. OH- e. NH3

f. HClO4 g. HClO2 h. H2SO42- i. H3O+ j. H2PO3-

3. a. Identify the strongest acid.
a) HCN b) HNO3 c) H2O d) OH– e) CH3OH
b. Identify the strongest base.
a) CH3O– b) CH3OH c) CN– d) H2O e) NO3–

4. For each of the following compounds, predict whether the solution is acidic, basic or neutral and why.

a. NH4Cl b. NaC2H3O2 c. NaCl d. AlCl3 e. KCN

5. Identify each type of acid.

a. HBr b. HBrO3 c. CH3CH2COOH d. H2PO4- e. H3PO4

6. Calculate the [OH-] or [H+] for each solution and determine if it is acidic, basic, or neutral.

a. 3 x 10-9 M OH- b. 6.6 x 10-10 M OH- c. 4.1 x 10-10 M H+

d. 2.4 x 10-10 M OH- e. 6.2 x 10-8 M H+ f. 4.1 x 10-6 M H+

7. Calculate the [H+] in a solution at 25°C for the following:
a. pH = 4.32 b. pH = 1.02 c. pH = 13.1 d. pH = 5.93 e. pH = 4.11

8. Calculate the pOH of the following OH- solutions at 25°C.

a. 6.03 x 10-11 M b. 2.57 x 10-11 M c. 6.46 x 10-4 M d. 4.88 x 10-6 M e. 2.88 x 10-6 M
9. Calculate the pH for each of the following OH– solutions at 25°C
a. 1.9 x 10-12 M b. 2.1 x 10-4 M c. 3.02 x 10-3 M d. 1.35 x 10-9 M e. 1.15 x 10-10 M

10. Calculate the pH of 0.208 M HNO3(aq).

11. What is the pH of a 0.375 M solution of benzoic acid? Ka = 6.3 × 10-5

12. A solution of 8.00 M formic acid (HCOOH) is 0.47% ionized. What is the Ka value of formic acid?

FOR YOUR ASSIGNMENTS TO BE DONE AT A CHEAPER PRICE PLACE THIS ORDER OR A SIMILAR ORDER WITH US NOW