Name:__________________________________

Lab: M W

Chem2A Exam 3Monday December 12, 2016

Pg1 _________Pg2 _________Pg3 _________Pg4 _________Pg5 _________Pg6 _________Pg7__________Pg8__________Pg9__________

Total ________/100

1. Increasing the temperature of a reaction:a. Increases the number of collisionsb. Increases the average kinetic energyc. Decreases the Ea

d. a and b

2. Increasing the concentration of a reaction:a. Increases the number of collisionsb. Increases the average kinetic energyc. Decreases the Ea

d. a and b

3. Adding a catalyst to the reaction:a. Increases the number of collisionsb. Increases the average kinetic energyc. Decreases the Ea

d. a and b

4. Which of the following species can be Bronsted-Lowry acids?

a. H2Ob. I-

c. HOCld. FeBr3

e. CH3CH2COOHf. CO2

5. Which of the following species can be a Bronsted-Lowry base?

a. Cl-

b. BH3

c. H2Od. Na+

e. Ca(OH)2

f. HCOO-

6. Which mixture has the largest particle size?a. Solutionb. Colloidc. Suspension

7. Which mixture has the smallest particle size?a. Solutionb. Colloidc. Suspension

8. When the bonds of the products are stronger than the bonds of the reactants, enthalpy of the reaction is:

a. Positiveb. Negativec. Zerod. >> 1

9. When K is around 1 (0.01 < K < 100)a. Concentration of products is greater than reactantsb. Concentration of reactants is greater than productsc. Both products and reactants are equal in concentrationd. Doesn’t tell you anything about concentration

10. If a reaction is at equilibrium and you add more reactants, the reaction:

a. Favors Productsb. Favors reactantsc. Has no effect on the reaction

11. If a reaction is at equilibrium and you constantly remove products, the reaction:

a. Favors Productsb. Favors reactantsc. Has no effect on the reaction

12. If a reaction is at equilibrium and you increase the pressure, the reaction:

a. Favors the side with fewer molesb. Favors the side with more molesc. Has no effect on the reaction

13. For the following reaction:H2(g) + I2(g) 2 HI(g)

a. Write the expression for the equilibrium constant:

_______________________

b. Calculate K using the following concentrations: [H2] = 0.95 M, [I2] = 0.78M, and [HI] = 0.27M

_______________________

14. If a solution contains 132 mEq/L of Na+, how many mEq of Na+ are present in the following volumes of solution?

a. 1.0L_________________

b. 2.0L_________________

c. 440mL_________________

15. Which of the following compounds are soluble in water?

a. Al(NO3)3

b. NaHCO3

c. Cr(OH)3

d. LiOHe. CuCO3

f. (NH4)2SO4

g. Fe(OH)3

16. How is the solubility of liquid ethanol in water affected by each of the following changes?

a. Increasing the temperature ______________________

b. Decreasing the temperature______________________

c. Increasing the pressure ________________________

d. Decreasing the pressure________________________

17. A glucose solution is isotonic when it contains 5% (w/v) glucose in water. Answer the following questions.

a. If you added a glucose solution that contained 5% (w/v) glucose would blood cells: Swell / Shrink / Maintain Shape

b. If you added a glucose solution that contained 0.01% (w/v) glucose would blood cells: Swell / Shrink / Maintain Shape

c. If you added a glucose solution that contained 50% (w/v) glucose would blood cells: Swell / Shrink / Maintain Shape

18. What is the weight/volume percent concentration using the given amount of solute and total volume of solution?

a. 10.0g of LiCl in 750mL of solution ________________

b. 25g of NaNO3 in 250mL of solution________________

c. 40.0g of NaOH in 500mL of solution_______________

19. Given the following (w/v) % or M, how many grams of solute are contained in a 250mL solution of

a. 4.8% (w/v) acetic acid in water ___________________

b. 22% (v/v) ethanol in water___________________

c. 2.5 M NaCl solution_________________________

20. How many milliliters of a 2.5 M sucrose solution would be needed to prepare each solution?

a. 25 mL of a 1.0 M solution___________________

b. 1.5 L of a 0.75 M solution___________________

c. 250 mL of a 0.025 M solution__________________

21.Write the conjugate base of each acid

a. H3O+ __________________

b. H2Se ___________________

c. HSO4- ___________________

d. H2O ___________________

22. Label the conjugate acid-base pairs in each equation

a. Cl- + H2SO4- HCl + SO4

2-

b. HPO42- + OH- PO4

3- + H2O

c. NH3 + HF NH4+ + F-

23.Label the stronger acid in each pair. Which acid has the stronger conjugate base?

a. HPO42- or HCN

i. Stronger acid _______________ii. Stronger Conjugate Base_____________

b. HSO4- or NH4

+

i. Stronger acid _______________ii. Stronger Conjugate Base_____________

c. H2O or HFi. Stronger acid _______________

ii. Stronger Conjugate Base_____________

24.Fill in the missing terms (strong or weak) and formulas in the following table.

Acid Formula Conjugate Base Formula

a Strong HI

b HCN Strong

c HBr Weak -

d Weak HCO2-

25.Fill in the missing terms (strong or weak) and formulas in the following table.

Base Formula Conjugate Acid Formula

a Strong -OH

b Strong H3O+

c CN- Weak

d Weak HClO4

26.Calculate the value of [-OH] from the given [H3O+] and label the solution as acidic, basic, or neutral

a. [H3O+] = 1x10-1 c. [H3O+] = 2.6x10-7

[-OH] ____________ [-OH] ____________Acidic / Basic / Neutral Acidic / Basic / Neutral

b. [H3O+] = 1x10--13 d. [H3O+] = 1.2x10-12 [-OH] ____________ [-OH] ____________Acidic / Basic / Neutral Acidic / Basic / Neutral

27. Calculate the pH of the solutions with the following [H3O+] and label them as acidic or neutral or basic

a. 1x10-2 Mi. pH ____

ii. Acidic / Basic / Neutral

b. 1x10-8

i. pH ____ii. Acidic / Basic / Neutral

c. 6.2x10-7

i. pH ____ii. Acidic / Basic / Neutral

d. 8.5x10-13

i. pH ____ii. Acidic / Basic / Neutral

28. Complete the following table with the needed [H3O+], [-OH], and pH, and classify the solution as acidic, basic, or neutral

[H3O+] [-OH] pH Classification

5.3x10-3

2.0x10-8

4.4

6.8x10-10

K = [Products] Ka = [H3O - ][OH - ] pH = -log ([H3O+]) [Reactants] [H2O]2

Kw = [H3O+] [OH-] = 1x10-14 M 10-pH = [H3O+]

[H3O+] = [OH-] = 1x10-7 M