What is the mass % of a solution prepared by dissolving 50.0 g NaCl in 150.0 g of water?

1. What is the mass % of a solution prepared by dissolving 50.0 g NaCl in 150.0 g of water?

25.0%

33.3%

0.250%

3.00%

40.0%

2. The molarity (M) of a solution refers to 

grams of solute/100 mL of solution.

moles of solute/L of solvent.

grams of solute/L of solution.

moles of solute/L of solution.

moles of solute/100 mL of solution.

3. What is the molarity , M, of a solution containing 5.00 moles of KCl in 2.00 L of solution?

2.50 M

0.400 M

5.00 M

10.0 M

none

4. How many moles of CaCl2  are in 250. mL of a 3.00 M of CaCl2 solution?

750. mol

1.33 mol

83.3 mol

0.750 mol

none

5. How many mL of 1.15 M KOH solution are needed to provide 0.665 moles of KOH? 

1.73 mL

173 mL

578 mL

764 mL

none

6. How many grams of sodium chloride are required to make 2.00 L of a solution with a concentration of 0.100 M?

0.0200 g

5.85 g

58.5 g

11.7 g

0.200 g

7. What volume of a 2.00 M solution of sulfuric acid is needed to prepare 50.0 mL of a 0.100 M solution by dilution?

2.50 mL

0.0250 L

1.00 mL

2.00 mL

none

8. What is the molarity, M of 25.00 mL of a KOH solution that reacts with with 47.70 mL of a 0.250 M solution of Al2(SO4)3 according to the equation below: Be sure to include the balanced equation step in your calculation.

 Al2(SO4)3  + 6 KOH → 2 Al(OH)3 + 3 K2SO4

0.131 M

6.00 M

0.477 M

2.86 M

none

9. How many grams of aluminum oxide are required to react completely with 75.0 mL of 3.00 M HCl according to the equation:

Al2O3  + 6 HCl → 2 AlCl3 + 3 H2O        Be sure to include the balanced equation step in your calculation.

.0375

3.82

22.9

225

none

10. According to the Bronsted-Lowry definition,

an acid is a proton acceptor.

an acid produces H+  in aqueous solutions.

an acid is a proton donor.

an acid has a low pH

an acid acts as the solvent.

11. Hydroflouric acid is a weak acid because

it is a dilute solution.

it is completely ionized in aqueous solution.

it cannot hold on to its H+ ions

it produces only few H+   ions in water, since it does not completely ionize

it is only slightly soluble in water.

12. In water solution (an aqueous solution), the conjugate base of HF is __________.

H+

H2O

H2

F

OH

13. An acid and base react to form a salt and water in a(n) __________ reaction.

oxidation

reduction

dissociation

ionization

neutralization

14. Which of the following is a neutralization (acid-base) reaction?

KCl + NaNO3 → KNO3 + NaCl

HNO3 + KOH → H2O + KNO3

H2O + SO3 → H2O4

4Na + O2 → 2Na2O

2NO2 → 2NO + O2

15. How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl according to: Ba(OH)2 + 2 HCl reacting completely?  Be sure to use the balanced equation for your calculation,  only the reactants are needed (and given above).

100. mL

50.0 mL

25.0 mL

0.250 mL

0.50 mL

16. For Kw, the product of [H3O+] and [OH-] is __________.  

(Recall H3O+ is the "formal" name for H+ and they are used interchangeably)

1 × 10-14

1 × 10-7

1 × 10-1

1

1 × 1014

17. What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-6 M?

1.0 × 10-2 M

1.0 × 10-6 M

1.0 × 10-8 M

1.0 × 10-10 M

1.0 × 10-12 M

18. A solution with a pH of 4 is

extremely acidic.

moderately acidic.

slightly basic.

extremely basic.

neutral.

19. What is the pH of a solution with [H+] = 1.0 × 10-9 M?

(Recall H3O+ is the "formal" name for H+ and they are used interchangeably)

1.0 × 10-5

-9.0

5.0

-5.0

9.0

20. Calculate the pH of a solution of potassium hydroxide, KOH, with [OH-] of 0.05 M.

1.3

13.5

5.0

12.7

9.0