Question

1. A solution that has a relatively large quantity of solute dissolved in the solvent in:

a) Homogenous

b) Dilute

c) Concentrated

d) Saturated

2. The concentration of flouride ions in municipal drinking water cannot exceed 1.5 ppm. What is the maximum mass of flouride ions that can be dissolved in 500 mL of water?

a) 3.0 mg

b) 0.003 mg

c) 750 mg

d) 1.5 mg

e) 0.75 mg

3. As the temperature of a solution increases, the solubility of salts and the solubility of gases

a) doesn't change, doesn't change

b) decreases, decreases

c) increases, decreases

d) increases, increases

4. What is the concentration of chlorine in a 2.0 L sample of pool water that contains 5.2 mg of chlorine?

a) 2.0 ppm

b) 2.6 ppm

c) 3.8 ppm

d) 0.4 ppm

5. According to its Arrhenius definition, a weak base

a) partially reacts with water to form OH - (aq)

b) complete dissociates to forrn OH - (aq)

c) is an ionic hydroxide

d) fully reacts with water to form OH - (aq)

e) has very high pH

6. 25.4 g of a salt was dissolved in 405 ml of distilled water to make 425 mL of solution. What is the percent w/v concentration?

a) 94%

b) 25.4%

c) 4.25%

d) 2.54%

e) 6%

7. Which statement is true if 10.0 g of substance A reacts with 15.0 g of substance 8?

a) Substance A is the limiting reagent.

b) Substance 8 is the limiting reagent.

c) Substance A is the excess reagent.

d) Substance 13 is the excess reagent.

e) not enough inforrnation

 

Answer 1

1) The correct answer is option C. That is, concentrated

2) The correct answer is option e. That is, 0.75 mg

1 ppm =1 mg/litre

Therefore, 1.5 ppm=1.5 mg /l=0.75 mg per 500 l

3) The correct answer is option C. That is, increases, decreases

4) The correct answer is option b. That is 2.6 ppm

1 ppm = 1 mg/l

Therefore, 5.2 mg/l =5.2 ppm

Therefore, 5.2 mg/2 L =2.6 ppm

5) The correct answer is option a. That is, partially reacts with water to form OH - (aq)

6) The correct answer is option e. That is, 6%

Weight by volume=25.4 g*100/425 ml=6%

7) The correct answer is option e. That is, not enough information.