1. 0.278 g of lead (II) nitrate are dissolved in water to produce 500.0 mL of so

Question

1. 0.278 g of lead (II) nitrate are dissolved in water to produce 500.0 mL of solution. Calculate:

a) Concentration of lead ions in ppm

b) Concentration of nitrate ions in ppt

2. A solution whose concentration of Na+ is 11.0 ppm is prepared by dissolving sodium sulfate in water. Calculate:

a) Analytical (molar) concentration of the solution

b) Species or equilibrium (molar) concentration

3. You are asked to prepare 500.0 mL of each of the following solutions from the reagent indicated. Calculate how much reagent you would need to weigh out in each case.

a) 7.0 parts per thousand K+ from potassium chloride

b) 1.0x102 ppb Zn2+ from zinc nitrate

c) 50.0 ppm Br- from sodium bromide

4. 10.63 g of copper(II) nitrate are dissolved in water to produce 500.0 mL of solution. Calculate:

a) The formal molar concentration of the solution

b) The analytical molar concentration of copper(II) ions

c) The analytical molar concentration of nitrate ions

5. Commercial sulfuric acid is 98.0 wt % sulfuric acid and has a density of 1.8 g mL-1. Calculate the molarity of commercial sulfuric acid.

6. You need to prepare 2.0 L of a 1.00 ppm solution of glucose (C6H12O6) in water.

a) How many grams of glucose do you need to weigh out?

b) What is the molar concentration of the solution?

7. 0.1072 g of potassium iodide are dissolved in water to produce 250.0 mL of solution. What is the

a) concentration of potassium ions in ppm?

b) concentration of iodine ions in ppt?

8. 1.023 g of sodium chloride are dissolved in water to produce 1.0 L of solution. Calculate the concentration of Na+ and Cl- in ppt.

9. 0.671 g of iron (II) nitrate is dissolved in water to make 1500 mL of solution. What is the concentration of NO3- in ppm?

10. 25.0 mL of a 0.1067 M solution of nickel (II) sulfate is diluted to 250 mL with water. 10 mL of this solution is taken and diluted to 1.0 L. Calculate the concentration of [Ni2+] in the final solution in ppm.

11. I need to make up 2.0 L of a solution whose concentration is 1000 ppm K+. How much potassium chloride must I weigh out to make this solution?

12. You need to make up a 10 ppm aqueous solution of a compound 'A'. What weight of 'A' must you weigh out to make the solution.

13. 5.26 g of silver nitrate are dissolevd in water to produce 250mL of solution. Assuming the density of the solution is close to 1.0g/mL, what is:

a) The weight percent of silver nitrate in the solution

b) The weight percent of silver in the solution

c) The weight percent of nitrate in the solution

Explanation / Answer

1. a) 3.48 x 102
ppm
b) 0.208 ppt

2. a) 2.39 x 10-4 M Na2SO4
b) 4.78 x 10-4 M Na
2.39 x 10-4 SO4
2-

3. a) 6.7g KCl
b) 1.4 x 10-4g Zn(NO3)2
c) 3.22 x 10-2g NaBr

4. a) 0.1134 M
b) 0.1134 M
c) 0.2267 M

5. 18M

6. a) 2.0 x 10-3 g
b) 5.6 x 10-6 M

7. a) 101.0 ppm K+

b) 0.3278 ppt I-

8. [Na+] = 0.40 ppt
[Cl-] = 0.62 ppt

9. [NO-3] = 308 ppm

10. [Ni2+] = 6.3 ppm

11. 3.81

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