Calculation in AC

SIH 1005
1. Calculate the weight of one mole of CaSO4 · 7H2O.

2. Calculate the number of moles in 500 mg Na2WO4 (sodium tungstate).
3. What is the weight, in milligrams, of 0.250 mmol Fe 2O3 (ferric oxide)?
4. A solution is prepared by dissolving 1.26 g AgNO3 in a 250-mL volumetric flask and
diluting to volume. Calculate the molarity of the silver nitrate solution. How many
millimoles AgNO3 were dissolved?
5. Calculate the concentration of potassium ion in grams per liter after mixing 100 mL of
0.250 M KCl and 200 mL of 0.100 M K2SO4.
6. How many milliliters of concentrated sulfuric acid, 94.0% (g/100 g solution), density
1.831 g/cm3, are required to prepare 1 liter of a 0.100 M solution?
7. You wish to prepare 500 mL of a 0.100 M K2Cr2O7 solution from a 0.250 M solution.
What volume of the 0.250 M solution must be diluted to 500 mL?
8. What volume of 0.40 M Ba(OH)2 must be added to 50 mL of 0.30 M NaOH to give a
solution 0.50 M in OH−?
9. How many grams per milliliter of NaCl are contained in a 0.250 M solution?
10. A 2.6 g sample of plant tissue was analyzed and found to contain 3.6 μg zinc. What is
the concentration of zinc in the plant in ppm? In ppb?
11. (a) Calculate the molar concentrations of 1 mg/L (1.00 ppm) solutions each of Li+ and
Pb2+. (b) What weight of Pb(NO3)2 will have to be dissolved in 1 liter of water to
prepare a 100 mg/L (100 ppm) Pb2+ solution?
12. What is the molarity of a solution that contains 4.53 moles of lithium nitrate in 2.85 L
of solution?
13. What is the molarity of a solution that contains 0.00372 moles hydrochloric acid in
2.39 x 10-2 L of solution?
14. A flask contains 85.5 g C12H22O11 (sucrose) in 1.00 L of solution. What is the molarity?
15. A beaker contains 214.2 g osmium (III) fluoride in 0.0673 L of solution. What is the
molarity?
16. Calculate the molarity if a flask contains 1.54 moles potassium sulfate in 125 ml of
solution.
17. A chalice contains 36.45 g ammonium chlorite in 2.36 L of solution - calculate the
molarity.
18. What is the molarity of a solution that contains 14.92 g magnesium oxalate in 3.65 ml
of solution?
19. What mass of lithium phosphate would you mass to make 2.5 L of 1.06 M lithium
phosphate solution?
20. If you evaporated 250 mL of a 3.5 M solution of iron (II) nitrite, what mass of iron (II)
nitrite would you recover?
21. A chemist has 4.0 g of silver nitrate and needs to prepare 2.0 L of a 0.010 M
solution. Will there be enough silver nitrate? If so, how much silver nitrate will be left
over?
22. George pours 500.00 mL of a 3.0000 molar solution of sodium hydroxide into a 2.000
liter volumetric flask and fills the flask up with water. What is the new molarity of the
solution?
23. What does dilution mean?
1
24. What volume of 0.113 M copper (II) sulphate is needed to make 50.00 mL of 0.02 M
copper (II)sulphate?
25. What is the molarity of a solution prepared by diluting 0.180 L of 0.600 M nitric acid to
0.540 L?
26. What volume of a 2.50 M NaOH solution is required to make 525 mL of a 0.150 M
NaOH solution?
27. What volume of a 10 M HCl solution is required to make 3 L of a 0.5 M HCl solution?
28. How to prepare 1 N hydrochloric acid from concentrated hydrochloric acid (12.1 M)?
29. How to prepare 0.1 N of sulphuric acid in 500 mL solution from concentrated sulphuric
acid solution (18.0 M)?
30. How to prepare 0.2 N hydrochloric acid in 250 mL from 1 N hydrochloric acid?
31. A glucose solution is 30% mass. How much glucose and water has 100 g of solution?
32. A solution has been prepared with 30 g of sugar solved in water till we get 200 ml of
solution. Which is its mass concentration of sugar in g/L?
33. The concentration of a substance in an aqueous solution can be expressed in different
ways.
a) Define: a) as weight percent
i) b) as volume percent
ii) c) as weight to volume percent
iii) d) parts per millions, ppm
34. We weight 5 g of sodium chloride and water is added till we have 250 ml of solution.
What mass concentration of sodium chloride we get?
35. We need to prepare 150 ml of a 20 g/L solution of iodine. How much iodine and water
do we need?
36. How to prepare standard solution of 100, 50, 20, 10, 5, 3, 2, 1 ppm K from stock
solution 1000 ppm K?
37. When 33g of sugar are dissolved in 198 g of water we get 0,22 liters of solution.
Calculate the mass concentration and the percent of mass of the solution
38. What will be the percent composition by mass of a solution made by dissolving 15.0
g of barium nitrate, Ba(NO3)2 in 45.0 g of water?
39. How many moles of potassium hydroxide, KOH, are required to prepare 2.00 L of
0.250 M solution?
40. What will be the molarity of a solution if 3.50 g of sodium hydroxide, NaOH, are
dissolved in water to make 150 mL of solution?
41. How many milliliters of 12.0 M HCl is needed to prepare 300 ml of 0.250 M HCl
solution?
42. How many grams of hydrogen chloride are in 50 mL concentrated (12M) HCl solution?
43. A sulfuric acid solution has density of 1.49 g/mL and contains 59 percent H 2SO4 by
mass. What is molarity of this solution?
44. How to prepare 0.1N HCl. (Density 1.18 and purity 35.4%).
45. How to prepare 60ppm Cu from Copper sulfate (CuSO4)?
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46. How to prepare 10 % (w/v %) of sodium hydroxide in 350 mL solution?
a) What is the molarity of a solution containing 9.478 grams of RuCl 3 in enough
water to make 1.00 L of solution?
b) What is the volume of a 0.2 M AgNO3 solution containing 8.5 grams of
AgNO3?
c) What is the volume of a 0.1 M HCl solution containing 1.46 grams of HCl?
47. A 2.00g of ammonium chloride reacts with 2.00g of calcium hydroxide. What is the
volume of ammonium gas formed at room temperature? [Relative Molecular Mass of
ammonium chloride is 53.5 and calcium hydroxide is 74.0; molar volume of gas in
room temperature is 24.400cm3]
48. Density = 1.98g/cm3
a) Weight of H2SO4 = 98g
b) Weight of Solution = 100g
c) Calculate the molarity of H2SO4
49. The solution contains 1.65g of NaF in a total volume of 150.0ml. what is its
concentration express as % (m/V)
50. What is the molarity of solution if 300ml of it contains 16.8g of KNO3? [formula weight
KNO3: 101.11amu]
51. Enough water is added to 50.0ml of 0.660M NaOH solution in order to bring the total
volume to 450.0ml. what is the molarity of this diluted solution?
52. Calculate the molarity of 30% W/V H2O2?
53. What is the molarity of pure water at 20°C? [Density of water at 20°C: 0.99821g/cm3]
54. You are requested to produce 2L of 1M solution from a 16M solution. How much of
16M solution is needed? How much water is needed to add to the previous amount of
16M solution to dilute it into 2L of 1M solution?
55. The density of 10% by mass of KCl solution is 1.06g/cm-3. Calculate the molarity of
the solution.
56. A 2.5g sample of groundwater was found to contain 5.4 g of Zn2+. What is the
concentration of Zn2+ in parts per million?
57. An aqueous solution of hydrochloric acid contains 36% HCl by mass. Calculate the
mole fraction of HCl in the solution.
58. A solution with a density of 0.876 g/mL contains 5.0 g of toluene (C7H8) and 225 g of
benzene. Calculate the molarity of the solution.
59. What mass of lead nitrate should be dissolved in 250 mL of water to make a solution
of concentration 0.040M?
60. What are the concentrations of iron(III) and of sulfate ions in 0.10M iron(III) sulfate?
61. In a solution of silver sulfate in water, the concentration of silver ions is 0.0004M. What
is the concentration of sulfate ions in the solution?
62. What is the concentration of nitrate ion in 0.40M aluminium nitrate solution?
63. What volume of 0.25M hydrochloric acid will exactly neutralize 40.0 mL of 2.00M
sodium hydroxide solution?
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64. Silver nitrate solution of concentration 0.025M is added to 50.0 mL of sodium sulfide
solution, causing silver sulfide to precipitate. 21.5 mL of the silver nitrate solution was
just sufficient to precipitate all the sulfide ions present. What was the concentration of
sulfide ions in the sodium sulfide solution?
65. When iron(II) sulfate solution is added to a solution of potassium cyanide, it reacts to
form 6 the hexacyanoferrate(II) ion, Fe(CN). What is the largest volume of 0.50M
iron(II) sulfate 4- solution that would react completely with 120.0 mL of 0.40M KCN
solution?
66. When 12 g of carbon is burned in air, 44 g of carbon dioxide is produced. What mass
of carbon is needed to produce 11 g of carbon dioxide?
67. When 5.0 g of calcium carbonate is decomposed by heating, it produces 2.2 g of
carbon dioxide. What mass of calcium carbonate is needed to produce 8.8 g of carbon
dioxide?

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SIH 1005

1. Calculate the weight of one mole of CaSO4 · 7H2O.

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