1. What mass of H2 should be produced by the reaction of Al with 75.0 mL of 2.95M HCl?  2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H2 (g). ln the lab, 0.15g H2 was collected. What is the % yield of the reaction?  

2. How many milliliters of 0.200M H2SO4 are required to react with 10.32 mL of 0.4042 M NaHCO3? H2SO4 (aq) + 2NaHCO3 (aq)  Na2SO4 (aq) + 2H2O (l) + 2CO2

3. Calculate the volume of 0.1250 M phosphoric acid solution necessary to react with 50.0mL of 0.250M Mg(OH)2.  2H3PO4 + 3Mg(OH)2  Mg3(PO4)2 + 6H2O

4. An excess of AgNO3 reacts with 185.5 mL of an AlCl3 solution to give 0.325g of AgCl. What is the concentration, in moles per liter, of the AlCl3 solution?  AlCl3 + 3AgNO3  3AgCl + Al(NO3)3

5. Lead ion react with phoshate ion to form the sparingly soluble Pb3(PO4)2  3Pb(NO3)2 + 2Na3PO4  Pb3(PO4)2 + 6NaNO3

What weight of Pb3(PO4)2 will form when 2.50 L of 0.285M Na3PO4 are mixed with 0.600 L of 0.178M Pb(NO3)2?

6. Oxalic acid reacts with the chromate ion in acidic solution as follows:  H2C2O4(aq) + 2 CrO42- (aq) + 10 H+  6 CO(g) + 2 Cr3+(aq) + 8 H2O(l)

2.5683g of K2CrO4 was weighed out, dissolved and diluted to 500mL in a volumetric flask. Calculate the molarity of the oxalic acid if a 25.00 mL aliquot of this acid solution consumed 28.54 mL of the chromate solution.

7. Calculate the volume of 0.1250 M phosphoric acid solution necessary to react with 50.0mL of 0.250M Mg(OH)2. 2H3PO4 + 3Mg(OH)2  Mg3(PO4)2 + 6H2O

8. An excess of AgNO3 reacts with 185.5 mL of an AlCl3 solution to give 0.325 g of AgCl. What is the concentration, in moles per liter, of the AlCl3 solution?  AlCl3 + 3AgNO3  3AgCl + Al(NO3)3 9. 100 mL of a solution contains 10.000 g of KCl. What is the concentration of KCl in mol/dm3?

10. What volume of water must be added to 450 cm3 of a 0,25 M NaCl solution in order to produce a 0,15 M solution?


11. How would you prepare these solutions?
11.1 600mL of 0.085M K2SO4 solution. 11.2 500 mL of 0.9 % (w/v) NaCl in H2O. 11.3 500 mg of 0.9 % (w/w) NaCl in H2O

12. A patient is given 1000 mL of 0.9 % (w/v) NaCl intravenously. How many grams of NaCl did the patient receive?

13. How would you prepare 750 g of an aqueous solution that is 2.5 % (w/w) NaOH?


14. An aqueous solution of hydrofluoric acid contains 49.0% HF by mass. The density of this solution is 1.17 g/mL. Calculate: 14.1 the molarity of the solution 14.2 the volume of this solution required to prepare 500 mL of 0.10 M hydrofluoric acid solution

15. How many mL of 15 M HNO3 is required to react with 2.5 g Cu according to the following reaction: 3Cu(s) + 8HNO3 (aq)  3 Cu(NO3)2(aq) + 2NO(g) + 4H2O(l)

16. How would you prepare 550 g of an aqueous solution that is 3.0 % (w/w) K2SO4?

17. What mass of CoCl2.6H2O must be weighed out to prepare 100 mL of a solution that is 300 ppm Co2+?


18. How many grams of sodium carbonate are required to neutralize 750 cm3 of 5.0 M HCl? Na2CO3 + 2HCl  2NaCl + H2O + CO2 19. Iodine, I2, reacts with the thiosulfate ion to give the iodide ion and the tetrathionate ion, S4O62-. 19.1 Balance the chemical equation for the above reaction. 19.2 If 10,0 grams of iodine is dissolved in an appropriate manner to give 300 cm3 of solution, what is the molarity of the iodine solution? 19.3 What volume of a 0,125 M sodium thiosulfate solution will be needed for complete reaction of the solution in (19.2)?

20. A solution was prepared by dissolving 373 mg of K4Fe(CN)6 in distilled water and diluting to exactly 500 mL. Calculate 20.1 The molar concentration of K4Fe(CN)6. 20.2 The molar concentration of K+

21. A water sample is found to contain 0.00569 M MgCO3. What is the MgCO3 content in parts per million (ppm)?

22. A bottle of perchloric acid stock solution indicates that the solution is 70.0 % HClO4 by mass and has a density of 1.67 g/mL. Calculate 22.1 The molarity of the solution. 22.2 The volume (in mL) of this solution required to prepare 500 mL of a 0.350 M HClO4 solution 23. Commercial sulphuric acid (d=1.831 g/mL) is 94 % H2SO4 by mass. What is the molarity of this solution? The normality?

24. A certain vinegar is 5.88 % acetic acid (CH3CO2H) by mass. What mass of CH3CO2H, in grams, is contained in a 355 mL bottle of vinegar? (Assume d = 1.01g/mL)


25. An aqueous solution is 26 % chromic acid, K2CrO4 and has a density of 1.036 g/mL. Calculate 25.1 The molarity 25.2 The volume required (in mL) to make up 1.5 L of 0.5 M K2CrO4