|1.||Ammonium sulphate is a "high-nitrogen" fertilizer. It is
manufactured by reacting sulphuric acid with ammonia. In a laboratory
study of this process, 50.0 mL of sulphuric acid reacts with 24.4 mL of a
2.20 M ammonia solution (ammonium hydroxide) to yield the product
ammonium sulphate in solution. Calculate the molar concentration of
the sulphuric acid used.
|2.||Slaked lime is sometimes used in water treatment plants to clarify
water for residential use. The lime is added to an aluminum sulphate
solution in the water. Fine particles in the water stick to the floc
precipitate produced, and settle out with it. Calculate the volume
of 0.0250 M calcium hydroxide solution that can be completely reacted with
25.0 mL of 0.25 M aluminum sulphate solution.
|3.||In designing a solution stoichiometry experiment for her class to perform, a chemistry teacher wants 75.0 mL of 0.200 M iron(III) chloride solution to react completely with an excess of 0.250 M sodium carbonate solution.|
|a) What is the minimum volume of this sodium carbonate
|b) What would be a reasonable volume of this
sodium carbonate solution to use in this experiment? Provide your
|4.||A student wishes to precipitate all the lead(II) ions from 2.0
L of solution containing, among other substances, 0.34 M Pb(NO3)2(aq).
The purpose of this reaction is to make the filtrate solution non-toxic.
If the student intends to precipitate lead(II) sulphate, suggest and calculate
an appropriate solute, and calculate the required mass of this solute.
|5.||Copper(II) ions can be precipitated from waste solution by adding aqueous sodium carbonate.|
|a) What is the minimum volume of 1.25 M Na2CO3(aq)
needed to precipiate all the copper(II) ions in 4.54 L of 0.0875 M CuSO4(aq)
|b) Suggest a suitable volume to use for this reaction.
|6.||A 24.89 piece of zinc is placed into a beaker containing 350 mL
of hydrochloric acid. The next day the remaining zinc is removed, dried,
weighed, and found to have a mass of 21.62 grams. Determine the concentration
of zinc chloride in the beaker.
|7.||How many millilitres of 0.300 M NiCl2(aq) solution
are required to completely react with 25.0 mL of 0.100 M Na2CO3(aq)
solution? How many grams of NiCO3(s) will be formed?
|8.||How many millilitres of 0.400 M CaCl2(aq) would be needed
to react completely with 35.0 mL of
0.600 M AgNO3(aq) solution?
|9.||Suppose that 30.0 mL of 0.400 M NaCl(aq) is added to 30.0 mL of 0.300 M AgNO3(aq).|
|a) How many moles and grams of AgCl(s) would precipitate?|
|b) What would be the concentrations of each of the remaining ions in the solution after reaction?|