Chemistry 101 - Worksheet #4 - Limiting Reactants & Titration
1. Classify each of the following substances as 1) acid, base, or neutral, and 2) strong or weak. Then 3) write a balanced equation for the ionization of the substance in water:
a) HNO3
b) HClO
c) NH3
d) NaNO3
e) Ba(OH)2
2. For the reaction: 6 Li(s) + N2(g) → 2 Li3N(s) determine:
a) the mass of N2 needed to react with 0.536 moles of Li.
b) the number of moles of Li required to make 46.4 g of Li3N.
c) the mass in grams of Li3N produced from 3.65 g Li.
d) the number of moles of lithium needed to react with 7.00 grams of N2.
3. A common method of preparing solutions is to make up a concentrated solution and then dilute it to the desired concentration.
a) What is the molarity of a solution prepared by dissolving 29.2 g NaCl in enough water to make 0.250 liters of solution?
b) What volume of the above solution is needed to make 125 ml of a 0.350 M NaCl solution?
4. Indicate whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction.
a) iron (III) nitrate and potassium hydroxide
b) ammonium chloride and lithium carbonate
c) sodium sulfide and nickel(II) sulfate
5. When iron(III) chloride and sodium hydroxide are mixed, a precipitate forms.
a) Write a balanced molecular equation for this reaction.
b) What volume of 0.200 M iron(III) chloride is needed to completely precipitate the product when mixed with 30.0 mL of 0.500 M sodium hydroxide?
c) What mass of precipitate is formed?
6. How many ml of 2.50 M HNO3 contain enough nitric acid to dissolve an old copper penny with a mass of 3.94 grams?
3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO32)(aq) + 2 NO(g) + 4 H2O
7. What is the concentration of a NaOH solution when 45.6 mL of that solution is titrated to the endpoint with 34.2 mL of 0.289M sulfuric acid?
Recitations Worksheet #7
