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Worksheet #4 - Limiting Reactants & Titration, Assignments of Chemistry

For students to practice their skills with “Limiting Reactants & Titration”

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2020/2021

Uploaded on 09/26/2022

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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
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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) HNO b) HClO c) NH d) NaNO e) Ba(OH)
  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 #

Chemistry 101 - Worksheet #4 - Limiting Reactants & Titration

  1. Cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible. What is the sign of Δ H for this reaction (ammonium nitrate dissolving) and is it exothermic or endothermic?
  2. Fill in the blanks: a) In a reaction in which the energy of the system decreases, the energy of the surroundings will ________________. b) The system is (circle one:) open or closed if it loses 5.6 g of mass to the surroundings during a change. c) The system (circle one:) gains or loses energy when it transfers heat to the surroundings at constant volume. d) The wall of a container is __________ if a reaction generates heat and the energy of the surroundings remains constant. e) When the system does work, its volume _________ and the sign of the work done is _________. f) If the energy of the reactants in a chemical reaction is more positive than the total energy of the products, the reaction is (circle one:) exothermic or endothermic.
  3. A system absorbs 21.6 kJ of heat while expanding its volume from 1.25 L to 71.85 L against a constant pressure of 0.965 atm. (conversion factor: 1 L•atm = 101.266 J) a) How much work is done by the system? b) What is the energy change of the system?
  4. Benzene is a starting material in the synthesis of nylon fibers and polystyrene (Styrofoam). Its specific heat capacity is 1.74 J/(g•K). If 16.7 kJ of energy is absorbed by a 225 g sample of benzene at 20.0 °C, what is its final temperature?
  5. A 1.000 g sample of octane (C8H18) is burned in a bomb calorimeter at an initial temperature of 25.00 °C. After the reaction, the temperature of the water and calorimeter is 33.20 °C. The heat capacity of the calorimeter is 5.87 kJ/°C. Calculate the heat of combustion (kJ/mol) of octane.
  6. When 50 mL of aqueous solution A is mixed with 50 mL of aqueous solution B in a constant pressure calorimeter, the temperature increases from 21.0 °C to 27.5 °C. Assuming that 6.7 g of product C are formed in the reaction and the molar mass of C is 46.7 g/mol, calculate the enthalpy change for the reaction per mole of product C. (Hint: assume the final solution has the same density (1.00 g/mL) and specific heat capacity as water). A + B → C
  7. Calculate the Δ H°rxn for the following reaction below: H3AsO4(aq) + 4H2(g) → AsH3(g) + 4H2O(l) Δ H°f [AsH3(g)] = 66.4 kJ/mol Δ H°f [H3AsO4(aq)] = -904.6 kJ/mol Δ H°f [H2O(l)] = -285.8 kJ/mol