Chemistry 30 Recap Chemistry 20 Complete the following chart: Extra Questions Name: Chemical Formula IUPAC Name Ionic, Molecular, or Acid PbI2 (s) ethanol NaHS (aq) sulfurous acid H2O2 (l) titanium (IV) oxide Co(NO3)2 6H2O (s) H2S (aq) gallium sulfate sulfuric acid CH4 (g) ammonium phosphate SO3 (g) HNO3 (aq) dinitrogen tetraoxide Al2(SO4)3 (s) Na2SO3 (aq) ammonia sodium thiosulfate iodine
Write the chemical formula and a dissociation equation for the following compounds. Chemical Formula Dissociation Equation 1. aluminum nitrite 2. calcium phosphate 3. calcium hydrogen oxalate 4. strontium hydrogen sulfate 5. sodium hydrogen phosphate 6. calcium dihydrogen phosphate 7. barium benzoate 8. cobalt(iii) cyanide 9. beryllium fluoride 10. nickel(ii) oxalate Calculations Review 1. What is the mass of one mole of sulfur? 2. Find the number of moles in 5.0 kg of ammonia 3. How many moles of gold are there in a 10.0g rock made of pure gold? 4. Find the mass of a sample containing 0.125 mol of ammonium phosphate. 5. What is the mass of 3.500 mol of cobalt (II) bromide? 6. How many moles of hydrochloric acid are required to react with 0.180 mol of aluminum hydroxide? 7. If a chemical reaction was supposed to produce 4.6 g of silver and only produced 3.6 g of silver, what was the efficiency of the reaction and silver recovery? 8. If 1.486 mol of copper (II) sulfate is used to make 302 ml of copper (II) sulfate solution, what will be concentration of that solution? (Answer in mol/l) 9. How many moles of sodium hypochlorite are required to prepare 300 ml of a 2.5 M sodium hypochlorite solution?
10. What volume of an 8.46 mol/l solution can be made using 5.7 mol of a solute? (Answer in ml) 11. Find the solution concentration made by dissolving 12.5g of sodium sulphate in 635mL of water. 12. Find the mass of solute needed to make 75.0 ml of 1.75 mol/l potassium sulphate solution. 13. Calculate the concentration of the resulting solution when 15 ml of 5.00 mol/l HCl solution is diluted with water to form 100 ml of solution. (Answer in mol/l) 14. What is the concentration of sulfate ions in a 2.50 mol/l solution of iron (III) sulfate? 15. A sample of windshield washer fluid contains 55.3% methanol by volume. What volume of an 881 ml sample of windshield washer fluid is methanol? (Answer in ml) Use the following information to answer the next question. Compound Number Compound Name 1 nitric acid 2 methanol 3 vinegar 16. Identify the compound, as numbered above, which matches each description listed below. Compound: Description: non-electrolyte weak electrolyte strong electrolyte 17. The boiling point of elemental mercury is 357 C. What is this temperature on the Kelvin scale? 18. What is the pressure, in kpa, at the bottom of a diving pool where the pressure measures 2.40 atm? Use the following information to answer the next question. 19. An industrial gas storage tank has an initial volume of 100.0 L when the gas temperature is 62.0 o C. The tank is designed to keep the pressure constant as the gas is used or as the temperature changes. In this case, the gas volume drops to 56.3 L. Assuming that no gas is used or lost, and that the pressure remains constant, what is the final temperature of the gas in the tank? (Answer in K) 20. A sample of CO2(g) has a mass of 20.0 g at STP. What volume does it occupy? (Answer in L) 21. A sample of nitrogen in a sealed vessel with adjustable walls has a volume of 560 ml at a pressure of 150 kpa. The temperature is kept the same, but the volume of the nitrogen is reduced to 400 ml. What is the new pressure inside the vessel? (Answer in kpa) 22. An average basketball contains 4.0 L of air. The average temperature in the gymnasiums where basketball is played is 20.0 o C. The measured pressure in one basketball is 300.5 kpa. How many moles of air are there in this basketball?
Stoichiometry Mass Stoichiometry 1. Hexane (C6H14) is one of the components of automobile gasoline. If 2500 g of pure hexane are burned completely in a car s engine, what mass of water vapor will be produced? 2. Zinc metal reacts violently with sulphur when heated. Predict the mass of sulphur required to react with 25 g of zinc. 3. Carbonic acid can be neutralized by the addition of sodium hydroxide. If 10.0 grams of sodium hydroxide are required, how many moles of carbonic acid are neutralized? 4. A 3.00 g strip of copper is placed in 135 ml of a 0.500 mol/l silver nitrate solution. After several days a large amount of silver precipitate has formed in the solution. This precipitate is removed by filtration and the water evaporated from the filtrate. What mass of silver should remain if the reaction and collection were 85.6 % efficient? 5. Silver tarnishes by reacting with Sulfur in the following reaction. If 4.58 mol of silver react, how many moles of silver sulfide must form? 16Ag(s) + S8(s) 8Ag2S(s) 6. Phosphoric acid can be neutralized by the addition of calcium carbonate in the following reaction. If 10.0 grams of calcium carbonate are required, how many moles of phosphoric acid are neutralized? 2 H3PO4(aq) + 3 CaCO3(s) 3 H2CO3(aq) + Ca3(PO4)2(s) 7. Magnesium hydroxide is used to neutralize acetic acid (vinegar). If 10.0 mol of magnesium hydroxide are used, what mass of water will be formed? 8. Octane (C8H18) is one of the main components of automobile gasoline. If 4000 g of octane are burned completely in a cars engine, what mass of carbon dioxide will be produced? 9. 12.00 g of silver nitrate are dissolved in 500 ml of water to make a solution. A 3.00 g strip of zinc is placed in the solution. After several days a large amount of silver precipitate has formed in the solution. This precipitate is removed by filtration and the water evaporated from the filtrate. What mass of zinc nitrate should form? Use the following information to answer the next two questions. An equation for the rusting of pure iron is: 2Fe(s) + 6HOH(l) 2Fe(OH)3(s) + 3 H2(g) 0.25 mol of iron is completely reacted to produce the products shown above. 10. What mass of Fe(OH)3(s) must be produced? 11. What mass of water is consumed?
Solution Stoichiometry 1. How many moles of copper (II) nitrate are required to make 50 L of a 0.040 M copper (II) nitrate solution? 2. What volume of concentrated 17.8 mol/l sulphuric acid would a lab tech need to make 2.00 L of 0.200 mol/l solution? 3. Calculate the volume of 0.0250 mol/l calcium hydroxide solution required to react completely with 25.0 ml of 0.125 mol/l aluminium sulphate solution. 4. What volume of 0.600 mol/l NaOH can be prepared from 4.80 g of the solute? 5. Describe how to make 100 ml of a 0.0800 mol/l ammonium chloride solution? 6. What volume of concentrated hydrochloric acid must be used to prepare 2.00 L of 0.250 mol/l HCl(aq)? The molar concentration of concentrated hydrochloric acid is 12.4 mol/l. 7. A piece of aluminum is placed in a beaker containing 500 ml of H2SO4(aq) solution. Using the data table below, calculate the concentration of the H2SO4(aq) solution. Time Mass of Aluminum (g) Before Reaction 9.07 After Reaction 3.69 8. A 20.4 g chunk of magnesium metal is added to 1.70 L of 0.450 M hydrochloric acid solution. What concentration of magnesium chloride will result? (Assume that the reaction goes to completion and that the total volume remains the same.) Gas Stoichiometry 1. The Haber process produces ammonia by reacting nitrogen gas with hydrogen gas under specific conditions. Find the mass of ammonia produced by reacting 15 kg of nitrogen gas with excess hydrogen gas. Paraffin (C25H52) is a common hydrocarbon burned in candles. The data collected in a laboratory while burning a candle are shown below. Initial mass of paraffin = 57.94 g Final mass of paraffin = 21.17 g Gaseous products were collected at 25.0 ºC and at 105.0 kpa. 2. What volume of carbon dioxide should be produced by this reaction? 3. Hydrogen gas can be produced by reacting zinc metal with nitric acid. The hydrogen can be collected in test tubes, through water in a pneumatic trough. In one such reaction, 134.96 g of solid zinc are placed into 1.56 L of 9.47 mol/l nitric acid. What volume of hydrogen collected at SATP should be produced by this reaction? 4. What volume of water vapor is released into a room at SATP when 10.0 g of methane burns?
Limiting Reagents 1. 5.00 g of magnesium is reacted with 7.00 g of hydrogen chloride gas. How much of which reagent in grams will be left over? (2.67 g) 2. 50 ml of 1.25 mol/l of hydrochloric acid is reacted with 75 ml of 1.00 mol/l potassium hydroxide. How much of which reagent in ml will be left over? (12.5 ml) 3. 25 ml of 0.55 mol/l phosphoric acid is reacted with 100 ml of 0.010 mol/l sodium hydroxide solution. Find the maximum mass of water that will form. (0.018 g) 4. A 6.72 g sample of zinc was placed in 100.0 ml of 1.50 mol/l hydrochloric acid. After all reaction stops, how much zinc should remain? (1.82 g) 5. 5.00 g of sodium hydroxide is added to 50.0 ml of 1.25 mol/l nitric acid solution. Calculate the mass of water that forms. (1.13 g) 6. 350 g of potassium hydroxide is added to 1.00 L of 6.0 mol/l phosphoric acid solution. How many moles of which reagent is in excess? (3.9 mol) 7. What mass of sodium hydroxide will react exactly with: a. 0.10 mol of hydrochloric acid? (4.0g) b. 0.10 mol of phosphoric acid? (12 g) Write the non-ionic, total ionic, and net ionic equation for the following reactions: 1. iodine reacted with barium bromide solution 2. zinc reacted with copper(ii) sulphate solution 3. potassium reacted with water 4. methanoic acid reacted with lithium hydroxide 5. A solution of iron (III) chloride is tested for the presence of the iron (III) ion by the addition of dilute sodium hydroxide. A red precipitate indicates a positive result. 6. Aqueous solutions of potassium sulphate and barium bromide are mixed. 7. Hydrocyanic acid is reacted with calcium hydroxide. 8. Perchloric acid is reacted with a solution of lithium hydroxide. 9. An aqueous solution of washing soda (sodium carbonate) is added to hard water containing magnesium sulphate. The magnesium ions are precipitated from water. 10. A copper (II) sulphate solution is tested for the presence of copper (II) ion by the addition of an aqueous solution of sodium sulphide. A black precipitate indicates a positive result. 11. Liquid bromine is added to an aqueous solution of sodium iodide. The solution turns brown indicating the presence of aqueous molecular iodine. 12. Sodium metal is reacted with potassium chloride solution.