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4.7: End of Chapter Problems

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    1. Explain what changes and what stays the same when 1.00 L of a solution of NaCl is diluted to 1.80 L.
    2. What information do we need to calculate the molarity of a sulfuric acid solution?
    3. What does it mean when we say that a 200-mL sample and a 400-mL sample of a solution of salt have the same molarity? In what ways are the two samples identical? In what ways are these two samples different?
    4. Determine the molarity for each of the following solutions:
      1. 0.444 mol of CoCl2 in 0.654 L of solution
      2. 98.0 g of phosphoric acid, H3PO4, in 1.00 L of solution
      3. 0.2074 g of calcium hydroxide, Ca(OH)2, in 40.00 mL of solution
      4. 10.5 kg of Na2SO4·10H2O in 18.60 L of solution
      5. 7.0 × 10−3 mol of I2 in 100.0 mL of solution
      6. 1.8 × 104 mg of HCl in 0.075 L of solution
    Answer
    a. 0.679 M; b. 1.00 M; c. 0.06998 M; d. 1.75 M; e. 0.070 M; f. 6.6 M
    1. Determine the molarity of each of the following solutions:
    1. 1.457 mol KCl in 1.500 L of solution
    2. 0.515 g of H2SO4 in 1.00 L of solution
    3. 20.54 g of Al(NO3)3 in 1575 mL of solution
    4. 2.76 kg of CuSO4·5H2O in 1.45 L of solution
    5. 0.005653 mol of Br2 in 10.00 mL of solution
    6. 0.000889 g of glycine, C2H5NO2, in 1.05 mL of solution
    Answer
    a. a. 0.9713 M; b. 5.25x10-3 M; c. 6.122x10-2 M; d. 7.62 M; e. 0.5653 M; f. 1.13x10-2 M
    1. Consider this question: What is the mass of the solute in 0.500 L of 0.30 M glucose, C6H12O6, used for intravenous injection?
    1. Outline the steps necessary to answer the question.
    2. Answer the question.
    Answer
    a. determine the number of moles of glucose in 0.500 L of solution; determine the molar mass of glucose; determine the mass of glucose from the number of moles and its molar mass; b. 27 g
    1. Consider this question: What is the mass of solute in 200.0 L of a 1.556-M solution of KBr?
      1. Outline the steps necessary to answer the question.
      2. Answer the question.
    Answer
    a. Calculate to moles of KBr by multiplying the Molarity by the amount of solution (200.0 L); then, Find the Molar Mass of KBr and convert moles of solute to grams; b. 37.03 kg
    1. Calculate the number of moles and the mass of the solute in each of the following solutions:
    1. 2.00 L of 18.5 M H2SO4, concentrated sulfuric acid
    2. 100.0 mL of 3.8 × 10−5 M NaCN, the minimum lethal concentration of sodium cyanide in blood serum
    3. 5.50 L of 13.3 M H2CO, the formaldehyde used to “fix” tissue samples
    4. 325 mL of 1.8 × 10−6 M FeSO4, the minimum concentration of iron sulfate detectable by taste in drinking water
    Answer
    a. 37.0 mol H2SO4; 3.63 × 103 g H2SO4; (b) 3.8 × 10−6 mol NaCN; 1.9 × 10−4 g NaCN; (c) 73.2 mol H2CO; 2.20 kg H2CO; (d) 5.9 × 10−7 mol FeSO4; 8.9 × 10−5 g FeSO4
    1. Calculate the number of moles and the mass of the solute in each of the following solutions:
    1. 325 mL of 8.23 × 10−5 M KI, a source of iodine in the diet
    2. 75.0 mL of 2.2 × 10−5 M H2SO4, a sample of acid rain
    3. 0.2500 L of 0.1135 M K2CrO4, an analytical reagent used in iron assays
    4. 10.5 L of 3.716 M (NH4)2SO4, a liquid fertilizer
    Answer
    a. 2.67x10-5 moles KI; 4.44x10-3g KI; b. 1.7x10-6 moles H2SO4 ; 1.6x10-4 g H2SO4; c. 2.838x10-2 moles K2CrO4 ; 5.510g K2CrO4; d. 39.0 moles (NH4)2SO4 ; 5,160 g (NH4)2SO4
    1. Consider this question: What is the molarity of KMnO4 in a solution of 0.0908 g of KMnO4 in 0.500 L of solution?
      1. Outline the steps necessary to answer the question.
      2. Answer the question.
    Answer
    a. Determine the molar mass of KMnO4; determine the number of moles of KMnO4 in the solution; from the number of moles and the volume of solution, determine the molarity; b. 1.15 × 10−3 M
    1. Consider this question: What is the molarity of HCl if 35.23 mL of a solution of HCl contain 0.3366 g of HCl?
      1. Outline the steps necessary to answer the question.
      2. Answer the question.
    Answer
    a. Convert g of HCl to moles of HCl and convert mL of solution to L of solution, Divide moles of HCl by L of solution; b. 0.2621 M ;
    1. Calculate the molarity of each of the following solutions:
      1. 0.195 g of cholesterol, C27H46O, in 0.100 L of serum, the average concentration of cholesterol in human serum
      2. 4.25 g of NH3 in 0.500 L of solution, the concentration of NH3 in household ammonia
      3. 1.49 kg of isopropyl alcohol, C3H7OH, in 2.50 L of solution, the concentration of isopropyl alcohol in rubbing alcohol
      4. 0.029 g of I2 in 0.100 L of solution, the solubility of I2 in water at 20 °C
    Answer
    a. 5.04 × 10−3 M; b. 0.499 M; c. 9.92 M; d. 1.1 × 10−3 M
    1. Calculate the molarity of each of the following solutions:
      1. 293 g HCl in 666 mL of solution, a concentrated HCl solution
      2. 2.026 g FeCl3 in 0.1250 L of a solution used as an unknown in general chemistry laboratories
      3. 0.001 mg Cd2+ in 0.100 L, the maximum permissible concentration of cadmium in drinking water
      4. 0.0079 g C7H5SNO3 in one ounce (29.6 mL), the concentration of saccharin in a diet soft drink.
    2. There is about 1.0 g of calcium, as Ca2+, in 1.0 L of milk. What is the molarity of Ca2+ in milk? Answer: 0.025 M
    3. What volume of a 1.00-M Fe(NO3)3 solution can be diluted to prepare 1.00 L of a solution with a concentration of 0.250 M?
    4. If 0.1718 L of a 0.3556-M C3H7OH solution is diluted to a concentration of 0.1222 M, what is the volume of the resulting solution? Answer: 0.5000 L
    5. If 4.12 L of a 0.850 M-H3PO4 solution is be diluted to a volume of 10.00 L, what is the concentration the resulting solution?
    6. What volume of a 0.33-M C12H22O11 solution can be diluted to prepare 25 mL of a solution with a concentration of 0.025 M? Answer: 1.9 mL
    7. What is the concentration of the NaCl solution that results when 0.150 L of a 0.556-M solution is allowed to evaporate until the volume is reduced to 0.105 L?
    8. What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?
      1. 1.00 L of a 0.250-M solution of Fe(NO3)3 is diluted to a final volume of 2.00 L
      2. 0.5000 L of a 0.1222-M solution of C3H7OH is diluted to a final volume of 1.250 L
      3. 2.35 L of a 0.350-M solution of H3PO4 is diluted to a final volume of 4.00 L
      4. 22.50 mL of a 0.025-M solution of C12H22O11 is diluted to 100.0 mL
    Answer
    a. 0.125 M; b. 0.04888 M; c. 0.206 M; d. 0.0056 M
    1. What is the final concentration of the solution produced when 225.5 mL of a 0.09988-M solution of Na2CO3 is allowed to evaporate until the solution volume is reduced to 45.00 mL?
    2. A 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 g of HCl. What is the molarity of the solution? Answer: 11.9 M
    3. An experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many mL of 11.9 M HCl would be required to make 250 mL of 2.00 M HCl?
    4. What volume of a 0.20-M K2SO4 solution contains 57 g of K2SO4? Answer: 1.6 L
    5. The US Environmental Protection Agency (EPA) places limits on the quantities of toxic substances that may be discharged into the sewer system. Limits have been established for a variety of substances, including hexavalent chromium, which is limited to 0.50 mg/L. If an industry is discharging hexavalent chromium as potassium dichromate (K2Cr2O7), what is the maximum permissible molarity of that substance?

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