A. PROBLEM SOLVING. Solve the following problems (5 points each). Use Given-RequiredEquation-Solution-Answer format in answering. 1-5. Using the following equation: \[ 2 \mathrm{NaOH}+\mathrm{H} 2 \mathrm{SO} 4 \rightarrow 2 \mathrm{H} 2 \mathrm{O}+\mathrm{Na} 2 \mathrm{SO} 4 \] How many grams of sodium sulfate will be formed, if you start with \( 1.50 \mathrm{~L} \) of a \( 4.0 \mathrm{M} \) solution of sodium hydroxide? 6-10. How many grams of \( \mathrm{Ca}(\mathrm{OH}) 2 \) are needed to neutralize \( 25.0 \mathrm{~mL} \) of \( 0.100 \mathrm{M} \) HNO3? The reaction proceeds as follows: \[ 2 \mathrm{HNO} 3(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH}) 2(\mathrm{~s}) \rightarrow \mathrm{H} 2 \mathrm{O}(\mathrm{l})+\mathrm{Ca}(\mathrm{NO} 3) 2(\mathrm{aq}) \] 11-15. At \( 40^{\circ} \mathrm{C} \), the blood has an osmotic pressure of \( 8.02 \mathrm{~atm} \). How many grams of glucose is contained in a \( 5 \mathrm{~mL} \) of intravenous injection to have the same osmotic pressure as the blood? MM of glucose is \( 180 \mathrm{~g} / \mathrm{mol} \). \( 16-20 \). What is the freezing point of a solution of 10 grams of glucose, \( \mathrm{C} 6 \mathrm{H} 12 \mathrm{O} 6 \) , and \( 1500 \mathrm{~g} \) of water? 21-25. Determine the boiling point of a solution of \( 10 \mathrm{grams} \) of a substance of molecular weight \( 94 \mathrm{~g} / \mathrm{mol} \) in 500 grams water. 26-30. What weight of \( \mathrm{NaCl} \) in \( 800 \mathrm{~g} \) acetone is needed to bring boiling point to \( 60^{\circ} \mathrm{C} \) ? (Boiling point of pure acetone \( =55.95^{\circ} \mathrm{C} ; \mathrm{Kb} \) of acetone \( =1.71^{\circ} \mathrm{C} / \mathrm{m} \) ) B. SHORT- ANSWER TYPE. Explain each of the following phenomena (5 points each). \( 31-35 \). Fishes need oxygen to survive. Goldfish in a crowded aquarium has a better chance of survival in cold water than in warm water. \( 36-40 \). Adding sugar to a glass of juice that already has crystals of sugar at the bottom makes the juice sweeter.
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Given: 1.50 L of 4.0 M NaOH solution Required: grams of Na2SO4 formed Equation: 2 NaOH + H2SO4 -> 2 H2O + Na2SO4 Solution: Show more…
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For 38-40: An alcohol, C2H5OH, is present in 1L of wine that is 12% alcohol by volume. The density of the solution is 0.984 g/mL, and the density of pure alcohol is 0.789 g/mL. (C2H5OH = 46.07 g/mol) 38. What is the weight of the alcohol present in the wine? a) 95 g b) 88 g c) 58 g d) 46 g 39. What is the molarity of the solution? a) 2.1 M b) 1.9 M c) 1.2 M d) 0.99 M 40. Ten milliliters of vinegar are diluted to 100 mL with water. A 10 mL sample of this diluted solution required 12 mL of 0.05 N NaOH for neutralization. If the vinegar has a density of 1.03 g/mL, calculate the % by weight of the acetic acid in the vinegar. (NaOH molar mass = 39.99 g/mol; Acetic acid molar mass = 60.05 g/mol) a) 1.8% b) 3.5% c) 6.0% d) 9.3% 41. Colligative properties depend on ____________. a) The physical properties of the solute particles dissolved in solution b) The nature of the solute particles dissolved in solution c) The number of solute particles in solution d) The nature of solvent particles 42. When mercuric iodide is added to the aqueous solution of potassium iodide, the _________. a) Freezing point is raised b) Freezing point is lowered c) Boiling point does not change d) Freezing point does not change 43. An aqueous solution of methanol in water has a vapor pressure that is a) Equal to that of methanol b) More than that of water c) Less than that of water d) Equal to that of water 44. 18 g of glucose (C6H12O6) is added to 178.2 g of water. The vapor pressure of water for this aqueous solution at 100°C is ________. (2 points) a) 7.60 torr b) 76.00 torr c) 752.40 torr d) 759.00 torr 45. Which of the following compounds corresponds van't Hoff factor 'i' to be equal to 2 for a dilute solution? (2 points) a) K2SO4 b) MgSO4 c) NaHSO4 d) C6H12O6 46. What is the freezing point of a non-volatile solution of 210.0 g of glycerol (C3H8O3) in 350 g of water? (2 points) a) -9.12°C b) -10.2°C c) -12.1°C d) -15.3°C 47. What is the vapor pressure of a non-electrolyte solution made by dissolving 82.4 g of urea (CH4N2O) in 212 mL of water at 35°C? The vapor pressure of pure water at the given temperature is 42.18 mmHg. The density of the resulting solution is assumed to be 1.0 g/mL. (2 points) a) 4.39 mmHg b) 6.78 mmHg c) 35.40 mmHg d) 37.79 mmHg 48. A strong electrolyte solution of potassium chloride was prepared using water. What will be the theoretical boiling point of this solution if 0.247 kg of potassium chloride is dissolved in 2,900 g of water? (2 points) a) 100.28°C b) 100.58°C c) 101.16°C d) 102.30°C 49. A 0.6837 M solution of C12H22O11 using water as the solvent has a density of 1.35 g/mL. What is the freezing point depression of this solution? (2 points) a) -5.12°C b) -3.57°C c) -1.14°C d) -0.11°C 50. A 500 mL of aqueous solution contains 30 g of a certain protein. The osmotic pressure of the solution is 15.28 atm at 25°C. What is the molar mass of the said protein? (2 points) a) 31.24 g/mol b) 62.05 g/mol c) 80.01 g/mol d) 96.07 g/mol
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* The pH of a sodium benzoate (C6H5COONa) solution is 9.00. What is C6H5COONa? (Ka = 6.0 x 10^-5 for C6H5COOH acid) * a) What are the concentrations of H+(aq), OCl-(aq), and HOCl(aq) in a 0.20 M HOCl solution? b) What is the ionization percentage of HOCl in this solution? (Ka = 3.2 x 10^-8 for HOCl) * C2H4(g) + H2(g) -> C2H6(g) The activation energy of the reaction is 181 kJ/mol and the value of the rate constant k at 700 K is 1.3 x 10^-3 L/mol.s. What is the rate constant value (k) of this reaction at 730 K? (R = 8.314 J/mol.K) * Compare the acidity of H2S, H2Se, and H2Te. How does acidity vary between the hydrides of a group of elements? * Explain how to prepare a 750 mL 0.125 M CaCl2 solution using 89% pure solid (MCaCl2 = 111 g/mol). * Cocaine (K) is a weak base and its ionization in water is as follows: K(aq) + OH-(aq) -> 5.0 x 10^-3 M. Since the pH of the cocaine solution is 10.04, what is the ionization constant of this substance? * At 25°C, 1 liter of water dissolves 1.7 x 10^-5 mol Cd(OH)2. Calculate the Ksp value of Cd(OH)2. * Diphosphorus tetraiodide is obtained by the reaction P4O6 + 4I2 -> 2P2I4 + P4O10. a) How many grams increase from each reagent? b) How many grams of P2I4 are formed? (P = 30.97 g/mol, O = 16 g/mol, I = 126.90 g/mol) * Find a) molarity and b) molality since the density of a 15% AgNO3 solution by mass is 1.08 g/mL. (AgNO3: 170 g/mol) * A solution containing 20.0 grams of a substance dissolved in exactly 1 mole of a volatile solvent has a vapor pressure of 0.500 atm at 20°C. If 1 mole more than the solvent is added to the mixture, the vapor pressure of the resulting solution at the same temperature is 0.550 atm. a) What is the molecular weight of the solute? b) What is the vapor pressure of a pure solvent at 20°C?
1. If 45.0 g of sugar is dissolved in 200.0 g of water, what is the mass percent of the sugar solution? 2. How many grams of a 23.4% salt solution are needed if you have 56 g of the salt in it? 3. How many moles of LiF would be present in 575 mL of 0.750 Molar LiF solution? 4. What is the ion concentration of a solution prepared by diluting 10.0 mL of 6.0 HCl to a final volume of 200.0 mL? 5. What are the final concentrations in a 0.15 M solution of MgCl2? 6. What is the molality of a solution made by dissolving 35 g of NaNO3 into 2500 g of water? 7. What is the change in freezing point given 1.6 moles of C6H12O6 into 4.3 kg of water? Kf for water is 1.86 C/mol. 8. What is the freezing point of a 2.2 molal Ca(NO3)2 solution? Kf for water is 1.86. 9. A 25.0 mL sample of 0.55 M HCl was titrated with 31 mL of Al(OH)3. What is the concentration of the Al(OH)3 given 3HCl + Al(OH)3 -> BaCl3 + 3H2?
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