Concept explainers
8-116 A railroad tank car derails and spills 26 tons of concentrated sulfuric acid (1 ton = 907.185 kg). The acid is 98.0% H2SO4 with a density of 1.836 g/mL.
(a) What is the molarity of the acid?
(b) Sodium carbonate, Na2CO3 is used to neutralize the acid spill. Determine the kilograms of sodium carbonate required to completely neutralize the acid. (Chapter 4)
(c) How many liters of carbon dioxide at 18°C and 745 mm Hg are produced by this reaction? (Chapter 5)
(a)
Interpretation:
The molarity of the sulfuric acid should be calculated.
Concept Introduction:
The molarity is the term used to describe the concentration of the aqueous solution. It is calculated by dividing the moles of a substance with volume of the substance in liters.
Answer to Problem 8.116P
The molarity of sulfuric acid is 18.36 M.
Explanation of Solution
The sulfuric acid is 98.0%. that means, if we have 100.0mL of 98.0% sulfuric acid with a density of 1.836g/mL, then the mass of the sulfuric acid would be
Given that, 100.0 g of acid contains 98.0 g of sulfuric acid.
183.6 g acid contains.
The equation of molarity is
The mass percentage and density of the acid are given. From we derived the mass of the acid present. Thus, molarity can be calculated and found to be 18.36 M.
(b)
Interpretation:
The amount of sodium carbonate required in kilograms to completely neutralize the acid should be calculated.
Concept Introduction:
The molar ratio of sulfuric acid and sodium carbonate is to be found. Then the amount of sodium carbonate required to neutralize the acid can be calculated easily.
Answer to Problem 8.116P
The mass of sodium carbonate required to completely neutralize the acid = 24,996.443 kg.
Explanation of Solution
The chemical reaction of sulfuric acid and sodium carbonate is represented using the following equation.
From the chemical equation, it is clear that the molar ratio of sulfuric acid and sodium carbonate is 1:1.
Mass of sulfuric acid = 26 tons.
Mass of each ton = 907.185 kg.
Mass of sulfuric acid in kg =
But we know that the acid is 98.0%
Thus, mass of sulfuric acid =
Moles of sulfuric acid are calculated as below.
From the chemical equation, the moles of sulfuric acid and sodium carbonate are in equal ratio. Hence, the number of moles of sodium carbonate is 235.86
Thus, the mass of sodium carbonate required to completely neutralize the acid = 24,996.443 kg.
The molar ratio of the reactants is used to calculate the mass of sodium carbonate. Thus, the mass of sodium carbonate required to completely neutralize the acid = 24,996.443 kg.
(c)
Interpretation:
The volume of carbon dioxide that is produced during the chemical reaction should be calculated.
Concept Introduction:
The molar ratio of sulfuric acid and carbon dioxide is to be found. The obtained amount of carbon dioxide is converted into volume using the ideal gas equation.
Answer to Problem 8.116P
The volume of carbon dioxide released during the chemical reaction =
Explanation of Solution
The chemical reaction of sulfuric acid and sodium carbonate is represented using the following equation.
From the chemical equation, it is clear that the molar ratio of sulfuric acid and carbon dioxide is 1:1.
Mass of sulfuric acid = 26 tons.
Mass of each ton = 907.185 kg.
Mass of sulfuric acid in kg =
But we know that the acid is 98.0%
Mass of sulfuric acid =
Moles of sulfuric acid are calculated as below.
From the chemical equation, the moles of sulfuric acid and carbon dioxide are in equal ratio. Hence, the number of moles of sodium carbonate is 235.86
Pressure of the gas = 745 mm Hg.
We know that 760 mm Hg = 1 atm.
Thus, 745 mm Hg = 0.9802 atm.
Temperature of the gas = 18
The volume can be calculated using ideal gas equation.
Thus, the volume of carbon dioxide released during the chemical reaction =
The molar ratio of the reactants is used to calculate the moles of carbon dioxide. Thus, the volume of carbon dioxide released during the chemical reaction =
Want to see more full solutions like this?
Chapter 8 Solutions
Introduction to General, Organic and Biochemistry
- 8-43 What is the molarity of a solution made by dissolving 12.7 g of HCI in enough water to make 1.00 L of solution?arrow_forward8-79 (Chemical Connections 8D) Another form of the sprinter's trick is to drink a sodium bicarbonate shake before the event. What would be the purpose of doing so? Give the relevant equations.arrow_forward8-14 Write an equation for the reaction that takes place when each acid is added to water. (a) HNO3 (b) HBr (c) HCO3- (d) NH4+arrow_forward
- 8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water is titrated with 0.200 M NaOH, 30.0 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown diprotic acid?arrow_forward8-50 The usual concentration of HCO3- ions in blood plasma is approximately 24 millimoles per liter (mmol/L). How would you make up 1.00 L of a solution containing this concentration of HCO3- ions?arrow_forward8-98 When a solution prepared by dissolving 4.00 g of an unknown monoprotic acid in 1.00 L of water is titrated with 0.600 M NaOH, 38.7 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown acid?arrow_forward
- What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?arrow_forwardWhich of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?arrow_forward8-41 What is the [OH-] and pOH of each solution? (a) 0.10 M KOH, (b) 0.10 M Na2CO3, (c) 0.10 M Na3PO4, (d) 0.10 M NaHCO3,arrow_forward
- 8-76 (Chemical Connections 8B) Name the most common bases used in over-the-counter antacids.arrow_forward6-82 (Chemical Connections 6C) A solution contains 54 mEq/L ofCI- and 12 mEq/L of HCO3-. If Na+ is the only cation present in the solution, what is the Na+ concentration in milliequivalents per liter?arrow_forward8-33 Write an equation for the reaction of HCI with each compound. Which are acid—base reactions? Which are redox reactions? (a) Na2CO3 (b) Mg (c) NaOH (d) Fe2O3 (e) NH3 (f) CH3NH2 (g) NaHCO3 (h) AIarrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning