Textbook Question
The density of a 20.0% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution.
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Ch.4 - Chemical Quantities & Aqueous Reactions
Chapter 4, Problem 104
Toilet bowl cleaners often contain hydrochloric acid, which dissolves the calcium carbonate deposits that accumulate within a toilet bowl. What mass of calcium carbonate (in grams) can be dissolved by 3.8 g of HCl? (Hint: Begin by writing a balanced equation for the reaction between hydrochloric acid and calcium carbonate.)
Verified step by step guidance1
Write the balanced chemical equation for the reaction: \( \text{CaCO}_3 (s) + 2\text{HCl} (aq) \rightarrow \text{CaCl}_2 (aq) + \text{CO}_2 (g) + \text{H}_2\text{O} (l) \).
Calculate the molar mass of HCl and CaCO₃ using the periodic table.
Determine the number of moles of HCl present in 3.8 g by using the formula: \( \text{moles of HCl} = \frac{\text{mass of HCl}}{\text{molar mass of HCl}} \).
Use the stoichiometry of the balanced equation to find the moles of CaCO₃ that react with the calculated moles of HCl. Note that 2 moles of HCl react with 1 mole of CaCO₃.
Convert the moles of CaCO₃ to grams using its molar mass: \( \text{mass of CaCO}_3 = \text{moles of CaCO}_3 \times \text{molar mass of CaCO}_3 \).
Related Practice
Textbook Question
Find the percent by mass of sodium chloride in a 1.35 M NaCl solution. The density of the solution is 1.05 g/mL.
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Open Question
People sometimes use sodium bicarbonate as an antacid to neutralize excess hydrochloric acid in an upset stomach. What mass of hydrochloric acid (in grams) can 2.5 g of sodium bicarbonate neutralize? (Hint: Begin by writing a balanced equation for the reaction between aqueous sodium bicarbonate and aqueous hydrochloric acid.)
Textbook Question
The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)
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Textbook Question
Many home barbeques are fueled with propane gas (C3H8). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)
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Textbook Question
Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3) with salicylic acid (C7H6O3) to form aspirin (C9H8O4) and acetic acid (C2H4O2). The balanced equation is: C4H6O3 + C7H6O3 → C9H8O4 + C2H4O2 In a laboratory synthesis, a student begins with 3.00 mL of acetic anhydride (density = 1.08 g/mL) and 1.25 g of salicylic acid. Once the reaction is complete, the student collects 1.22 g of aspirin. Determine the limiting reactant. Determine the theoretical yield of aspirin. Determine the percent yield for the reaction.
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