Chemistry
13th Edition
ISBN: 9781259911156
Author: Raymond Chang Dr., Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 1, Problem 1.105QP
Tums is a popular remedy for acid indigestion. A typical Tums tablet contains calcium carbonate plus some inert substances. When ingested, it reacts with the gastric juice (hydrochloric acid) in the stomach to give off carbon dioxide gas. When a 1.328-g tablet reacted with 40.00 mL of hydrochloric acid (density: 1.140 g/mL), carbon dioxide gas was given off and the resulting solution weighed 46.699 g. Calculate the number of liters of carbon dioxide gas released if its density is 1.81 g/L.
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A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass
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Here's how the student prepared the solution:
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What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits.
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A chemistry student must write down in her lab notebook the concentration of a solution of sodium hydroxide. The concentration of a solution equals the mass
of what's dissolved divided by the total volume of the solution.
Here's how the student prepared the solution:
• The label on the graduated cylinder says:
empty weight: 6.20 g
• She put some solid sodium hydroxide into the graduated cylinder and weighed it. With the sodium hydroxide added, the cylinder weighed 34.241 g.
• She added water to the graduated cylinder and dissolved the sodium hydroxide completely. Then she read the total volume of the solution from the
markings on the graduated cylinder. The total volume of the solution was 61.69 mL.
What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits.
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Chapter 1 Solutions
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