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Ch.1 - Introduction: Matter, Energy, and Measurement
All textbooksBrown 14th EditionCh.1 - Introduction: Matter, Energy, and MeasurementProblem 37c
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Chapter 1, Problem 37c

(c) Is a graduated cylinder such as that shown in Figure 1.21 likely to afford the accuracy of measurement needed?
Graduated cylinder showing measurement markings up to 20 mL, illustrating precision in measurements.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Graduated Cylinder

A graduated cylinder is a common laboratory instrument used to measure the volume of liquids. It features marked graduations along its length, allowing for precise volume readings. The accuracy of measurement depends on the cylinder's design, the clarity of the markings, and the observer's ability to read the meniscus correctly.
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Meniscus

The meniscus is the curve seen at the surface of a liquid in a container, such as a graduated cylinder. It occurs due to surface tension and the adhesive forces between the liquid and the container's walls. Accurate volume measurement requires reading the bottom of the meniscus at eye level to avoid parallax errors.

Precision and Accuracy

Precision refers to the consistency of repeated measurements, while accuracy indicates how close a measurement is to the true value. In the context of a graduated cylinder, precision is influenced by the smallest division on the scale, while accuracy can be affected by factors such as calibration and user technique in reading the meniscus.
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Textbook Question

(b) Carbon dioxide (CO2) is a gas at room temperature and pressure. However, carbon dioxide can be put under pressure to become a 'supercritical fluid' that is a much safer dry-cleaning agent than tetrachloroethylene. At a certain pressure, the density of supercritical CO2 is 0.469 g/cm3. What is the mass of a 25.0-mL sample of supercritical CO2 at this pressure?

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Textbook Question

(a) To identify a liquid substance, a student determined its density. Using a graduated cylinder, she measured out a 45-mL sample of the substance. She then measured the mass of the sample, finding that it weighed 38.5 g. She knew that the substance had to be either isopropyl alcohol 1density 0.785 g/mL2 or toluene (density 0.866 g/mL). What are the calculated density and the probable identity of the substance?

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Textbook Question

(b) An experiment requires 45.0 g of ethylene glycol, a liquid whose density is 1.114 g/mL. Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylinder. What volume of the liquid should he use?

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Textbook Question

(d) A cubic piece of metal measures 5.00 cm on each edge. If the metal is nickel, whose density is 8.90 g/cm3, what is the mass of the cube?

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Textbook Question

(a) After the label fell off a bottle containing a clear liquid believed to be benzene, a chemist measured the density of the liquid to verify its identity. A 25.0-mL portion of the liquid had a mass of 21.95 g. A chemistry handbook lists the density of benzene at 15 °C as 0.8787 g/mL. Is the calculated density in agreement with the tabulated value?

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Textbook Question

(b) An experiment requires 15.0 g of cyclohexane, whose density at 25 C is 0.7781 g>mL. What volume of cyclohexane should be used?

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