Passage III

A chemist performed 3 experiments to determine the boiling points and freezing points of purified water (H2O) and solutions of various types of solids dissolved in H2O.

Experiment 1

Fifty milliliters (mL) of H2O was heated in a beaker. The temperature of the H2O was recorded every 2 minutes (min) until it remained constant, indicating the boiling point. The procedure was repeated with a solution of 5 grams (g) of sodium chloride (NaCl) in 50 mL of H2O and with 10 g of NaCl in 50 mL of H2O. The results are shown in Figure 1.

Figure adapted from M. Lesser, C. Constant, and J. Weisler, Contemporary Science — Book 3. ©1978 by Amsco School Publications, Inc.

Experiment 2

A beaker containing 50 mL of H2O was placed in a dry ice bath (an insulated bowl of solid CO2, which produces temperatures below -70°C). When the H2O began to solidify, the temperature was recorded. The procedure was repeated with various amounts of NaCl added to 50 mL of H2O. The percentages of NaCl by mass, the masses of NaCl, and the freezing points are shown in Table 1.

Experiment 3

The freezing points of various solutions of potassium chloride (KCl) and calcium chloride (CaCl2 ) were measured using the same method as in Experiment 2. The results are shown in Tables 2 and 3.

15. If, in Experiment 3, the chemist had measured the freezing point of Solution 11, the value would most likely be closest to:

Answer and Explanation

Your Answer is

Correct Answer is B

Explanation

According to the data in table 2, it can be speculated that the higher the %KCl, the lower the freezing point.

The %KCl of Solution 11 is greater than the %KCl of Solution 10, so the freezing point of Solution 11 should also be lower than -6.45°C, so first exclude option A;

Then compare the table From Solution 9 and Solution 10 in 2, it can be seen that %KCl increases by 4%, and the freezing point decreases by about 2.15°C, so it is predicted that the freezing point of Solution 11 is about -6.45-2.15=-9, and option B is the closest