Q: A solution is prepared by dissolving 0.134 grams of yellow #5 dye in water and diluting to 100.0 mL. What is the molarity of the solution if the molar mass of yellow #5 is 534 g/mol?

$$2.51 \times 10$$^{-3}$$\ \text{M}$$

Question 1

A 100.0 mL sample of 1.000 M KCl solution is combined with 100.0 mL of 0.250 M AlCl$$_3$$ solution. What is the molarity of Cl$$^-$$ ions in the final mixture?

Accepted Answer

$$0.625\ 	ext{M}$$

Question 2

Which of the following conditions least favors the process of dissolution?

Accepted Answer

Stronger solute-solute attraction, weaker solvent-solute attraction, weaker solvent-solvent attraction

Question 3

Nonpolar solutes dissolve more readily in nonpolar solvents than in polar solvents because:

Accepted Answer

The induced dipole of the solute molecule creates an induced dipole in the solvent molecule and London dispersion forces occur.

Question 4

How many additional grams of potassium nitrate would need to be added at minimum to maintain a saturated solution if the temperature is raised from 10$$^	ext{o}C to 50$^	ext{o}C$$? (Assume the solution is not supersaturated at any time.)

Accepted Answer

$$62\ 	ext{grams}$$

Question 5

About how many milliliters of water need to be added to 50.0 mL of a 0.50 M solution of NaOH to obtain a 0.10 M solution?

Accepted Answer

$$250\ 	ext{mL}$$

Question 6

Which procedure is recommended for reading the level of an aqueous solution in a burette or graduated cylinder?

Accepted Answer

Keep eye level with the bottom of the meniscus and record that reading

Question 7

A stock solution of 12.0 M sulfuric acid is made available. What is the best procedure to make up 100.0 mL of 4.00 M sulfuric acid using the stock solution and water prior to mixing?

Accepted Answer

Add 33.3 mL of 12.0 M acid to the flask and then dilute it with 66.7 mL of water.

Question 8

Toluene, C$$_6H$_5CH$_3$$, is only sparingly soluble (0.52 g/L) in water. Which statement best describes the molecular reason for the low solubility between water and toluene?

Accepted Answer

There are dipole-induced dipole and London dispersion interactions between water and toluene.

Question 9

The reaction $$	ext{NaOCl(aq)} + 2\ 	ext{H}_2	ext{O(aq)} ightarrow 	ext{Cl}_2	ext{(g)} + 	ext{NaCl(aq)} + 	ext{H}_2	ext{O(l)}$$ occurs when an excess of HCl(aq) is added to 100.0 mL of NaOCl(aq) of unknown concentration. If the reaction goes to completion and 0.010 mol of Cl$$_2(g) is $$produced, what was the molarity of the NaOCl(aq) solution?

Accepted Answer

$$0.010\ 	ext{M}$$

Question 10

What is the relative order of conductivity of these three substances: I. Water, II. 0.1 M aqueous NH$$_4$$ solution, III. 0.1 M aqueous NH$$_4Cl $$solution?

Accepted Answer

I \u003c II \u003c III

Question 11

A student prepared solutions with different concentrations and filled five cuvettes, each containing one of the solutions. The absorbance of each solution was measured and recorded. The student plotted absorbance versus concentration, as shown in the figure above. What is the explanation for the error of the 3rd data point?

Accepted Answer

The cuvette used for the solution had not been wiped clean before being put in the spectrophotometer.

Question 12

Which of the following best explains why oil and water do not mix?

Accepted Answer

Oil is mostly made up of nonpolar compounds and water is a polar molecule, so they cannot form hydrogen bonds.

Question 13

A solution is prepared by dissolving 0.134 grams of yellow #5 dye in water and diluting to 100.0 mL. What is the molarity of the solution if the molar mass of yellow #5 is 534 g/mol?

Accepted Answer

$$2.51 	imes 10$$^{-3}$$\ 	ext{M}$$

Question 14

Which of the following is NOT a reason why Beer's Law is not appropriate for a NaCl solution?

Accepted Answer

NaCl does not absorb visible light in the range used for Beer's Law measurements.

Question 15

Which of the following best describes the hydration of ions in aqueous solution?

Accepted Answer

Water molecules orient so that the oxygen atom faces cations and the hydrogen atoms face anions.

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