Q: A solution has a pH of 5.23. What is the concentration of hydrogen ions, $$[H^+]$$, in the solution?

$$5.9 \times 10$$^{-6}$$\ \mathrm{M}$$

Question 1

Which element is represented by the following electron configuration: $$1s^2$$ $$2s^2$$ $$2p^6$$ $$3s^2$$ $$3p^6$$ $$4s^2$$ $$3d^6$$?

Accepted Answer

Iron (Fe)

Question 2

Refer to the orbital diagram shown. How many unpaired electrons are present in the 3d sublevel?

Accepted Answer

5

Question 3

Which of the following molecules, based on their Lewis structures, exhibits hydrogen bonding as its strongest intermolecular force?

Accepted Answer

Water

Question 4

Given the Lewis structure for ammonia (NH$$_3$$), what is the molecular geometry and approximate bond angle?

Accepted Answer

Trigonal pyramidal, 107°

Question 5

Which of the following best describes the bond between the oxygen and hydrogen atoms within a water molecule?

Accepted Answer

Polar covalent

Question 6

A sample of gas occupies 42 L at STP. What will its volume be at 855 torr and 40°C? (Use $$P_1V_1/T_1$ = P_2V_2/T_2$)

Accepted Answer

$$43\ \mathrm{L}$$

Question 7

Which of the following statements about intermolecular forces is correct?

Accepted Answer

London dispersion forces are the weakest of the three main types.

Question 8

A solution has a pH of 5.23. What is the concentration of hydrogen ions, $$[H^+]$$, in the solution?

Accepted Answer

$$5.9 	imes 10$$^{-6}$$\ \mathrm{M}$$

Question 9

Which of the following best explains why N$$_2$$ has a very low boiling point?

Accepted Answer

It has only London dispersion forces.

Question 10

If you have 300 mL of a 4.0 M NaCl solution and dilute it with 200 mL of water, what is the new molarity?

Accepted Answer

$$2.4\ \mathrm{M}$$

Question 11

Which of the following is true about the heating curve shown in the image?

Accepted Answer

The substance melts at 80°C and boils at 218°C.

Question 12

Which of the following best describes a supersaturated solution?

Accepted Answer

A solution that contains more solute than can theoretically dissolve at a given temperature.

Question 13

Which of the following pairs is a correct conjugate acid-base pair?

Accepted Answer

H$$_2SO$_4$$ and HSO$$_4^-$$

Question 14

What is the molarity of a solution prepared by dissolving 10.0 g of NaCl (molar mass = 58.44 g/mol) in 750 mL of solution?

Accepted Answer

$$0.23\ \mathrm{M}$$

Question 15

Which of the following gases would have the highest vapor pressure at room temperature?

Accepted Answer

CH$$_4$$

Question 16

Which of the following best describes the relationship between molecular size and the strength of London dispersion forces?

Accepted Answer

As molecular size increases, London dispersion forces increase.

Question 17

A 1.6-g sample of metal requires 5.8 J to change its temperature from 23°C to 41°C. What is the specific heat of the metal? Is it gold? ($$q = m \cdot c \cdot \Delta T$$; specific heat of gold = $$0.13\ \mathrm{J/g}^\circ\mathrm{C})$$

Accepted Answer

$$0.20\ \mathrm{J/g}^\circ\mathrm{C}$$; No, it is not gold.

Question 18

Which of the following best explains why water has a higher boiling point than dimethyl ether, even though both have similar molar masses?

Accepted Answer

Water forms hydrogen bonds, which are stronger than the dipole-dipole forces in dimethyl ether.

Question 19

If the pOH of a solution is 11, what is the pH and is the solution acidic or basic?

Accepted Answer

pH = 3; acidic

Comprehensive Study Guidance for Honors Chemistry Final Review

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