Q: Which of the following best describes an Arrhenius acid?

A substance that produces H\textsuperscript{+} ions in aqueous solution.

Q: Which of the following is the correct calculation for the number of moles of H$$_3PO$_4 in 14.20 mL of 0.141 M $$solution?

$$0.01420 \text{ L} \times 0.141 \text{ mol/L}$$

Question 1

Which of the following best describes an Arrhenius acid?

Accepted Answer

A substance that produces H	extsuperscript{+} ions in aqueous solution.

Question 2

Which of the following is the correct net ionic equation for the reaction between hydrochloric acid and sodium hydroxide?

Accepted Answer

$$\mathrm{H^+} (aq) + \mathrm{OH^-} (aq) \rightarrow \mathrm{H_2O} (l)$$

Question 3

A student mixes 0.10 M HCl with 0.10 M NaOH in equal volumes. What is the expected pH of the resulting solution?

Accepted Answer

pH $$= 7$$

Question 4

Which of the following substances is a strong electrolyte in water?

Accepted Answer

KClO$$_4$$

Question 5

Which of the following best describes the equivalence point in a titration?

Accepted Answer

The point where the amount of titrant added results in complete neutralization of the analyte.

Question 6

A reaction between sodium carbonate and hydrochloric acid produces which of the following products?

Accepted Answer

Water, a salt, and a gas

Question 7

Which of the following is a weak electrolyte?

Accepted Answer

NH$$_3$$

Question 8

What is the mass of NaOH required to precipitate all Cd$$^{2+}$$ ions from 35.0 mL of 0.500 M Cd(NO$$_3$$)$$_2$$ solution? (Molar mass NaOH = 40.00 g/mol)

Accepted Answer

1.40 g

Question 9

Which of the following statements about titrations is FALSE?

Accepted Answer

The endpoint is always exactly the same as the equivalence point.

Question 10

How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)$$_2$$ solution?

Accepted Answer

84.2 mL

Question 11

Which of the following best explains why strong acids are also strong electrolytes?

Accepted Answer

They completely ionize in water.

Question 12

A 0.205-g sample of a mixture of Na$$_2SO$_4$$ and K$$_2SO$_4$$ produces 0.298 g of BaSO$$_4$$ upon reaction with excess BaCl$$_2. $$What is the mass percent of SO$$_4$$^{2-}$$ in the sample? (Molar mass BaSO_4$ = 233.4 g/mol, SO$$_$$4^{2-} = 96.06 g/$$mol)

Accepted Answer

60.0%

Question 13

Which of the following is the correct balanced equation for the neutralization of H$$_2SO$_4$$ with NaOH?

Accepted Answer

$$\mathrm{H_2SO_4} + 2\mathrm{NaOH} \rightarrow \mathrm{Na_2SO_4} + 2\mathrm{H_2O}$$

Question 14

Which solution contains the highest concentration of potassium ions?

Accepted Answer

0.15 M K$$_2$$CrO$$_4$$

Question 15

Which of the following is a requirement for a successful titration?

Accepted Answer

The exact reaction between titrant and analyte must be known.

Question 16

Which of the following best describes a Lewis base?

Accepted Answer

An electron pair donor

Question 17

A student is performing a titration and observes the indicator change color before the equivalence point is reached. What is the most likely result?

Accepted Answer

The calculated concentration of analyte will be too low.

Question 18

Which of the following is NOT a product of the reaction between NaHCO$$_3$$ and HCl?

Accepted Answer

NaOH (base)

Question 19

Which of the following best describes the role of an indicator in a titration?

Accepted Answer

It changes color at or near the equivalence point.

Question 20

Which of the following is the correct calculation for the number of moles of H$$_3PO$_4 in 14.20 mL of 0.141 M $$solution?

Accepted Answer

$$0.01420 	ext{ L} 	imes 0.141 	ext{ mol/L}$$

Acid-Base Reactions and Solution Chemistry: Study Notes

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