Question 1

Which of the following best describes the role of a reducing agent in a redox reaction?

Accepted Answer

It loses electrons and is oxidized.

Question 2

A student prepares a solution by dissolving 5.00 g of NaCl (molar mass = 58.44 g/mol) in enough water to make 250.0 mL of solution. What is the molarity of the solution?

Accepted Answer

$$0.342\ \mathrm{M}$$

Question 3

Which of the following metals will NOT be oxidized by Zn$$^{2+}$$ ions in solution, according to the activity series?

Accepted Answer

Copper (Cu)

Question 4

What is the correct name for the compound CuS?

Accepted Answer

Copper(II) sulfide

Question 5

A 10.0 mL sample of 0.500 M HCl is diluted to a final volume of 100.0 mL. What is the final concentration of HCl?

Accepted Answer

$$0.0500\ \mathrm{M}$$

Question 6

Which of the following statements about acids and bases is TRUE?

Accepted Answer

Acids are proton donors and bases are proton acceptors.

Question 7

In a titration, 25.0 mL of 0.200 M NaOH is required to neutralize 50.0 mL of HCl. What is the concentration of the HCl solution?

Accepted Answer

$$0.100\ \mathrm{M}$$

Question 8

Which laboratory glassware is most appropriate for preparing a solution of known molarity?

Accepted Answer

Volumetric flask

Question 9

A solution is prepared by diluting 10.0 mL of 1.00 M stock solution to a final volume of 100.0 mL. What is the molarity of the diluted solution?

Accepted Answer

$$0.100\ \mathrm{M}$$

Question 10

Which of the following best explains why the reaction Cu(s) + 2 Ag$$^+(aq$$) → Cu$$^{2+}(aq) + 2 Ag(s) is $$spontaneous, but the reverse reaction is not?

Accepted Answer

Copper is higher than silver in the activity series and is more easily oxidized.

Question 11

What is the oxidation state of sulfur in the compound CS$$_2$$?

Accepted Answer

$$-2$$

Question 12

Which of the following is a correct balanced equation for the neutralization of sulfuric acid with sodium hydroxide?

Accepted Answer

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

Question 13

A chemist adds excess silver nitrate to 100.0 mL of a chloride solution and obtains 0.287 g of AgCl precipitate. What is the molarity of Cl$$^- in $$the original solution? (Molar mass AgCl = 143.32 g/mol)

Accepted Answer

$$0.0200\ \mathrm{M}$$

Question 14

Which of the following best describes the equivalence point in an acid-base titration?

Accepted Answer

The point where the amount of acid equals the amount of base in moles.

Question 15

If you dilute 5.00 mL of a 0.200 M solution to 20.00 mL, what is the final concentration?

Accepted Answer

$$0.0500\ \mathrm{M}$$

Question 16

Which of the following is a property of strong acids such as sulfuric acid (H$$_2SO$_4$$)?

Accepted Answer

Strongly dehydrating and can cause severe burns.

Question 17

A titration requires 30.0 mL of 0.150 M NaOH to neutralize 25.0 mL of H$$_2SO$_4. $$What is the molarity of the H$$_2SO$_4$$ solution? (Balanced equation: $$\mathrm{H_2SO_4} + 2\ \mathrm{NaOH} \rightarrow \mathrm{Na_2SO_4} + 2\ \mathrm{H_2O})$$

Accepted Answer

$$0.0900\ \mathrm{M}$$

Reactions in Aqueous Solution, Solution Concentration, and Titration: Study Guide

Guida di studio - Domande di pratica

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