Q: What is the molarity of a solution prepared by dissolving 0.50 mol of NaCl in enough water to make 2.0 L of solution?

$$M = \frac{0.50\ \text{mol}}{2.0\ \text{L}} = 0.25\ \text{M}$$

Q: A student needs to prepare 500.0 mL of 0.250 M HNO$$_3$$ from a stock solution of 2.00 M HNO$$_3. $$What volume of the stock solution should be used?

$$V_1$$ = \frac{$$M_2$$ $$V_2$$}{$$M_1$$} = \frac{0.250 \times 500.0}{2.00} = 62.5\ \text{mL}$$

Q: Which of the following is the correct net ionic equation for the reaction between AgNO$$_3(aq) $$and NaCl(aq)?

$$\text{Ag}^+(aq) + \text{Cl}^-(aq) \rightarrow \text{AgCl}(s)$$

Q: A 0.762-g sample of vinegar is titrated with 0.2250 M NaOH. The buret reading changes from 0.31 mL to 24.48 mL. What is the percent by mass of acetic acid in the sample? (Molar mass of acetic acid = 60.05 g/mol)

$$\text{Percent} = \frac{(0.2250\ \text{mol/L}) \times (24.17\ \text{mL} \times \frac{1\ \text{L}}{1000\ \text{mL}}) \times 60.05\ \text{g/mol}}{0.762\ \text{g}} \times 100 \approx 42.7\%$$

Q: Which of the following is the correct balanced molecular equation for the neutralization of H$$_2SO$_4(aq) $$with KOH(aq)?

$$\text{H}_2\text{SO}_4(aq) + 2\text{KOH}(aq) \rightarrow 2\text{H}_2\text{O}(l) + \text{K}_2\text{SO}_4(aq)$$

Q: Which of the following is a correct net ionic equation for the reaction between Ba(NO$$_3$$)$$_2(aq) $$and Na$$_2SO$_4(aq$$)?

$$\text{Ba}^{2+}(aq) + \text{SO}_4$$^{2-}$$(aq) \rightarrow \text{BaSO}_4(s)$$

Q: Which of the following reactions is a redox reaction?

$$2\text{Na}(s) + 2\text{H}_2\text{O}(l) \rightarrow 2\text{NaOH}(aq) + \text{H}_2(g)$$

Q: Which of the following is a correct example of a gas-evolution reaction?

$$\text{K}_2\text{SO}_3(aq) + 2\text{HCl}(aq) \rightarrow 2\text{KCl}(aq) + \text{H}_2\text{O}(l) + \text{SO}_2(g)$$

Q: A mixture is made by combining 50.0 mL of 0.20 M NaCl and 50.0 mL of 0.40 M Na$$_2SO$_4. $$What is the final concentration of Na$$^+$$ ions in the mixture?

$$[\text{Na}^+] = \frac{(0.20\ \text{mol/L} \times 50.0\ \text{mL} \times \frac{1}{1000}) + (0.40\ \text{mol/L} \times 50.0\ \text{mL} \times \frac{1}{1000} \times 2)}{0.100\ \text{L}} = 0.60\ \text{M}$$

Question 1

Which of the following statements best describes a solution?

Accepted Answer

A solution is a homogeneous mixture where the majority component is the solvent and the minority component is the solute.

Question 2

What is the molarity of a solution prepared by dissolving 0.50 mol of NaCl in enough water to make 2.0 L of solution?

Accepted Answer

$$M = \frac{0.50\ 	ext{mol}}{2.0\ 	ext{L}} = 0.25\ 	ext{M}$$

Question 3

A student needs to prepare 500.0 mL of 0.250 M HNO$$_3$$ from a stock solution of 2.00 M HNO$$_3. $$What volume of the stock solution should be used?

Accepted Answer

$$V_1$$ = \frac{$$M_2$$ $$V_2$$}{$$M_1$$} = \frac{0.250 	imes 500.0}{2.00} = 62.5\ 	ext{mL}$$

Question 4

Which of the following compounds is expected to be soluble in water according to the solubility rules?

Accepted Answer

Na$$_2CO$_3$$

Question 5

Which of the following is a strong electrolyte?

Accepted Answer

NaOH (sodium hydroxide)

Question 6

Which of the following is the correct net ionic equation for the reaction between AgNO$$_3(aq) $$and NaCl(aq)?

Accepted Answer

$$	ext{Ag}^+(aq) + 	ext{Cl}^-(aq) ightarrow 	ext{AgCl}(s)$$

Question 7

Which of the following acids is classified as a strong acid?

Accepted Answer

HNO$$_3 ($$nitric acid)

Question 8

A 0.762-g sample of vinegar is titrated with 0.2250 M NaOH. The buret reading changes from 0.31 mL to 24.48 mL. What is the percent by mass of acetic acid in the sample? (Molar mass of acetic acid = 60.05 g/mol)

Accepted Answer

$$	ext{Percent} = \frac{(0.2250\ 	ext{mol/L}) 	imes (24.17\ 	ext{mL} 	imes \frac{1\ 	ext{L}}{1000\ 	ext{mL}}) 	imes 60.05\ 	ext{g/mol}}{0.762\ 	ext{g}} 	imes 100 \approx 42.7\%$$

Question 9

Which of the following is the correct balanced molecular equation for the neutralization of H$$_2SO$_4(aq) $$with KOH(aq)?

Accepted Answer

$$	ext{H}_2	ext{SO}_4(aq) + 2	ext{KOH}(aq) ightarrow 2	ext{H}_2	ext{O}(l) + 	ext{K}_2	ext{SO}_4(aq)$$

Question 10

Which of the following is a correct net ionic equation for the reaction between Ba(NO$$_3$$)$$_2(aq) $$and Na$$_2SO$_4(aq$$)?

Accepted Answer

$$	ext{Ba}^{2+}(aq) + 	ext{SO}_4$$^{2-}$$(aq) ightarrow 	ext{BaSO}_4(s)$$

Question 11

Which of the following is the correct oxidation state of nitrogen in NO$$_3^-$$?

Accepted Answer

$$+5$$

Question 12

Which of the following reactions is a redox reaction?

Accepted Answer

$$2	ext{Na}(s) + 2	ext{H}_2	ext{O}(l) ightarrow 2	ext{NaOH}(aq) + 	ext{H}_2(g)$$

Question 13

Which species acts as the oxidizing agent in the reaction: $$2	ext{Na}(s) + 2	ext{H}_2	ext{O}(l) ightarrow 2	ext{NaOH}(aq) + 	ext{H}_2(g)$$?

Accepted Answer

H$$_2O(l)$$

Question 14

Which of the following is a correct example of a gas-evolution reaction?

Accepted Answer

$$	ext{K}_2	ext{SO}_3(aq) + 2	ext{HCl}(aq) ightarrow 2	ext{KCl}(aq) + 	ext{H}_2	ext{O}(l) + 	ext{SO}_2(g)$$

Question 15

A mixture is made by combining 50.0 mL of 0.20 M NaCl and 50.0 mL of 0.40 M Na$$_2SO$_4. $$What is the final concentration of Na$$^+$$ ions in the mixture?

Accepted Answer

$$[	ext{Na}^+] = \frac{(0.20\ 	ext{mol/L} 	imes 50.0\ 	ext{mL} 	imes \frac{1}{1000}) + (0.40\ 	ext{mol/L} 	imes 50.0\ 	ext{mL} 	imes \frac{1}{1000} 	imes 2)}{0.100\ 	ext{L}} = 0.60\ 	ext{M}$$

Question 16

Which of the following is the correct molecular equation for the precipitation reaction between Pb(NO$$_3$$)$$_2(aq) $$and KCl(aq)?

Accepted Answer

$$	ext{Pb(NO}_3)_2(aq) + 2	ext{KCl}(aq) ightarrow 	ext{PbCl}_2(s) + 2	ext{KNO}_3(aq)$$

Question 17

Which of the following is the correct oxidation state for sulfur in SO$$_4$$^{2-}$$?

Accepted Answer

$$+6$$

Module 6: Introduction to Solutions and Aqueous Reactions – Study Notes

Guida di studio - Domande di pratica

Study guide - Flashcard