Q: A solution is prepared by dissolving 110.0 grams of Fe2(SO4)3 in enough water to make 750.0 mL of solution. What is the molarity of Fe2(SO4)3? (Molar mass = 399.9 g/mol)

$$0.337\ \text{M Fe}_2(\text{SO}_4)_3$$

Q: Iron(III) carbonate decomposes to form iron(III) oxide and carbon dioxide. What mass (in grams) of iron(III) carbonate must be decomposed to collect 10.4 liters of CO2 at STP? (Molar mass Fe2(CO3)3 = 399.9 g/mol)

$$83.2\ \text{g Fe}_2(\text{CO}_3)_3$$

Q: Which of the following is the correct formula for calculating the molarity (M) of a solution?

$$M = \frac{\text{moles of solute}}{\text{liters of solution}}$$

Question 1

Which of the following best defines molality?

Accepted Answer

Moles of solute per kilogram of solvent

Question 2

A solution is prepared by dissolving 110.0 grams of Fe2(SO4)3 in enough water to make 750.0 mL of solution. What is the molarity of Fe2(SO4)3? (Molar mass = 399.9 g/mol)

Accepted Answer

$$0.337\ 	ext{M Fe}_2(	ext{SO}_4)_3$$

Question 3

What is the molarity of a solution made by diluting 25.00 mL of 1.75 M NaCl to a final volume of 500.0 mL?

Accepted Answer

$$0.0875\ 	ext{M NaCl}$$

Question 4

How many mL of 0.70 M NaCl solution are needed to prepare 25.00 mL of 0.175 M NaCl solution?

Accepted Answer

$$6.25\ 	ext{mL}$$

Question 5

Calculate the weight/weight percent of a solution made by dissolving 6.99 g H2SO4 in enough water to make 100.0 g of solution.

Accepted Answer

$$6.99\%\ 	ext{w/w}$$

Question 6

A 37.7% w/w aqueous solution of HCl has a density of 1.19 g/mL. What is the molality of HCl in this solution? (Molar mass = 36.46 g/mol)

Accepted Answer

$$13.3\ 	ext{mol/kg}$$

Question 7

What volume (in mL) of 0.89 M H2SO4 solution is needed to neutralize 10.0 mL of 1.00 M NaOH solution? (Reaction: $$	ext{H}_2	ext{SO}_4 + 2	ext{NaOH} ightarrow 	ext{Na}_2	ext{SO}_4 + 2	ext{H}_2	ext{O})$$

Accepted Answer

$$5.62\ 	ext{mL}$$

Question 8

Calculate the volume (in mL) of 3.13% w/w NaCl solution needed to react with 3.75 g Pb(NO3)2 according to the reaction: $$	ext{Pb(NO}_3)_2 + 2	ext{NaCl} ightarrow 2	ext{NaNO}_3 + 	ext{PbCl}_2 ($$Molar mass NaCl = 58.44 g/mol, solution density = 1.04 g/mL).

Accepted Answer

$$211\ 	ext{mL}$$

Question 9

What volume of 18.0% w/w (NH4)2SO4 solution is needed to react with 18.5 grams of a mixture that is 7.4% w/w AgNO3? (Reaction: $$2	ext{AgNO}_3 + (	ext{NH}_4)_2	ext{SO}_4 ightarrow 2	ext{NH}_4	ext{NO}_3 + 	ext{Ag}_2	ext{SO}_4$$; solution density = 1.10 g/mL, molar mass AgNO3 = 169.87 g/mol, molar mass (NH4)2SO4 = 132.14 g/mol)

Accepted Answer

$$15.6\ 	ext{mL}$$

Question 10

Calculate the pressure (in atm) exerted by 3.58 moles of O2 in a 3.7 liter cylinder at 25°C.

Accepted Answer

$$24.0\ 	ext{atm}$$

Question 11

A gas was collected in a 3.60 liter flask at 800 torr. Calculate the pressure (in atm) the same gas would exert if the flask was transferred to a 3.60 liter flask at 100 liter flask.

Accepted Answer

$$0.029\ 	ext{atm}$$

Question 12

The mass of 560 mL of an unknown gas is 1.60 grams at STP. Which of the following is a possibility for the unknown gas?

Accepted Answer

SO2

Question 13

Iron(III) carbonate decomposes to form iron(III) oxide and carbon dioxide. What mass (in grams) of iron(III) carbonate must be decomposed to collect 10.4 liters of CO2 at STP? (Molar mass Fe2(CO3)3 = 399.9 g/mol)

Accepted Answer

$$83.2\ 	ext{g Fe}_2(	ext{CO}_3)_3$$

Question 14

Calculate the volume (in liters) of NH3 at a pressure of 1.00 atm and a temperature of 25°C that can be prepared by the reaction of 56.0 grams of N2 with excess H2: $$	ext{N}_2 + 3	ext{H}_2 ightarrow 2	ext{NH}_3$$

Accepted Answer

$$101\ 	ext{L NH}_3$$

Question 15

Which of the following statements about STP (Standard Temperature and Pressure) is correct?

Accepted Answer

STP is defined as 0°C and 1 atm

Question 16

Which of the following is the correct formula for calculating the molarity (M) of a solution?

Accepted Answer

$$M = \frac{	ext{moles of solute}}{	ext{liters of solution}}$$

Question 17

A student needs to prepare 100 mL of 0.250 M NaCl solution. How many grams of NaCl are required? (Molar mass NaCl = 58.44 g/mol)

Accepted Answer

$$1.46\ 	ext{g}$$

Question 18

Which of the following best describes a solution with a concentration of 1.0 M?

Accepted Answer

1.0 mole of solute per 1.0 liter of solution

General Chemistry Study Guide: Solutions, Molarity, Stoichiometry, and Gas Laws

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