Chemistry Chapter 4 Practice Exam

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Questions and Answers

How much PbSO4 can be produced by the addition of 25 mL of a 0.50 M solution of aluminum sulfate to excess lead(II) nitrate?

3.8 g

3.00 g

11.4 g (correct)

1.26 g

What volume of 0.0250 M HNO3 solution is needed to fully react with 12.5 mL of a 0.0100 M Ca(OH)2 solution?

15.0 mL

20.0 mL (correct)

10.0 mL

12.5 mL

Based on the balanced reaction, how much Cl2 is needed to react with 60.0 g of NaOH?

14.6 g

106 g

26.6 g (correct)

142 g

What is the concentration of a solution after 25.00 mL of a 3.50 M NaOH solution is diluted to 500.0 mL?

0.175 M Signup and view all the answers

What is the oxidation number of sulfur in Na2S2O8?

7 Signup and view all the answers

Which of the following metals would dissolve in a solution of Ni(NO3)2?

Zinc Signup and view all the answers

How much 0.500 M HNO3 is required to dissolve 27.0 g of Al?

0.167 L Signup and view all the answers

What is the mass of NaCl produced when 60.0 g of NaOH react with Cl2?

53.2 g Signup and view all the answers

What is the maximum amount of PbI2 that may precipitate when 2.57 g of Pb(NO3)2 and 2.28 g of KI are reacted?

4.44 g Signup and view all the answers

How many of the following ionic compounds are soluble in water: BaSO4, AgBr, Sr(NO3)2, PbS, Na2CO3?

Four are soluble Signup and view all the answers

Which statement accurately describes the effect of dissolving sodium nitrite in water?

Weakly basic, nitrite ion partially reacts with water to form OH- ions Signup and view all the answers

What is the net ionic reaction for the reaction between potassium chloride and lead(II) nitrate?

Pb2+ (aq) + 2 Cl- (aq) → PbCl2 (s) Signup and view all the answers

What is the molarity of a sulfuric acid solution titrated with 2.19 M NaOH using 16.25 mL of NaOH?

0.712 M Signup and view all the answers

Which ionic compounds from the following list are insoluble in water? 1. BaSO4 2. AgBr 3. Sr(NO3)2 4. PbS 5. Na2CO3

1 and 4 Signup and view all the answers

How does sodium nitrite behave when it is dissolved in water?

Forms a weakly basic solution Signup and view all the answers

In the reaction of Pb(NO3)2 and KI, what products are formed?

PbI2 and KNO3 Signup and view all the answers

Which compound would most likely produce the least number of ions when dissolved in water?

NH3 Signup and view all the answers

Which statement about electrolytes is correct?

All strong electrolytes are water-soluble ionic compounds. Signup and view all the answers

Which compounds act as weak acids when dissolved in water?

CH3COOH and HClO Signup and view all the answers

Which combination of compounds will result in a precipitate when mixed in water?

Ba(NO3)2 and (NH4)2S Signup and view all the answers

What best describes the acid-base properties of NH4Cl when dissolved in water?

Weak electrolyte, weak base Signup and view all the answers

What are the molarities of all ions in the solution after the metathesis reaction between AgNO3 and CaCl2 is complete?

[Ag+] = 0.50 M, [NO3-] = 0.50 M, [Ca2+] = none, [Cl-] = none Signup and view all the answers

Which of the following is true regarding weak acids in water?

They partially ionize, resulting in a weakly electrolytic solution. Signup and view all the answers

Which solution would likely contain the highest concentration of ions when dissolved?

NaOH Signup and view all the answers

Study Notes

Ionic Compounds and Solutions

NH3 (ammonia) is expected to contain the least number of ions when dissolved due to being a weak electrolyte.
Strong electrolytes include ionic compounds that fully dissociate in water, while weak electrolytes only partially dissociate.
Common strong electrolytes: all water-soluble ionic compounds.
Weak acids like acetic acid (CH3COOH) and hypochlorous acid (HClO) yield weakly electrolytic solutions.

Precipitation Reactions

Mixing MgCl2 and NaOH can result in a precipitate.
Ba(NO3)2 and (NH4)2S will also produce a precipitate.
Solubility rules help determine the formation of precipitates in aqueous solutions.

Metathesis Reactions

A metathesis reaction involves the exchange of ions between two compounds to form new compounds.
For the reaction between AgNO3 and CaCl2, the final ion concentrations, after the reaction completes and assuming a total volume of 2 L, can be calculated.

Acid-Base Reactions

Sodium nitrite (NaNO2) in solution is weakly basic; it partially reacts with water to form hydroxide ions (OH-).
Titration problems often require knowledge of stoichiometry to find the molarity of an acid based on neutralization with a base.

Precipitation Calculations

When calculating the maximum amount of precipitate formed, molar masses of compounds involved are essential.
The reaction of Pb(NO3)2 with KI leads to the formation of PbI2.

Solubility in Water

Not all ionic compounds are soluble in water. For example:
- BaSO4 and PbS are generally insoluble.
- Sr(NO3)2 and Na2CO3 are soluble.

Net Ionic Reactions

The net ionic equation simplifies aqueous reactions by removing the spectator ions and focusing on the formation of solid precipitates.

Molarity and Dilution

The concentration of a solution can change upon dilution. If a concentrated solution is diluted, the final concentration can be calculated using the formula C1V1 = C2V2.

Oxidation States and Activity Series

The oxidation state of sulfur in Na2S2O8 can be calculated based on known oxidation states of oxygen and other elements.
The activity series helps predict the reactivity of metals; metals like zinc and manganese can displace nickel from its ionic solution.

Balancing Redox Reactions

Oxidation-reduction reactions involve electron transfer. Balancing these reactions often requires half-reaction methods.
Calculating the amount of reactants needed to dissolve a specific mass of a metal involves stoichiometric calculations related to the molarity of the solution used.

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Description

Test your knowledge with this practice exam focused on Chapter 4 of your chemistry course. This quiz covers key concepts related to solutions and electrolytes, including the behavior of various compounds dissolved in water. Prepare to identify which solutions contain the least number of ions and evaluate statements regarding strong electrolytes.