Question 1

A piece of lead metal was added to an aqueous solution of copper(II)nitrate, and within a few minutes it was observed that the lead turned black and crumbled, and the blue solution characteristic of copper(II)ions faded.(NOTE: Lead forms a 2+ ion when it reacts.)
Write the net ionic equation for this reaction.

Accepted Answer

The answer of A piece of lead metal was added...

Question 2

Silver chloride (AgCl)has an extremely low solubility in water; therefore, it is a weak electrolyte.

Accepted Answer

Silver chloride (AgCl) has an extremely low solubility in water, which means it dissociates into ions to a very small extent. However, being a salt, if it does dissolve, it dissociates completely into its ions (Ag+ and Cl-), making it a strong electrolyte. The term "weak electrolyte" refers to a substance that only partially dissociates into ions in solution, which is not the case for AgCl.

Question 3

Write balanced molecular and net ionic equations for the reaction that would occur between CuCl₂(aq)and Pb(s).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

Accepted Answer

The answer of Write balanced molecular and net ionic equations...

Question 4

A weak acid or a weak base ionizes completely.

Accepted Answer

A weak acid or a weak base does not ionize completely in water. They only partially ionize or dissociate.

Question 5

The following experiments were carried out and observations recorded.
Expt.#1: copper metal was added to an aqueous solution of silver nitrate
Observation: The copper become coated with a substance.
Expt.#2: lead metal was added to an aqueous solution of copper(II)nitrate
Observation: The lead turned black and crumbled.
Expt.#3: zinc metal was added to an aqueous solution of lead(II)nitrate
Observation: The zinc appeared to fall apart.
Rank the metals from most active to least active.

Accepted Answer

The answer of The following experiments were carried out and...

Question 6

The oxidation number of N in NO is +7.

Accepted Answer

The oxidation number of N in NO is +2, not +7.

Question 7

Sugar dissolves in water, therefore it is a strong electrolyte.

Accepted Answer

Sugar (sucrose) is a non-electrolyte, meaning it does not dissociate into ions in water and does not conduct electricity.

Question 8

Hydrogen is oxidized in the following chemical reaction. H₂ + Cl₂$\rarr$2HCl

Accepted Answer

The presence of Cl indicates that it is the oxidizing agent, and hydrogen is being oxidized in the reaction.

Question 9

If 73.5 mL of 0.200 M KI(aq)was required to precipitate all of the lead(II)ion from an aqueous solution of lead(II)nitrate, how many moles of Pb²⁺ were originally in the solution?

Accepted Answer

The answer of If 73.5 mL of 0.200 M KI(aq)was...

Question 10

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper and the solution turned a blue color characteristic of copper(II)ions.
Write the net ionic equation for this reaction.

Accepted Answer

The answer of A piece of copper metal was added...

Question 11

Write balanced molecular and net ionic equations for the reaction that would occur between Al(s)and Co(NO₃)₂(aq).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

Accepted Answer

The answer of Write balanced molecular and net ionic equations...

Question 12

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel.
Write the balanced chemical equation for this reaction.

Accepted Answer

The answer of A piece of zinc metal was added...

Question 13

Most compounds containing chlorides, bromides, and iodides are soluble except those containing Ag⁺, Hg₂²⁺, and Pb²⁺.

Accepted Answer

This statement is true according to the solubility rules for chlorides, bromides, and iodides. The compounds listed (Ag⁺, Hg₂²⁺, and Pb²⁺) contain ions that form insoluble compounds with these anions.

Question 14

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel.
Write the net ionic equation for this reaction.

Accepted Answer

The answer of A piece of zinc metal was added...

Question 15

The following reaction is an acid-base neutralization reaction. H₂SO₄(aq)+ CaBr₂(aq)$\rarr$CaSO₄(s)+ 2HBr(g)

Accepted Answer

The answer of The following reaction is an acid-base neutralization...

Question 16

A piece of lead metal was added to an aqueous solution of copper(II)nitrate, and within a few minutes it was observed that the lead turned black and crumbled, and the blue solution characteristic of copper(II)ions faded.(NOTE: Lead forms a 2+ ion when it reacts.)
Write the balanced chemical equation for this reaction.

Accepted Answer

The answer of A piece of lead metal was added...

Question 17

The oxidation number of iodine increases by 6 in the following reaction. 2MnO₄^- + I^- + H₂O $\rarr$ 2MnO₂ + IO₃^- + 2OH^-

Accepted Answer

In the reactant side, iodine has an oxidation number of -1 in the I^- molecule. In the product side, iodine has an oxidation number of +5 in the IO₃^- molecule. Therefore, the oxidation number of iodine increases by 6 in the reaction.

Question 18

Write a balanced molecular equation for the reaction that occurs when aqueous solutions of potassium iodide and lead(II)nitrate are combined.

Accepted Answer

The answer of Write a balanced molecular equation for the...

Question 19

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper and the solution turned a blue color characteristic of copper(II)ions.
Write the balanced chemical equation for this reaction.

Accepted Answer

The answer of A piece of copper metal was added...

Question 20

The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq)$\rarr$ AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)

Accepted Answer

The answer of The following equation is an example of...

Quiz 4: Reactions in Aqueous Solution

Silver chloride (AgCl)has an extremely low solubility in water; therefore, it is a weak electrolyte.

Write balanced molecular and net ionic equations for the reaction that would occur between CuCl₂(aq)and Pb(s).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

A weak acid or a weak base ionizes completely.

The oxidation number of N in NO is +7.

Sugar dissolves in water, therefore it is a strong electrolyte.

Hydrogen is oxidized in the following chemical reaction. H₂ + Cl₂ $\rarr$ 2HCl

If 73.5 mL of 0.200 M KI(aq)was required to precipitate all of the lead(II)ion from an aqueous solution of lead(II)nitrate, how many moles of Pb²⁺ were originally in the solution?

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper and the solution turned a blue color characteristic of copper(II)ions. Write the net ionic equation for this reaction.

Write balanced molecular and net ionic equations for the reaction that would occur between Al(s)and Co(NO₃)₂(aq).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Write the balanced chemical equation for this reaction.

Most compounds containing chlorides, bromides, and iodides are soluble except those containing Ag⁺, Hg₂²⁺, and Pb²⁺.

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Write the net ionic equation for this reaction.

The following reaction is an acid-base neutralization reaction. H₂SO₄(aq)+ CaBr₂(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)

The oxidation number of iodine increases by 6 in the following reaction. 2MnO₄^- + I^- + H₂O $\rarr$ 2MnO₂ + IO₃^- + 2OH^-

Write a balanced molecular equation for the reaction that occurs when aqueous solutions of potassium iodide and lead(II)nitrate are combined.

The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq) $\rarr$ AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)

Quiz 4: Reactions in Aqueous Solution

Silver chloride (AgCl)has an extremely low solubility in water; therefore, it is a weak electrolyte.

Write balanced molecular and net ionic equations for the reaction that would occur between CuCl2(aq)and Pb(s).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

A weak acid or a weak base ionizes completely.

The oxidation number of N in NO is +7.

Sugar dissolves in water, therefore it is a strong electrolyte.

Hydrogen is oxidized in the following chemical reaction. H2 + Cl2 →\rarr→ 2HCl

If 73.5 mL of 0.200 M KI(aq)was required to precipitate all of the lead(II)ion from an aqueous solution of lead(II)nitrate, how many moles of Pb2+ were originally in the solution?

A piece of copper metal was added to an aqueous solution of silver nitrate, and within a few minutes it was observed that a grey crystalline solid formed on surface of the copper and the solution turned a blue color characteristic of copper(II)ions. Write the net ionic equation for this reaction.

Write balanced molecular and net ionic equations for the reaction that would occur between Al(s)and Co(NO3)2(aq).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Write the balanced chemical equation for this reaction.

Most compounds containing chlorides, bromides, and iodides are soluble except those containing Ag+, Hg22+, and Pb2+.

A piece of zinc metal was added to an aqueous solution of lead(II)nitrate.After some time it was observed that the zinc metal had appeared to fall apart and a solid had accumulated at the bottom of the reaction vessel. Write the net ionic equation for this reaction.

The following reaction is an acid-base neutralization reaction. H2SO4(aq)+ CaBr2(aq) →\rarr→ CaSO4(s)+ 2HBr(g)

The oxidation number of iodine increases by 6 in the following reaction. 2MnO4- + I- + H2O →\rarr→ 2MnO2 + IO3- + 2OH-

Write a balanced molecular equation for the reaction that occurs when aqueous solutions of potassium iodide and lead(II)nitrate are combined.

The following equation is an example of a net ionic equation. Na+(aq)+ Br-(aq)+ Ag+(aq)+ NO3-(aq) →\rarr→ AgBr(s)+ Na+(aq)+ NO3-(aq)

Write balanced molecular and net ionic equations for the reaction that would occur between CuCl₂(aq)and Pb(s).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

Hydrogen is oxidized in the following chemical reaction. H₂ + Cl₂ $\rarr$ 2HCl

If 73.5 mL of 0.200 M KI(aq)was required to precipitate all of the lead(II)ion from an aqueous solution of lead(II)nitrate, how many moles of Pb²⁺ were originally in the solution?

Write balanced molecular and net ionic equations for the reaction that would occur between Al(s)and Co(NO₃)₂(aq).Be sure to include the correct states in your final equations.If no reaction is expected, write "no reaction."

Most compounds containing chlorides, bromides, and iodides are soluble except those containing Ag⁺, Hg₂²⁺, and Pb²⁺.

The following reaction is an acid-base neutralization reaction. H₂SO₄(aq)+ CaBr₂(aq) $\rarr$ CaSO₄(s)+ 2HBr(g)

The oxidation number of iodine increases by 6 in the following reaction. 2MnO₄^- + I^- + H₂O $\rarr$ 2MnO₂ + IO₃^- + 2OH^-

The following equation is an example of a net ionic equation. Na⁺(aq)+ Br^-(aq)+ Ag⁺(aq)+ NO₃^-(aq) $\rarr$ AgBr(s)+ Na⁺(aq)+ NO₃^-(aq)