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AP Chemistry : Chemical Reactions

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Example Question #1 : Net Ionic Equations

What is the net ionic equation for the reaction that occurs when sodium chloride is mixed with silver nitrate.

Possible Answers:

Na⁺ (aq) + NO₃^- (aq) -> NaNO₃ (s)

Ag⁺(aq) + Cl^- (aq) -> AgCl (s)

NaCl (aq) + AgNO₃ (aq) -> NaNO₃ (s) + AgCl (aq)

NaCl (aq) + AgNO₃ (aq) -> NaNO₃ (aq) + AgCl (s)

NaCl (aq) + AgNO3 (aq) -> NaNO₃ (aq) + AgCl (aq)

Correct answer:

Ag⁺(aq) + Cl^- (aq) -> AgCl (s)

Explanation:

Only the Ag and Cl ions are reacting to form solid silver chloride.

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Example Question #1 : Net Ionic Equations

What is the net ionic equation that occurs when sodium chloride is mixed with potassium nitrate?

Possible Answers:

NaCl (aq) + KNO₃ (aq) -> NaNO₃ (s) + KCl (aq)

NaCl (aq) + KNO3 (aq) -> NaNO₃ (aq) + KCl (aq)

No Reaction

Na⁺ (aq) + NO₃^- (aq) -> NaNO₃ (s)

NaCl (aq) + KNO₃ (aq) -> KNO₃ (aq) + KCl (s)

Correct answer:

No Reaction

Explanation:

Since no precipitation is predicted by the solubility rules, there will be no reaction.

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Example Question #1 : Chemical Reactions

What is the net ionic reaction when potassium carbonate is mixed with Calcium bromide?

Possible Answers:

2 K₂CO₃ (aq) + CaBr₂ (aq) -> 2 KBr (aq) + CaCO₃(aq)

Ca²⁺ (aq) + CO₃^2- (aq) -> CaCO₃(s)

2 K₂CO₃ (aq) + CaBr₂ (aq) -> 2 KBr (aq) + CaCO₃(s)

2 K₂CO₃ (aq) + CaBr₂(aq) -> 2 KBr (s) + CaCO₃(aq)

2 K⁺ (aq) + Br^- (aq) -> 2 KBr (s)

Correct answer:

Ca²⁺ (aq) + CO₃^2- (aq) -> CaCO₃(s)

Explanation:

Only the calcium and carbonate ions are reacting according to the solubility rules to form calcium carbonate.

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Example Question #4 : Net Ionic Equations

What is the net ionic reaction when a solution of Cd(NO₃)₂ is reacted with (NH₄)₂S?

Possible Answers:

NH4⁺ (aq) + NO₃^- (aq) -> NH₄NO₃ (s)

Cd(NO₃)₂ (aq) + (NH₄)₂S (aq) -> CdS (s) + 2 NH₄NO₃ (aq)

Cd(NO₃)₂ (aq) + (NH₄)₂S (aq) -> CdS (aq) + 2 NH₄NO₃(aq)

Cd²⁺(aq) + S^2- -> CdS (s)

Cd(NO₃)₂ (aq) + (NH₄)₂S (aq) -> CdS (s) + 2 NH₄NO₃(aq)

Correct answer:

Cd²⁺(aq) + S^2- -> CdS (s)

Explanation:

Only Cd and S ions are interacting according to the solubility rules to form a solid precipitant.

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Example Question #1 : Net Ionic Equations

What is the net ionic reaction when a solution of rubidium sulfate is mixed with barium hydroxide?

Possible Answers:

Ba²⁺ (aq) + SO₄^2- (aq) -> BaSO4 (s)

Rb₂SO₄ (aq) + Ba(OH)₂ (aq) -> 2 RbOH (s) + BaSO₄ (aq)

Rb₂SO₄ (aq) + Ba(OH)₂ (aq) -> 2 RbOH (aq) + BaSO₄ (s)

No Reaction

Rb⁺ (aq) + OH^- (aq) -> RbOH (s)

Correct answer:

Ba²⁺ (aq) + SO₄^2- (aq) -> BaSO4 (s)

Explanation:

Only the Ba and sulfate ions will react according to the solubility rules.

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Example Question #22 : Chemical Reactions

$CaCO_{3} (s) \rightarrow CaO (s) + CO_{2} (g)$

The reaction above could be classified as __________.

Possible Answers:

oxidation-reduction

single displacement

decomposition

synthesis

decomposition and oxidation-reduction

Correct answer:

decomposition

Explanation:

When one molecule is converted into two or more smaller molecules, the reaction is considered a decomposition reaction. In this example, none of the elements under go a change in oxidation number, so this is not an oxidation-reduction reaction. (Calcium is always , oxygen is always , and carbon remains throughout the reaction.)

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Example Question #2 : Chemical Reactions

Which of the following represents a combustion reaction?

Possible Answers:

$\small 2Cu(NO_{3})_{2} \rightarrow 2CuO + 4NO_{2} + O_{2}$

$\small CH_{4} + O_{2} \rightarrow CO_{2} + H_{2}O + heat$

$\small 2NaCl + 2H_{2}O \rightarrow 2NaOH + H_{2} + Cl_{2}$

$\small HCl + H_{2}O \rightarrow H_{3}O^{+} + Cl^{-}$

Correct answer:

$\small CH_{4} + O_{2} \rightarrow CO_{2} + H_{2}O + heat$

Explanation:

Combustion reactions always produce $\small CO_{2} + H_{2}O$ and excess heat. Depending on the molecule that is oxidized by oxygen, which in this case was methane $\small (CH_{4})$ , the ratios between $\small CO_{2}$ and $\small H_{2}O$ can vary.

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Example Question #3 : Chemical Reactions

What is the chemical formula of the salt formed when a chemist mixes solvated Potassium and Arsenic ions in solution?

Possible Answers:

$KAs_2$

$K_2As$

$KAs_3$

$KAs$

$K_3As$

Correct answer:

$K_3As$

Explanation:

Potassium is a Group I element, so to get to a filled valence shell, it will lost one electron, yielding $K^+$ .

Arsenic is a Group 5 element, so it needs to gain three electrons to obtain a filled valence shell, yielding $As^{-3}$ .

In order to balance out the charges, the resultant salt will be $K_3As$ .

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Example Question #41 : Chemical Reactions

What is the net ionic equation for the ion exchange reaction between ferrous sulfate and calcium iodide? Assume all compounds are soluble.

Possible Answers:

$FeSO_4 + CaI \rightarrow FeI +CaSO_4$

$FeSO_4 + CaI_2 \rightarrow FeI_2 +CaSO_4$

$Fe_2SO_4 + CaI_2 \rightarrow 2FeI +CaSO_4$

$Fe(SO_4)_2 + CaI_2 \rightarrow FeI_2 +Ca(SO_4)_2$

None of the available answers

Correct answer:

$FeSO_4 + CaI_2 \rightarrow FeI_2 +CaSO_4$

Explanation:

First, we must know what ferrous sulfate is. Ferrous refers to $Fe^{2+}$ , and sulfate has the formula $SO_4^{-2}$ . When we combine the two together we get FeSO_4 .

Calcium is a divatent cation and iodide is a monovalent anion, so their salt is CaI_2 . The ion exchange reaction is then:

$FeSO_4 + CaI_2 \rightarrow FeI_2 +CaSO_4$

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Example Question #5 : Chemical Reactions

Select the net ionic equation from this molecular reaction:

$Ba(NO_{3})_{2} (aq) + K_{2}SO_{4} (aq) \rightarrow 2KNO_{3} (aq) + BaSO_{4} (s)$

Possible Answers:

$Ba^{2+} (aq) + 2K^{+} (aq) + SO_{4}^{2-} (aq) \rightarrow 2K^{+} (aq) + BaSO_{4} (s)$

None of the other choices

$2K^{+} (aq)+SO_{4}^{2-}(aq)\rightarrow K_{2}SO_{4} (aq)$

$Ba^{2+} (aq) + SO_{4}^{2-} (aq) \rightarrow BaSO_{4} (s)$

$K^{+} (aq) + NO_{3}^{-} (aq) \rightarrow KNO_{3} (aq)$

Correct answer:

$Ba^{2+} (aq) + SO_{4}^{2-} (aq) \rightarrow BaSO_{4} (s)$

Explanation:

The net ionic equation is derived by removing all spectator ions from the total ionic equation (in which all ions are listed). To put it another way, the net ionic equation involves only the ions that participate in a reaction which, in this case, is the precipitation of barium sulfate.

Begin by writing all aqueous compounds in their dissociated (ionic) forms.

$Ba(NO_{3})_{2} (aq) + K_{2}SO_{4} (aq) \rightarrow 2KNO_{3} (aq) + BaSO_{4} (s)$

$Ba^{2+}+2NO_3^-+2K^++SO_4^{2-}\rightarrow2K^++2NO_3^-+BaSO_4(s)$

Cancel out any ions that appear in equal quantities on both sides of the equation. In this case, we can cancel the nitrate and potassium ions.

$Ba^{2+}+SO_4^{2-}\rightarrow BaSO_4(s)$

This is our net ionic equation.

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AP Chemistry : Chemical Reactions

Study concepts, example questions & explanations for AP Chemistry

All AP Chemistry Resources

Example Questions

Example Question #1 : Net Ionic Equations

Example Question #1 : Net Ionic Equations

Example Question #1 : Chemical Reactions

Example Question #4 : Net Ionic Equations

Example Question #1 : Net Ionic Equations

Example Question #22 : Chemical Reactions

Example Question #2 : Chemical Reactions

Example Question #3 : Chemical Reactions

Example Question #41 : Chemical Reactions

Example Question #5 : Chemical Reactions

All AP Chemistry Resources

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