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Chapter 1: Problem 2

If solutions containing equal amounts of \(\mathrm{AgNO}_{3}\) and \(\mathrm{KCl}\) are mixed, what is the identity of the spectator ions? (A) \(\mathrm{Ag}^{+}, \mathrm{NO}_{3}^{-}, \mathrm{K}^{+},\) and \(\mathrm{Cl}^{-}\) (B) \(\mathrm{Ag}^{+}\) and \(\mathrm{Cl}^{-}\) (C) \(\mathrm{K}^{+}\) and \(\mathrm{Ag}^{+}\) (D) \(\mathrm{K}^{+}\) and \(\mathrm{NO}_{3}^{-}\)

Short Answer

Expert verified
The spectator ions in the reaction are K+ and NO3-. Therefore, the correct answer is (D) K+ and NO3-.

Step by step solution

01

Breaking compounds into ions

The first step is to dissociate the compounds into their constituent ions. Dissociation of AgNO3 gives Ag+ and NO3- ions and dissociation of KCl gives K+ and Cl- ions.
02

Forming the reaction

The next step is to visualize the reaction that occurs when the two solutions are mixed. The equation below represents the reaction that occurs: \n AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3(aq) . This is a precipitation reaction, as AgCl is an insoluble compound that precipitates out of the solution.
03

Identifying the spectator ions

In a precipitation reaction, the ions that do not participate in the formation of the precipitate are called spectator ions. These ions remain in the solution and do not undergo any change. Looking at the equation, we can see that the K+ and NO3- ions do not participate in the reaction. Thus, these are the spectator ions.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Precipitation Reaction
When two aqueous solutions are mixed together, sometimes an insoluble solid forms, which is called a precipitate. This occurs in a specific type of chemical reaction known as a **precipitation reaction**. In this process, ions from the two solutions interact to form a compound that does not dissolve in water and settles down as a solid.
For example, when a solution of silver nitrate ( AgNO_3 ) is mixed with a solution of potassium chloride ( KCl ), a precipitation reaction takes place. Here, silver chloride ( AgCl ) is the insoluble product that forms and precipitates.
This concept is important in chemistry as it helps in the separation and purification of substances and has applications in areas such as analytical chemistry, medicine, and environmental science.
Ionic Equation
To deeply understand chemical reactions like the one between AgNO_3 and KCl , it's helpful to use **ionic equations**. These equations break down the compounds into their individual ions and help identify which ions participate in the reaction, and which do not.
For the silver nitrate ( AgNO_3 ) and potassium chloride ( KCl ) reaction, the complete ionic equation looks like this: Ag^+(aq) + NO_3^-(aq) + K^+(aq) + Cl^-(aq) -> AgCl(s) + K^+(aq) + NO_3^-(aq) .
In this equation, it's easier to see which ions recombine to form the solid precipitate (AgCl), and which ions remain unchanged in the solution. According to the ionic equation, spectator ions are the ones that do not participate in the chemical change.
AgNO3 Dissociation
AGNO\(_3\) is an ionic compound and in an aqueous solution, it dissociates into ions. This process is called **dissociation**. As the compound dissociates, it separates into positively charged silver ions (Ag^+) and negatively charged nitrate ions (NO_3^-).
This dissociation is crucial for the reaction with potassium chloride (KCl) to occur. Without this breakdown into ions, the reaction producing silver chloride (AgCl) as the precipitate would not transpire.
Understanding dissociation helps in predicting the outcomes of chemical reactions and plays a significant role in determining the solubility of substances.
KCl Dissociation
Similarly, potassium chloride ( KCl ) is an ionic compound that also dissociates when dissolved in water. During this **dissociation**, KCl separates into potassium ions ( K^+ ) and chloride ions ( Cl^- ).
This dissociation allows the chloride ions to combine with silver ions from AgNO_3 , leading to the formation of the precipitate AgCl .
The leftover ions, K^+ and NO_3^- , are the spectator ions. These ions do not engage in the precipitation process and remain dissolved in the solution, representing the concept of non-reacting ions in chemistry.

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Most popular questions from this chapter

Directions: Questions 1-3 are long free-response questions that require about 23 minutes each to answer and are worth 10 points each. Write your response in the space provided following each question. Examples and equations may be included in your responses where appropriate. For calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Pay attention to significant figures. The unbalanced reaction between potassium permanganate and acidified iron (II) sulfate is a redox reaction that proceeds as follows: $$\mathrm{H}^{+}(a q)+\mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-(a q)} \rightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$$ (a) Provide the equations for both half-reactions that occur below: (i) Oxidation half-reaction (ii) Reduction half-reaction (b) What is the balanced net ionic equation? A solution of 0.150 M potassium permanganate is placed in a buret before being titrated into a flask containing 50.00 mL of iron (II) sulfate solution of unknown concentration. The following data describes the colors of the various ions in solution: $$\begin{array}{|c|c|}\hline \text { Ion } & {\text { Color in solution }} \\\ \hline \mathrm{H^{+ }} & {\text { Colorless }} \\ \hline \mathrm{Fe}^{2+} & {\text { Pale Green }} \\ \hline \mathrm{MnO}_{4^{-}} & {\text {Dark Purple }} \\ \hline \mathrm{Mn}^{2+} & {\text { Colorless }} \\ \hline \mathrm{Fe}^{3+} & {\text { Yellow }} \\ \hline \mathrm{K}^{+} & {\text {Colorless }} \\ \hline \mathrm{SO}_{4}^{2-} & {\text { Colorless }} \\\ \hline\end{array}$$ (c) Describe the color of the solution in the flask at the following points: (i) Before titration begins (ii) During titration prior to the endpoint (iii) At the endpoint of the titration (d) (i) If 15.55 mL of permanganate are added to reach the endpoint, what is the initial concentration of the iron (II) sulfate? (ii) The actual concentration of the \(\mathrm{FeSO}_{4}\), is 0.250 \(M\) . Calculate the percent error. (e) Could the following errors have led to the experimental result deviating in the direction that it did? You must justify your answers quantitatively. (i) 55.0 \(\mathrm{mL}\) of \(\mathrm{FeSO}_{4}\) was added to the flask prior to titration instead of 50.0 mL . (ii) The concentration of the potassium permanganate was actually 0.160 \(M\) instead of 0.150 \(M\) .

In general, do metals or nonmetals from the same period have higher ionization energies? Why? (A) Metals have higher ionization energies because they usually have more protons than nonmetals. (B) Nonmetals have higher ionization energies because they are larger than metals and harder to ionize. (C) Metals have higher ionization energies because there is less electron shielding than there is in nonmetals. (D) Nonmetals have higher ionization energies because they are closer to having filled a complete energy level.

The following mechanism is proposed for a reaction: \(\begin{array}{ll}{2 \mathrm{A} \rightarrow \mathrm{B}} & {\text { (fast equilibrium) }} \\ {\mathrm{C}+\mathrm{B} \rightarrow \mathrm{D}} & {\text { (slow) }} \\ {\mathrm{D}+\mathrm{A} \rightarrow \mathrm{E}} & {\text { (fast) }}\end{array}\) Which of the following is the correct rate law for compete reaction? (A) Rate \(=k[\mathrm{C}]^{2}[\mathrm{B}]\) (B) Rate \(=k\left[\mathrm{Cl}[\mathrm{A}]^{2}\right.\) (C) Rate \(=k[\mathrm{C}][\mathrm{A}]^{3}\) (D) Rate \(=k[\mathrm{D}][\mathrm{A}]\)

The six carbon atoms in a benzene molecule are shown in different resonance forms as three single bonds and three double bonds. If the length of a single carbon-carbon bond is 154 pm and the length of a double of a single carbon bond is \(133 \mathrm{pm},\) what length would be expected for the carbon-carbon bonds in benzene? (A) 126 \(\mathrm{pm}\) (B) 133 \(\mathrm{pm}\) (C) 140 \(\mathrm{pm}\) (D) 154 \(\mathrm{pm}\)

Choose the correct net ionic equation representing the reaction that occurs when solutions of potassium carbonate and copper (I) chloride are mixed. (A) \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+2 \mathrm{CuCl}(a q) \rightarrow 2 \mathrm{KCl}(a q)+\mathrm{Cu}_{2} \mathrm{CO}_{3}(s)\) (B) \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+2 \mathrm{CuCl}(a q) \rightarrow 2 \mathrm{KCl}(\mathrm{s})+\mathrm{Cu}_{2} \mathrm{CO}_{3}(a q)\) (C) \(\mathrm{CO}_{3}^{2-}+2 \mathrm{Cu}^{+} \rightarrow \mathrm{Cu}_{2} \mathrm{CO}_{3}\) (D) \(\mathrm{CO}_{3}^{2-}+\mathrm{Cu}^{2+} \rightarrow \mathrm{CuCO}_{3}(s)\)
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