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Chapter 8: Problem 9

Select the correct option if it is known that \(K_{\text {sp }}(\mathrm{AgCl})>K_{\text {sp }}(\mathrm{AgBr})>K_{\mathrm{sp}}(\) AgI \()\)

Short Answer

Expert verified
AgCl is the most soluble, AgI is the least soluble, and AgBr has intermediate solubility.

Step by step solution

01

Understanding the Solubility Product Constant (Ksp)

The solubility product constant, denoted as Ksp, is a measure of the solubility of a compound in a solvent. A larger Ksp value indicates a more soluble compound.
02

Comparing the Ksp values

If the Ksp value for AgCl is greater than the Ksp for AgBr, and the Ksp for AgBr is greater than the Ksp for AgI, this signifies that AgCl is the most soluble, followed by AgBr, and AgI is the least soluble of the three.
03

Putting Ksp values in context

Since Ksp values reflect how much of a substance can dissociate in solution to form its constituent ions, the substance with the highest Ksp will produce the most ions in solution. Hence, the option that reflects AgCl being the most soluble and AgI being the least soluble is the correct one.

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Key Concepts

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

Solubility of Ionic Compounds
The solubility of ionic compounds is a crucial concept in chemistry, referring to how well a compound can be dissolved in a solvent to form a homogeneous mixture or solution. When an ionic compound dissolves in water, it dissociates into its constituent cations and anions. This dissolving process is governed by the concept of the solubility product constant (Ksp).

The Ksp is an equilibrium constant that quantifies the maximum amount of the compound that can dissolve in a solution before the solution becomes saturated. The greater the Ksp value, the more soluble the compound is; thus, a high Ksp means that more ions will be in solution, leading to better conductivity and more chemical reactivity in the solution.

Solubility is influenced by various factors, including temperature, the nature of the solvent, and the presence of other ions in the solution. Understanding the solubility of different ionic compounds helps predict and explain their behavior in various chemical processes, such as precipitation reactions and the formation of complexes.
Comparing Solubility
When it comes to comparing the solubility of various ionic compounds, the Ksp is an essential tool. It allows chemists to get an idea of their relative solubility. For instance, by knowing the Ksp values, one can deduce that a compound with a higher Ksp is more soluble than one with a lower Ksp.

However, one must be cautious when comparing solubility across different ions or compounds. While Ksp provides a general guideline, solubility is not only determined by Ksp but also by the ionic compound's specific properties, such as ionic size and the solvent’s properties.

In the given exercise, AgCl, AgBr, and AgI have different Ksp values, meaning they have varying solubilities in water. AgCl with the highest Ksp is the most soluble, indicating that it dissociates the most in solution followed by AgBr, and AgI with the lowest Ksp is the least soluble. This ranking helps predict the behavior of these compounds in a mixture or during a reaction.
Ionic Product and Precipitation
The concept of the ionic product is closely related to Ksp and solubility. The ionic product, often denoted as Q, is the product of the concentrations of the ionic species in a solution at any given moment. When the ionic product (Q) exceeds the solubility product constant (Ksp), it indicates that the solution is supersaturated, and precipitation is likely to occur.

Precipitation is the process in which ions in a supersaturated solution combine to form a solid, which then falls out or precipitates from the solution. Precipitation reactions play a vital role in fields ranging from industrial synthesis to water treatment.

For a solution to remain unsaturated and free of precipitates, the ionic product must be less than or equal to the Ksp. In practice, comparing the ionic product to the Ksp assists in predicting whether a precipitate will form when different ionic solutions are mixed. For example, if one were to combine solutions of AgNO3 and NaCl, knowing the Ksp of AgCl would help determine if silver chloride will precipitate.

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Most popular questions from this chapter

A solution containing \(1.0 \mathrm{M}\) each of \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{AgNO}_{3}, \mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}\) is being electrolysed using inert electrodes. The values of standard electrode potential are: \(\mathrm{Ag}^{+}\left|\mathrm{Ag}=0.80 \mathrm{~V}, \mathrm{Hg}^{2+}\right| \mathrm{Hg}=0.79 \mathrm{~V}\) \(\mathrm{Cu}^{2+}\left|\mathrm{Cu}=0.34 \mathrm{~V}, \mathrm{Mg}^{2+}\right| \mathrm{Mg}=-2.37 \mathrm{~V}\) With increasing voltage, the sequence of deposit of metals on the cathode will be (a) \(\mathrm{Ag}, \mathrm{Hg}, \mathrm{Cu}, \mathrm{Mg}\) (b) \(\mathrm{Mg}, \mathrm{Cu}, \mathrm{Hg}, \mathrm{Ag}\) (c) \(\mathrm{Ag}, \mathrm{Mg}, \mathrm{Cu}\) (d) \(\mathrm{Cu}, \mathrm{Hg}, \mathrm{Ag}\)

The value of equilibrium constant for a feasible cell reaction must be (a) \(\leq 1\) (b) Zero \((\mathrm{c})=1\) (d) \(>1\)

Astudent made the followingobservations in the laboratory: (I) Clean copper metal did not react with \(1 \mathrm{M}-\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution. (II) Clean lead metal dissolves in \(1 \mathrm{M}\) \(-\mathrm{AgNO}_{3}\) solution and crystals of Ag metal appeared. (III) Clean silver metal did not react with \(1 \mathrm{M}-\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) solution. The order of decreasing reducing character of the three metals is (a) \(\mathrm{Cu}>\mathrm{Pb}>\mathrm{Ag}\) (b) \(\mathrm{Cu}>\mathrm{Ag}>\mathrm{Pb}\) (c) \(\mathrm{Pb}>\mathrm{Cu}>\mathrm{Ag}\) (d) \(\mathrm{Pb}>\mathrm{Ag}>\mathrm{Cu}\)

The EMF of the cell: \(\mathrm{Hg}(1) \mid \mathrm{Hg}_{2} \mathrm{Cl}_{2}(\mathrm{~s})\), \(\mathrm{KCl}\) sol. \((1.0 \mathrm{~N}) \mid\) Quinohydrone \(\mid \mathrm{Pt}\), is \(0.210 \mathrm{~V}\) at \(298 \mathrm{~K}\). What is the \(\mathrm{pH}\) of the quinohydrone solution, the potential of the normal calomel electrode is \(0.279 \mathrm{~V}\) and \(E^{\circ}\) for the quinohydrone electrode is \(0.699 \mathrm{~V}\), both at the same temperature. \([2.303 R T / F=0.06]\) (a) \(3.5\) (b) \(7.0\) (c) \(1.85\) (d) \(-3.5\)

A Tl'|Tlcouple was prepared by saturating \(0.10 \mathrm{M}-\mathrm{KBr}\) with TIBr and allowing \(\mathrm{Tl}^{+}\) ions form the insoluble bromide to equilibrate. This couple was observed to have a potential \(-0.444 \mathrm{~V}\) with respect to \(\mathrm{Pb}^{2+} \mid \mathrm{Pb}\) couple in which \(\mathrm{Pb}^{2+}\) was \(0.10 \mathrm{M} .\) What is the \(K_{\mathrm{sp}}\) of TIBr. [Given: \(E_{\mathrm{Pb}^{2+} \mid \mathrm{Pb}}^{\circ}=-0.126 \mathrm{~V}, E_{\mathrm{T}^{+} \mid \mathrm{T}}^{o}=-0.336 \mathrm{~V}\) \(\log 2.5=0.4,2.303 R T / F=0.06]\) (a) \(4.0 \times 10^{-6}\) (b) \(2.5 \times 10^{-4}\) (c) \(4.0 \times 10^{-5}\) (d) \(6.3 \times 10^{-3}\)
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