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Chapter 4: Problem 16

Specify what ions are present upon dissolving each of the following substances in water: (a) \(\mathrm{MgI}_{2}\), (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\), (c) \(\mathrm{HClO}_{4}\) (d) \(\mathrm{NaCH}_{3} \mathrm{COO}\).

Short Answer

Expert verified
Upon dissolving each of the following substances in water, we obtain the following ions: (a) \( MgI_2 \rightarrow Mg^{2+} + 2 I^{-}\) (b) \( Al(NO_3)_3 \rightarrow Al^{3+} + 3 NO_3^-\) (c) \( HClO_4 \rightarrow H^+ + ClO_4^-\) (d) \( NaCH_3COO \rightarrow Na^+ + CH_3COO^-\)

Step by step solution

01

(a) Dissociation of MgI鈧�

When MgI鈧� (magnesium iodide) is dissolved in water, it dissociates into its ions. Magnesium is in group 2 of the periodic table and has a charge of +2, while iodide is in group 17 (halogens) and has a charge of -1. Therefore, when MgI鈧� dissociates, it forms the following ions: \[ MgI_2 \rightarrow Mg^{2+} + 2 I^{-}\]
02

(b) Dissociation of Al(NO鈧�)鈧�

When Al(NO鈧�)鈧� (aluminum nitrate) is dissolved in water, it dissociates into its ions. Aluminum is in group 13 of the periodic table and has a charge of +3, while the nitrate ion (NO鈧冣伝) has a charge of -1. Therefore, when Al(NO鈧�)鈧� dissociates, it forms the following ions: \[ Al(NO_3)_3 \rightarrow Al^{3+} + 3 NO_3^-\]
03

(c) Dissociation of HClO鈧�

When HClO鈧� (perchloric acid) is dissolved in water, it dissociates into its ions. Hydrogen ion (H鈦�) has a charge of +1, and the perchlorate ion (ClO鈧勨伝) has a charge of -1. Therefore, when HClO鈧� dissociates, it forms the following ions: \[ HClO_4 \rightarrow H^+ + ClO_4^-\]
04

(d) Dissociation of NaCH鈧僀OO

When NaCH鈧僀OO (sodium acetate) is dissolved in water, it dissociates into its ions. Sodium is in group 1 of the periodic table and has a charge of +1, while the acetate ion (CH鈧僀OO鈦�) has a charge of -1. Therefore, when NaCH鈧僀OO dissociates, it forms the following ions: \[ NaCH_3COO \rightarrow Na^+ + CH_3COO^-\]

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Key Concepts

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

Dissociation in Water
When ionic compounds are added to water, they tend to dissociate into their constituent ions. This process is important in chemistry because ions in solution can participate in various reactions.

Ions are charged particles, and when they are free in a solution, they allow the solution to conduct electricity.
  • The process depends on the compound's structure and the attraction between the ions and water molecules.
  • Strong ionic bonds can be overcome by the polar nature of water molecules, which can separate the ions from each other.
This is why the dissociation process is essential for many biological and chemical reactions that require ions in solution.
Magnesium Iodide (MgI鈧�)
Magnesium iodide is composed of magnesium ions (Mg虏鈦�) and iodide ions (I鈦�). When magnesium iodide dissolves in water, it breaks apart into its ions.

The dissociation reaction for magnesium iodide is given by: \[ MgI_2 \rightarrow Mg^{2+} + 2 I^- \]
  • Magnesium ions have a charge of +2 because magnesium is from group 2 of the periodic table.
  • Iodide ions each have a charge of -1, compensating for the +2 charge of magnesium by pairing with two iodide ions.
These ions in water can participate in a range of chemical reactions.
Aluminum Nitrate (Al(NO鈧�)鈧�)
Aluminum nitrate consists of aluminum ions (Al鲁鈦�) and nitrate ions (NO鈧冣伝).
When it dissolves in water, it splits into its respective ions:\[ Al(NO_3)_3 \rightarrow Al^{3+} + 3 NO_3^- \]
  • Since aluminum is found in group 13 of the periodic table, it has a +3 charge.
  • Nitrate ions carry a single negative charge each, so three nitrate ions are needed to balance the charge of one aluminum ion.
The dissociation of aluminum nitrate is crucial for processes involving nitrogen compounds.
Perchloric Acid (HClO鈧�)
Perchloric acid is an important chemical that dissociates in water to form hydrogen ions (H鈦�) and perchlorate ions (ClO鈧勨伝).

This dissociation reaction is expressed as: \[ HClO_4 \rightarrow H^+ + ClO_4^- \]
  • The hydrogen ion (H鈦�) is the main contributor to the acidic nature of the solution.
  • The perchlorate ion carries a single negative charge.
Perchloric acid is a strong acid, meaning it dissociates completely in water, which is essential for various industrial and research applications.
Sodium Acetate (NaCH鈧僀OO)
Sodium acetate is composed of sodium ions (Na鈦�) and acetate ions (CH鈧僀OO鈦�).
When this compound dissolves in water, it dissociates as follows:\[ NaCH_3COO \rightarrow Na^+ + CH_3COO^- \]
  • Sodium is in group 1, which contributes to its +1 charge as an ion.
  • The acetate ion is a common organic ion found in many biological and chemical processes.
Sodium acetate's dissociation in water is significant in buffer solutions, which are used to maintain stable pH levels in various applications.

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Most popular questions from this chapter

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid; (b) chromium with hydrobromic acid; (c) tin with hydrochloric acid; (d) aluminum with formic acid, \(\mathrm{HCOOH}\).

The mass percentage of chloride ion in a 25.00-mL sample of seawater was determined by titrating the sample with silver nitrate, precipitating silver chloride. It took \(42.58 \mathrm{~mL}\) of \(0.2997 \mathrm{M}\) silver nitrate solution to reach the equivalence point in the titration. What is the mass percentage of chloride ion in the seawater if its density is \(1.025 \mathrm{~g} / \mathrm{mL} ?\)

Which of the following solutions is the most basic? (a) \(0.6 \mathrm{M} \mathrm{NH}_{3}\), (b) \(0.150 \mathrm{M} \mathrm{KOH}\), (c) \(0.100 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\). Explain.

You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion \(\left(\mathrm{CrO}_{4}{ }^{2-}\right)\) and the oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}{ }^{2-}\right)\). You are given \(0.01 \mathrm{M}\) solutions (A, B, C, D) of four water-soluble salts: $$ \begin{array}{lll} \hline \text { Solution } & \text { Solute } & \text { Color of Solution } \\ \hline \mathrm{A} & \mathrm{Na}_{2} \mathrm{CrO}_{4} & \text { Yellow } \\ \mathrm{B} & \left(\mathrm{NH}_{4}\right)_{2} \mathrm{C}_{2} \mathrm{O}_{4} & \text { Colorless } \\ \mathrm{C} & \mathrm{AgNO}_{3} & \text { Colorless } \\ \mathrm{D} & \mathrm{CaCl}_{2} & \text { Colorless } \\ \hline \end{array} $$ When these solutions are mixed, the following observations are made: $$ \begin{array}{lll} \hline \text { Expt } & \text { Solutions } & \\ \text { Number } & \text { Mixed } & \text { Result } \\ \hline 1 & \mathrm{~A}+\mathrm{B} & \text { No precipitate, yellow solution } \\\ 2 & \mathrm{~A}+\mathrm{C} & \text { Red precipitate forms } \\ 3 & \mathrm{~A}+\mathrm{D} & \text { No precipitate, yellow solution } \\ 4 & \mathrm{~B}+\mathrm{C} & \text { White precipitate forms } \\ 5 & \mathrm{~B}+\mathrm{D} & \text { White precipitate forms } \\ 6 & \mathrm{C}+\mathrm{D} & \text { White precipitate forms } \\ \hline \end{array} $$ (a) Write a net ionic equation for the reaction that occurs in each of the experiments. (b) Identify the precipitate formed, if any, in each of the experiments. (c) Based on these limited observations, which ion tends to form the more soluble salts, chromate or oxalate?

A sample of \(1.50 \mathrm{~g}\) of lead(II) nitrate is mixed with \(125 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) sodium sulfate solution. (a) Write the chemical equation for the reaction that occurs. (b) Which is the limiting reactant in the reaction? (c) What are the concentrations of all ions that remain in solution after the reaction is complete?
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