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Chapter 3: Problem 15

Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when the compound dissolves in water. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (c) NiS (b) \(\mathrm{CuSO}_{4}\) (d) \(\mathrm{BaBr}_{2}\)

Short Answer

Expert verified
(a) Soluble: produces \(\mathrm{Na}^+\) and \(\mathrm{CO}_3^{2-}\). (c) NiS insoluble. (b) Soluble: produces \(\mathrm{Cu}^{2+}\) and \(\mathrm{SO}_4^{2-}\). (d) Soluble: produces \(\mathrm{Ba}^{2+}\) and \(\mathrm{Br}^-\).

Step by step solution

01

Determine Solubility of Na2CO3

Sodium carbonate, \(\mathrm{Na}_2\mathrm{CO}_3\), is soluble in water. According to solubility rules, compounds containing sodium (\(\mathrm{Na}^+\)) ions are generally soluble in water.
02

Identify Ions from Na2CO3 Dissolution

When \(\mathrm{Na}_2\mathrm{CO}_3\) dissolves in water, it dissociates into two sodium ions \((\mathrm{Na}^+)\) and one carbonate ion \((\mathrm{CO}_3^{2-})\).
03

Determine Solubility of NiS

Nickel sulfide, \(\mathrm{NiS}\), is insoluble in water. Sulfides are typically insoluble, except for those of the alkali metals and a few others.
04

Determine Solubility of CuSO4

Copper (II) sulfate, \(\mathrm{CuSO}_4\), is soluble in water. Sulfates are generally soluble, except for a few exceptions like barium, lead, and calcium.
05

Identify Ions from CuSO4 Dissolution

When \(\mathrm{CuSO}_4\) dissolves in water, it dissociates into one copper ion \((\mathrm{Cu}^{2+})\) and one sulfate ion \((\mathrm{SO}_4^{2-})\).
06

Determine Solubility of BaBr2

Barium bromide, \(\mathrm{BaBr}_2\), is soluble in water. Bromides are generally soluble except for those combined with silver, lead, and mercury.
07

Identify Ions from BaBr2 Dissolution

When \(\mathrm{BaBr}_2\) dissolves in water, it dissociates into one barium ion \((\mathrm{Ba}^{2+})\) and two bromide ions \((\mathrm{Br}^-)\).

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Key Concepts

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

Ionic Compounds
Ionic compounds are composed of positively and negatively charged ions. These ions are held together by strong electrostatic forces known as ionic bonds. Let's dive into what makes an ionic compound unique and significant in chemistry:
  • The positive ions, called cations, are typically metal atoms that have lost electrons.
  • Negative ions, called anions, are usually non-metals that have gained electrons.
  • The chemical formula of an ionic compound reflects the balance of positive and negative charges to ensure the compound is neutral overall.
For example, in \(\mathrm{Na}_2\mathrm{CO}_3\), you have two sodium ions \((\mathrm{Na}^+)\) and one carbonate ion \[\left(\mathrm{CO}_3^{2-}\right)\], balancing out the charges perfectly. Understanding the makeup of ionic compounds is essential in predicting their behavior in water and their solubility characteristics.
Dissociation
When an ionic compound dissolves in water, it undergoes a process called dissociation. This involves splitting into its individual ions. Dissociation in water is a key topic as it provides insights into chemical reactivity and environmental behaviors:
  • The water molecules, which are polar, surround the individual ions and pull them away from the lattice structure of the compound.
  • This leads to free moving ions in solution, capable of conducting electricity.
Consider the dissolution of \(\mathrm{CuSO}_4\) in water. It dissociates into copper ions \(\mathrm{Cu}^{2+}\) and sulfate ions \[\mathrm{SO}_4^{2-}\]. This dissociation is crucial for the compound's ability to participate in further chemical reactions or processes.
Solubility Rules
Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. These rules are based on empirical observations of various compounds. Understanding solubility rules is critical for chemistry calculations and practical applications.
Key solubility rules include:
  • Compounds with alkali metal ions (like \(\mathrm{Na}^+\)) and ammonium ions \((\mathrm{NH}_4^+\) are soluble.
  • Most nitrates \(\mathrm{NO}_3^-\) and acetates (\(\mathrm{CH}_3\mathrm{COO}^-\) are soluble.
  • Halides such as chloride, bromide, and iodide are generally soluble, except when paired with silver, lead, or mercury.
  • Sulfates are soluble, with notable exceptions including those of barium, lead, and calcium.
For instance, \(\mathrm{Na}_2\mathrm{CO}_3\) is soluble due to the presence of sodium ions, following these solubility rules.
Water-Soluble Compounds
Water-soluble compounds easily dissolve in water, forming a solution that has uniform composition. This solubility is crucial in various fields from biochemistry to environmental science.
Characteristics of water-soluble compounds include:
  • The ability to dissolve in water, forming aqueous solutions suitable for chemical reactions.
  • Participation in biological systems where transport in the blood or cellular fluid is necessary.
  • Influence on natural processes like the transport of minerals in soil.

An example is \(\mathrm{BaBr}_2\), which dissolves, providing barium ions \(\mathrm{Ba}^{2+}\) and bromide ions \(\mathrm{Br}^-\). Understanding water solubility allows for prediction of how substances interact in nature and technology.

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Most popular questions from this chapter

Equal amounts of two acids- -HCl and HCO \(_{2} \mathrm{H}\) (formic acid) - are placed in solution. When equilibrium has been achieved, the HCl solution has a much greater electrical conductivity than the HCO,H solution. Which reaction is more product-favored at equilibrium? $$\begin{aligned}\mathrm{HCl}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \\\\\mathrm{HCO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) & \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HCO}_{2}^{-}(\mathrm{aq})\end{aligned}$$

Write balanced chemical equations for the following reactions. (a) The reaction of aluminum and iron(III) oxide to form iron and aluminum oxide (known as the thermite reaction, page 142). (b) The reaction of carbon and water at high temperature to form a mixture of gaseous \(\mathrm{CO}\) and \(\mathrm{H}_{2}\) (known as water gas and once used as a fuel). (c) The reaction of liquid silicon tetrachloride and magnesium forming silicon and magnesium chloride. This is one step in the preparation of ultrapure silicon used in the semiconductor industry.

Complete and balance the equations for the following acid-base reactions. Name the reactants and products. (a) \(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow\) (b) \(\mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{NH}_{3}(\mathrm{aq}) \rightarrow\)

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species \((\mathrm{s}, \ell, \mathrm{aq}, \text { or } \mathrm{g})\). $$\mathrm{CdCl}_{2}+\mathrm{NaOH} \rightarrow \mathrm{Cd}(\mathrm{OH})_{2}+\mathrm{NaCl}$$

The presence of arsenic in a sample that may also contain another Group 5 A element, antimony, can be confirmed by first precipitating the \(\mathrm{As}^{3+}\) and \(\mathrm{Sb}^{3+}\) ions as yellow solid \(\mathrm{As}_{2} \mathrm{S}_{3}\) and orange solid \(\mathrm{Sb}_{2} \mathrm{S}_{3} .\) If aqueous HCl is then added, only \(\mathrm{Sb}_{2} \mathrm{S}_{3}\) dissolves, leaving behind solid \(\mathrm{As}_{2} \mathrm{S}_{3} .\) The \(\mathrm{As}_{2} \mathrm{S}_{3}\) can then be dissolved using aqueous HNO \(_{3}\) $$\begin{aligned} 3 \mathrm{As}_{2} \mathrm{S}_{3}(\mathrm{s})+10 \mathrm{HNO}_{3}(\mathrm{aq})+4 \mathrm{H}_{2} \mathrm{O}(\ell) & \rightarrow \\ 6 \mathrm{H}_{3} \mathrm{AsO}_{4}(\mathrm{aq})+10 \mathrm{NO}(\mathrm{g})+9 \mathrm{S}(\mathrm{s}) \end{aligned}$$ Finally, the presence of arsenic is confirmed by adding \(\mathrm{AgNO}_{3}\) to the solution of \(\mathrm{H}_{3} \mathrm{AsO}_{4}\) to precipitate a reddish brown solid \(\mathrm{Ag}_{x} \mathrm{AsO}_{y} .\) The composition of this solid is As, \(16.199 \%\) and \(\mathrm{Ag}, 69.964 \%\) (a) What are the oxidation numbers of As, \(S,\) and \(N\) in the reaction of \(\mathrm{As}_{2} \mathrm{S}_{3}\) with nitric acid? (b) What is the formula of the reddish brown solid \(\mathrm{Ag}_{\mathrm{x}} \mathrm{A} \mathrm{s} \mathrm{O}_{\mathrm{y}} ?\)
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