/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 3 Explain the terms soluble and in... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 3

Explain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound.

Short Answer

Expert verified
Soluble compounds dissolve in solvents; insoluble compounds do not. Lead chloride ( ext{PbCl}_2) is insoluble.

Step by step solution

01

Understanding Solubility

Solubility refers to the ability of a substance to dissolve in a solvent. A compound is soluble if it dissolves in the solvent, forming a homogenous mixture at the molecular level. Conversely, a compound is insoluble if it does not dissolve, resulting in a heterogeneous mixture with distinct phases.
02

Reviewing Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. Some general rules include: most nitrate ( ext{NO}_3^-) salts are soluble, most salts containing alkali metal ions ( ext{Li}^+, ext{Na}^+, ext{K}^+, etc.) and the ammonium ion ( ext{NH}_4^+) are soluble, and most chloride ( ext{Cl}^-), bromide ( ext{Br}^-), and iodide ( ext{I}^-) salts are soluble except those of silver ( ext{Ag}^+), lead ( ext{Pb}^{2+}), and mercury ( ext{Hg}_2^{2+}).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Soluble Compounds
Soluble compounds are substances that have the ability to dissolve in a solvent, such as water, forming a uniform solution. When you add a soluble compound to a solvent, it disperses evenly at the molecular level. This property is vital for many everyday processes, like making a cup of tea or a bath with dissolved salts.
  • Solubility can depend on various factors like temperature, pressure, and the nature of the solvent.
  • For example, stirring sugar into warm water will allow it to dissolve more quickly than in cold water.
Soluble compounds play a significant role in chemical reactions, especially in aqueous solutions where they often serve as reactants. Compounds that are known to be soluble in water include many salts, sugars, acids, and gases like carbon dioxide.
Insoluble Compounds
Insoluble compounds are substances that do not dissolve in a solvent, leading to a mixture where the compound and solvent remain separate. Rather than forming a clear solution, they may result in a suspension or simply settle at the bottom of the container.
  • An example of an insoluble compound is sand in water. No matter how much you stir, the sand remains at the bottom.
  • Insoluble compounds can form precipitates in chemical reactions, which are helpful in identifying certain types of ions in a solution.
Understanding insolubility is crucial in processes like water treatment or during the development of pharmaceuticals, where the presence of insoluble impurities can affect the final product significantly.
Solubility Rules
Solubility rules are a set of general guidelines that help predict whether an ionic compound will dissolve in water. These rules are immensely useful in chemistry for determining the solubility of a compound in a given situation.
Some key solubility rules include:
  • Most nitrate \((\text{NO}_3^- )\) salts are soluble.
  • Salts containing alkali metal ions \((\text{Li}^+, \text{Na}^+, \text{K}^+)\) and the ammonium ion \((\text{NH}_4^+)\) are generally soluble.
  • Chloride \((\text{Cl}^-)\), bromide \((\text{Br}^-)\), and iodide \((\text{I}^-)\) salts are typically soluble, except when combined with silver \((\text{Ag}^+)\), lead \((\text{Pb}^{2+})\), and mercury \((\text{Hg}_2^{2+})\).
By referencing solubility rules, chemists can predict outcomes of reactions, especially precipitation reactions, and determine the feasibility of forming certain solutions.
Ionic Compounds
Ionic compounds are chemical compounds composed of ions held together by electrostatic forces termed ionic bonding. These compounds are typically composed of a metal and a non-metal. Ionic compounds are prevalent in both nature and industry.
  • When dissolved in water, ionic compounds dissociate into their respective ions. For example, NaCl dissolves into \(\text{Na}^+\) and \(\text{Cl}^-\).
  • They can conduct electricity when dissolved or melted, as the ions are free to move.
Ionic compounds exhibit distinct properties such as high melting and boiling points due to the strong forces holding the ions in place. Their role in solutions is fundamental, as they form the basis of electrolytic solutions necessary for conducting electricity.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

For each of the following, write the molecular equation, including phase labels. Then write the net ionic equation. Note that the salts formed in these reactions are soluble. a. the neutralization of hydrobromic acid with calcium hydroxide solution b. the reaction of solid aluminum hydroxide with nitric acid c. the reaction of aqueous hydrogen cyanide with calcium hydroxide solution d. the neutralization of lithium hydroxide solution by aqueous hydrogen cyanide

Barium carbonate is the source of barium compounds. It is produced in an aqueous precipitation reaction from barium sulfide and sodium carbonate. (Barium sulfide is a soluble compound obtained by heating the mineral barite, which is barium sulfate, with carbon.) What are the molecular equation and net ionic equation for the precipitation reaction? A solution containing \(33.9 \mathrm{~g}\) of barium sulfide requires \(21.2 \mathrm{~g}\) of sodium carbonate to react completely with it, and \(15.6 \mathrm{~g}\) of sodium sulfide is produced in addition to whatever barium carbonate is obtained. How many grams of barium sulfide are required to produce \(10.0\) tons of barium carbonate? (One ton equals 2000 pounds.)

What volume of \(0.250 \mathrm{M} \mathrm{HNO}_{3}\) (nitric acid) reacts with \(44.8 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) (sodium carbonate) in the following reaction? $$ 2 \mathrm{HNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \stackrel{\longrightarrow}{2 \mathrm{NaNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g)} $$

Balance the following oxidation-reduction reactions by the half-reaction method. a. \(\mathrm{FeI}_{3}(a q)+\mathrm{Mg}(s) \longrightarrow \mathrm{Fe}(s)+\mathrm{MgI}_{2}(a q)\) b. \(\mathrm{H}_{2}(g)+\mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Ag}(s)+\mathrm{H}^{+}(a q)\)

An alloy of aluminum and magnesium was treated with sodium hydroxide solution, in which only aluminum reacts. \(2 \mathrm{Al}(s)+2 \mathrm{NaOH}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{NaAl}(\mathrm{OH})_{4}(a q)+3 \mathrm{H}_{2}(g)\) If a sample of alloy weighing \(1.118\) g gave \(0.1068 \mathrm{~g}\) of hydrogen, what is the percentage of aluminum in the alloy?
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.