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Chapter 4: Problem 23

Show how each of the following strong electrolytes "breaks up" into its component ions upon dissolving in water by drawing molecular-level pictures. a. NaBr b. \(\mathrm{MgCl}_{2}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) e, \(\mathrm{NaOH}\) f. \(\mathrm{FeSO}_{4}\) g. \(\mathrm{KMnO}_{4}\) h. \(\mathrm{HClO}_{4}\) i. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

Short Answer

Expert verified
a. NaBr (s) ⟶ Na⁺ (aq) + Br⁻ (aq) b. \(\mathrm{MgCl}_{2}\) (s) ⟶ Mg²⁺ (aq) + 2Cl⁻ (aq) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (s) ⟶ Al³⁺ (aq) + 3NO₃⁻ (aq) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) (s) ⟶ 2NH₄⁺ (aq) + SO₄²⁻ (aq) e. \(\mathrm{NaOH}\) (s) ⟶ Na⁺ (aq) + OH⁻ (aq) f. \(\mathrm{FeSO}_{4}\) (s) ⟶ Fe²⁺ (aq) + SO₄²⁻ (aq) g. \(\mathrm{KMnO}_{4}\) (s) ⟶ K⁺ (aq) + MnO₄⁻ (aq) h. \(\mathrm{HClO}_{4}\) (s) ⟶ H⁺ (aq) + ClO₄⁻ (aq) i. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (s) ⟶ NH₄⁺ (aq) + C₂H₃O₂⁻ (aq)

Step by step solution

01

a. NaBr

When NaBr dissolves in water, it breaks up into its individual ions: sodium ion (Na⁺) and bromide ion (Br⁻). Therefore, the molecular-level picture is: NaBr (s) ⟶ Na⁺ (aq) + Br⁻ (aq)
02

b. \(\mathrm{MgCl}_{2}\)

When \(\mathrm{MgCl}_{2}\) dissolves in water, it breaks up into its individual ions: magnesium ion (Mg²⁺) and two chloride ions (2Cl⁻). Therefore, the molecular-level picture is: \(\mathrm{MgCl}_{2}\) (s) ⟶ Mg²⁺ (aq) + 2Cl⁻ (aq)
03

c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)

When \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) dissolves in water, it breaks up into its individual ions: aluminum ion (Al³⁺) and three nitrate ions (3NO₃⁻). Therefore, the molecular-level picture is: \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) (s) ⟶ Al³⁺ (aq) + 3NO₃⁻ (aq)
04

d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

When \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) dissolves in water, it breaks up into its individual ions: two ammonium ions (2NH₄⁺) and one sulfate ion (SO₄²⁻). Therefore, the molecular-level picture is: \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) (s) ⟶ 2NH₄⁺ (aq) + SO₄²⁻ (aq)
05

e. \(\mathrm{NaOH}\)

When \(\mathrm{NaOH}\) dissolves in water, it breaks up into its individual ions: sodium ion (Na⁺) and hydroxide ion (OH⁻). Therefore, the molecular-level picture is: \(\mathrm{NaOH}\) (s) ⟶ Na⁺ (aq) + OH⁻ (aq)
06

f. \(\mathrm{FeSO}_{4}\)

When \(\mathrm{FeSO}_{4}\) dissolves in water, it breaks up into its individual ions: iron (II) ion (Fe²⁺) and sulfate ion (SO₄²⁻). Therefore, the molecular-level picture is: \(\mathrm{FeSO}_{4}\) (s) ⟶ Fe²⁺ (aq) + SO₄²⁻ (aq)
07

g. \(\mathrm{KMnO}_{4}\)

When \(\mathrm{KMnO}_{4}\) dissolves in water, it breaks up into its individual ions: potassium ion (K⁺) and permanganate ion (MnO₄⁻). Therefore, the molecular-level picture is: \(\mathrm{KMnO}_{4}\) (s) ⟶ K⁺ (aq) + MnO₄⁻ (aq)
08

h. \(\mathrm{HClO}_{4}\)

When \(\mathrm{HClO}_{4}\) dissolves in water, it breaks up into its individual ions: hydrogen ion (H⁺) and perchlorate ion (ClO₄⁻). Therefore, the molecular-level picture is: \(\mathrm{HClO}_{4}\) (s) ⟶ H⁺ (aq) + ClO₄⁻ (aq)
09

i. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

When \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) dissolves in water, it breaks up into its individual ions: ammonium ion (NH₄⁺) and acetate ion (C₂H₃O₂⁻). Therefore, the molecular-level picture is: \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (s) ⟶ NH₄⁺ (aq) + C₂H₃O₂⁻ (aq)

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Most popular questions from this chapter

What mass of silver chloride can be prepared by the reaction of \(100.0 \mathrm{~mL}\) of \(0.20 \mathrm{M}\) silver nitrate with \(100.0 \mathrm{~mL}\) of \(0.15 \mathrm{M}\) calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{KMnO}_{4}\) b. \(\mathrm{NiO}_{2}\) c. \(\mathrm{Na}_{4} \mathrm{Fe}(\mathrm{OH})_{6}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) e. \(\mathrm{P}_{4} \mathrm{O}_{6}\) f. \(\mathrm{Fe}_{3} \mathrm{O}_{4}\) g. \(\mathrm{XeOF}_{4}\) h. \(\mathrm{SF}_{4}\) i. CO j. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

If \(10 . \mathrm{g}\) of \(\mathrm{AgNO}_{3}\) is available, what volume of \(0.25 \mathrm{MAgNO}_{3}\) solution can be prepared?

A student titrates an unknown amount of potassium hydrogen phthalate \(\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\right.\), often abbreviated \(\mathrm{KHP}\) ) with \(20.46 \mathrm{~mL}\) of a \(0.1000-M \mathrm{NaOH}\) solution. KHP (molar mass \(=204.22 \mathrm{~g} /\) mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

You wish to prepare \(1 \mathrm{~L}\) of a \(0.02-M\) potassium iodate solution. You require that the final concentration be within \(1 \%\) of \(0.02 M\) and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of \(\mathrm{KIO}_{7}\) that can be used.
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