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Chapter 11: Problem 16

Write equations showing the ions present after the following strong electrolytes are dissolved in water. a. \(\mathrm{HNO}_{3}\) d. \(\mathrm{SrBr}_{2}\) g. \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) b. \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) e. \(\mathrm{KClO}_{4}\) h. \(\mathrm{CuSO}_{4}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) f. \(\mathrm{NH}_{4} \mathrm{Br}\) i. \(\mathrm{NaOH}\)

Short Answer

Expert verified
a. \(\mathrm{HNO}_3 \to \mathrm{H}^{+} + \mathrm{NO}_3^-\) b. \(\mathrm{SrBr}_{2} \to \mathrm{Sr}^{2+} + 2\mathrm{Br}^{-}\) c. \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_3 \to \mathrm{Al}^{3+} + 3\mathrm{NO}_{3}^{-}\) d. \(\mathrm{Na}_{2}\mathrm{SO}_{4} \to 2\mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\) e. \(\mathrm{KClO}_{4} \to \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\) f. \(\mathrm{NH}_{4}\mathrm{Br} \to \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\) g. \(\mathrm{NH}_{4}\mathrm{NO}_3 \to \mathrm{NH}_{4}^+ + \mathrm{NO}_{3}^{-}\) h. \(\mathrm{CuSO}_4 \to \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\) i. \(\mathrm{NaOH} \to \mathrm{Na}^{+} + \mathrm{OH}^{-}\)

Step by step solution

01

a. HNO3 dissociation

When HNO3, a strong acid, is dissolved in water, it completely dissociates into hydrogen ions (H+) and nitrate ions (NO3-): \[ \mathrm{HNO}_3 \to \mathrm{H}^{+} + \mathrm{NO}_3^-\]
02

b. SrBr2 dissociation

When SrBr2 is dissolved in water, it dissociates into strontium ions (Sr2+) and bromide ions (Br-): \[\mathrm{SrBr}_{2} \to \mathrm{Sr}^{2+} + 2\mathrm{Br}^{-}\]
03

c. Al(NO3)3 dissociation

When Al(NO3)3 is dissolved in water, it dissociates into aluminum ions (Al3+) and nitrate ions (NO3-): \[\mathrm{Al}\left(\mathrm{NO}_{3}\right)_3 \to \mathrm{Al}^{3+} + 3\mathrm{NO}_{3}^{-}\]
04

d. Na2SO4 dissociation

When Na2SO4 is dissolved in water, it dissociates into sodium ions (Na+) and sulfate ions (SO4^2-): \[\mathrm{Na}_{2}\mathrm{SO}_{4} \to 2\mathrm{Na}^{+} + \mathrm{SO}_{4}^{2-}\]
05

e. KClO4 dissociation

When KClO4 is dissolved in water, it dissociates into potassium ions (K+) and perchlorate ions (ClO4-): \[\mathrm{KClO}_{4} \to \mathrm{K}^{+} + \mathrm{ClO}_{4}^{-}\]
06

f. NH4Br dissociation

When NH4Br is dissolved in water, it dissociates into ammonium ions (NH4+) and bromide ions (Br-): \[\mathrm{NH}_{4}\mathrm{Br} \to \mathrm{NH}_{4}^{+} + \mathrm{Br}^{-}\]
07

g. NH4NO3 dissociation

When NH4NO3 is dissolved in water, it dissociates into ammonium ions (NH4+) and nitrate ions (NO3-): \[\mathrm{NH}_{4}\mathrm{NO}_3 \to \mathrm{NH}_{4}^+ + \mathrm{NO}_{3}^{-}\]
08

h. CuSO4 dissociation

When CuSO4 is dissolved in water, it dissociates into copper(II) ions (Cu2+) and sulfate ions (SO4^2-): \[\mathrm{CuSO}_4 \to \mathrm{Cu}^{2+} + \mathrm{SO}_{4}^{2-}\]
09

i. NaOH dissociation

When NaOH, a strong base, is dissolved in water, it completely dissociates into sodium ions (Na+) and hydroxide ions (OH-): \[\mathrm{NaOH} \to \mathrm{Na}^{+} + \mathrm{OH}^{-}\]

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Most popular questions from this chapter

Which solvent, water or carbon tetrachloride, would you choose to dissolve each of the following? a. \(\mathrm{KrF}_{2}\) e. \(\mathrm{MgF}_{2}\) b. \(\mathrm{SF}_{2}\) f. \(\mathrm{CH}_{2} \mathrm{O}\) c. \(\mathrm{SO}_{2}\) g. \(\mathrm{CH}_{2}=\mathrm{CH}_{2}\) d. \(\mathrm{CO}_{2}\)

A \(1.37 M\) solution of citric acid \(\left(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)\) in water has a density of \(1.10 \mathrm{~g} / \mathrm{cm}^{3} .\) Calculate the mass percent, molality, mole fraction, and normality of the citric acid. Citric acid has three acidic protons.

How would you prepare \(1.0 \mathrm{~L}\) of an aqueous solution of sodium chloride having an osmotic pressure of \(15 \mathrm{~atm}\) at \(22^{\circ} \mathrm{C} ?\) Assume sodium chloride exists as \(\mathrm{Na}^{+}\) and \(\mathrm{Cl}^{-}\) ions in solution.

The solubility of nitrogen in water is \(8.21 \times 10^{-4} \mathrm{~mol} / \mathrm{L}\) at \(0^{\circ} \mathrm{C}\) when the \(\mathrm{N}_{2}\) pressure above water is \(0.790 \mathrm{~atm} .\) Calculate the Henry's law constant for \(\mathrm{N}_{2}\) in units of \(\mathrm{mol} / \mathrm{L} \cdot\) atm for Henry's law in the form \(C=k P\), where \(C\) is the gas concentration in mol/L. Calculate the solubility of \(\mathrm{N}_{2}\) in water when the partial pressure of nitrogen above water is \(1.10 \mathrm{~atm}\) at \(0{ }^{\circ} \mathrm{C}\).

Calculate the solubility of \(\mathrm{O}_{2}\) in water at a partial pressure of \(\mathrm{O}_{2}\) of 120 torr at \(25^{\circ} \mathrm{C}\). The Henry's law constant for \(\mathrm{O}_{2}\) is \(1.3 \mathrm{X}\) \(10^{-3} \mathrm{~mol} / \mathrm{L} \cdot\) atm for Henry's law in the form \(C=k P\), where \(C\) is the gas concentration \((\mathrm{mol} / \mathrm{L})\).
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