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Chapter 4: Problem 6

Sodium sulfate \(\left(\mathrm{Na}_{2} \mathrm{SO}_{4}\right)\) is a strong electrolyte. What species are present in \(\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) ?\)

Short Answer

Expert verified
The species present in an aqueous solution of Sodium Sulfate (\(\mathrm{Na}_{2}\mathrm{SO}_{4}\)) are Sodium ions (\(\mathrm{Na}^{+}\)) and Sulfate ions (\(\mathrm{SO}_4^{2-}\)).

Step by step solution

01

Identify the ions of Sodium Sulfate

In a molecule of Sodium Sulfate (\(\mathrm{Na}_{2} \mathrm{SO}_{4}\)), there are two sodium ions (\(\mathrm{Na}^{+}\)) and one sulfate ion (\(\mathrm{SO}_4^{2-}\)).
02

Predict the dissolution of Sodium Sulfate in water

When Sodium Sulfate (\(\mathrm{Na}_{2} \mathrm{SO}_{4}\)) dissolves in water, it separates into its constituent ions due to their interaction with water molecules. This process is called dissociation.
03

Write the dissociation reaction

So, the dissociation of Sodium Sulfate in water can be represented as follows: \(\mathrm{Na}_{2} \mathrm{SO}_{4}(aq) \rightarrow 2\mathrm{Na}^{+}(aq) + \mathrm{SO}_4^{2-}(aq)\). This indicates that in an aqueous solution, Sodium Sulfate exists as separate Sodium and Sulfate ions.

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Most popular questions from this chapter

Describe in each case how you would separate the cations or anions in an aqueous solution of: (a) \(\mathrm{NaNO}_{3}\) and \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2},\) (b) \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) and \(\mathrm{KNO}_{3}\), (c) \(\mathrm{KBr}\) and \(\mathrm{KNO}_{3}\), (d) \(\mathrm{K}_{3} \mathrm{PO}_{4}\) and \(\mathrm{KNO}_{3}\), (e) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and \(\mathrm{NaNO}_{3}\).

Describe the basic steps involved in gravimetric analysis. How does this procedure help us determine the identity of a compound or the purity of a compound if its formula is known?

Oxygen \(\left(\mathrm{O}_{2}\right)\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.

The concentration of lead ions \(\left(\mathrm{Pb}^{2+}\right)\) in a sample of polluted water that also contains nitrate ions \(\left(\mathrm{NO}_{3}^{-}\right)\) is determined by adding solid sodium sulfate \(\left(\mathrm{Na}_{2} \mathrm{SO}_{4}\right)\) to exactly \(500 \mathrm{~mL}\) of the water. (a) Write the molecular and net ionic equations for the reaction. (b) Calculate the molar concentration of \(\mathrm{Pb}^{2+}\) if \(0.00450 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). was needed for the complete precipitation of \(\mathrm{Pb}^{2+}\) ions as \(\mathrm{PbSO}_{4}\).

A 22.02-mL solution containing \(1.615 \mathrm{~g} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with a 28.64-mL solution containing \(1.073 \mathrm{~g}\) \(\mathrm{NaOH}\). Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive.
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