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Chapter 32: Problem 5

When one mole of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is dissolved in water: a) how many moles of sodium ions are found in the solution? b) how many moles of sulfate ions are found in the solution?

Short Answer

Expert verified
a) Two moles of sodium ions are found in the solution when one mole of sodium sulfate is dissolved. b) One mole of sulfate ions is found in the solution when one mole of sodium sulfate is dissolved.

Step by step solution

01

Understand the Molecular Formula

Look at the molecular formula of sodium sulfate \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). There are two sodium ions (Na+) and one sulfate ion (SO4-2) in one molecule of sodium sulfate.
02

Identify the Number of Moles of Sodium Ions

When one mole of sodium sulfate \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) dissolves in water, it separates into its ions. Therefore, since there are two sodium ions in one molecule of sodium sulfate, two moles of sodium ions will be produced when one mole of sodium sulfate is dissolved.
03

Identify the Number of Moles of Sulfate Ions

Since there is one sulfate ion (SO4-2) in one molecule of sodium sulfate, so one mole of sulfate ions will be produced when one mole of sodium sulfate is dissolved.

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Most popular questions from this chapter

Verify that when \(5.26 \mathrm{~g}\) of glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\), dissolves in water: a) there are \(2.92 \times 10^{-2}\) moles of glucose in the water. b) there are \(1.76 \times 10^{22}\) molecules of glucose in the water.

Verify that when \(10.0 \mathrm{~g}\) of sodium sulfate dissolves in water: a) there are \(7.04 \times 10^{-2}\) moles of sodium sulfate in the water. b) there are \(7.04 \times 10^{-2}\) moles of sulfate in the water. c) there are \(14.1 \times 10^{-2}\) moles of sodium in the water.

Which is more concentrated with respect to sodium ions, \(0.50 \mathrm{M} \mathrm{NaCl}\) or \(0.30 \mathrm{M}\) \(\mathrm{Na}_{2} \mathrm{SO}_{4} ?\)

Which is more concentrated with respect to sodium ions, \(50.0 \mathrm{~g}\) of \(\mathrm{NaCl}\) in \(500.0\) \(\mathrm{mL}\) of solution or \(59.0 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in \(500.0 \mathrm{~mL}\) of solution?
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