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Ch.5 - Introduction to Solutions and Aqueous Solutions
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.5 - Introduction to Solutions and Aqueous SolutionsProblema 47
Capitolo 5, Problema 47

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. RbBr b. Na3OH c. C12H22O11 d. MgSO4

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Identify if each compound is an electrolyte or a non-electrolyte. Electrolytes dissociate into ions in water, conducting electricity, while non-electrolytes do not.
For RbBr, recognize it as an ionic compound composed of Rb⁺ and Br⁻ ions. Ionic compounds typically dissociate in water, making them strong electrolytes.
For Na₃OH, note that it seems to be a typo or a non-standard formula. Assuming it refers to a sodium compound, sodium compounds are generally ionic and dissociate in water, making them strong electrolytes.
For C₁₂H₂₂O₁₁ (sucrose), identify it as a covalent compound. Covalent compounds do not dissociate into ions in water, making them non-electrolytes.
For MgSO₄, recognize it as an ionic compound composed of Mg²⁺ and SO₄²⁻ ions. Ionic compounds typically dissociate in water, making them strong electrolytes.

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Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes, such as salts and strong bases, fully dissociate into ions, while weak electrolytes only partially dissociate. Understanding whether a compound is a strong or weak electrolyte is crucial for predicting its ability to conduct electrical current in solution.
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Electrolytes and Strong Acids

Solubility of Ionic Compounds

Ionic compounds, such as RbBr and MgSO4, typically dissolve in water to form ions, which contribute to electrical conductivity. The solubility of these compounds in water is influenced by factors like lattice energy and hydration energy. Recognizing which ionic compounds are soluble helps determine if their aqueous solutions will conduct electricity.
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Soluble Ionic Solutes

Non-electrolytes

Non-electrolytes are substances that do not dissociate into ions in solution, thus failing to conduct electricity. An example is sucrose (C12H22O11), which dissolves in water but remains as intact molecules. Identifying non-electrolytes is essential for understanding which compounds will not contribute to electrical conductivity in an aqueous solution.
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02:29
Weak Bases and Non-Electrolytes
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