Question:
Which of the following is a weak electrolyte?
Which of the following is a weak electrolyte?
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Weak acids and weak bases are generally weak electrolytes because they ionize partially in solution.
Updated On: May 7, 2026
- \(H_2CO_3\)
- \(H_2SO_4\)
- \(NaCl\)
- \(NaOH\)
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The Correct Option is A
Solution and Explanation
Concept:
A weak electrolyte ionizes only partially in aqueous solution, whereas a strong electrolyte ionizes almost completely.
Step 1: \(H_2SO_4\) is a strong acid and dissociates strongly in water.
Step 2: \(NaCl\) is an ionic salt and dissociates almost completely in water.
Step 3: \(NaOH\) is a strong base and dissociates almost completely in water.
Step 4: \(H_2CO_3\), carbonic acid, is a weak acid. It ionizes only partially in water: \[ H_2CO_3 \rightleftharpoons H^+ + HCO_3^- \] Therefore, it is a weak electrolyte. Hence, \[ \boxed{H_2CO_3} \]
Step 1: \(H_2SO_4\) is a strong acid and dissociates strongly in water.
Step 2: \(NaCl\) is an ionic salt and dissociates almost completely in water.
Step 3: \(NaOH\) is a strong base and dissociates almost completely in water.
Step 4: \(H_2CO_3\), carbonic acid, is a weak acid. It ionizes only partially in water: \[ H_2CO_3 \rightleftharpoons H^+ + HCO_3^- \] Therefore, it is a weak electrolyte. Hence, \[ \boxed{H_2CO_3} \]
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