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Question
When acidulated water (dil.H2SO4 solution) is electrolysed, will the pH of the solution be affected? Justify your answer.
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Solution
Anode: \[\ce{2H2O(l) -> O2(g) + 4H + (aq) + 4e^{-}}\]
Cathode: \[\ce{4H^{+} + 4e^{-} -> 2H2}\]
Overall cell reaction: \[\ce{2H2O(l) -> O2(g) + 2H2(g)}\]
pH remains the same because concentration of H+ ions remains constant.
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RELATED QUESTIONS
Define “Molar conductivity”.
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\[\ce{\Lambda^0_m(NH4OH)}\] is equal to ______.
\[\ce{Λ^0_m H2O}\] is equal to:
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| Column I | Column II |
| (i) F2 | (a) metal is the strongest reducing agent |
| (ii) Li | (b) metal ion which is the weakest oxidising agent |
| (iii) Au3+ | (c) non metal which is the best oxidising agent |
| (iv) Br– | (d) unreactive metal |
| (v) Au | (e) anion that can be oxidised by Au3+ |
| (vi) Li+ | (f) anion which is the weakest reducing agent |
| (vii) F– | (g) metal ion which is an oxidising agent |
Consider figure and answer the question to given below.
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Given below are two statements:
Statements I: The limiting molar conductivity of KCl (strong electrolyte) is higher compared to that of CH3COOH (weak electrolyte).
Statement II: Molar conductivity decreases with decrease in concentration of electrolyte.
In the light of the above statements, choose the most appropriate answer from the options given below:
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Reason (R) : Number of ions per unit volume that carry the current in a solution decreases on dilution.
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