Questions: Which solution is acidic? (A) H2O + H+ + Cl- (B) H2O + Na+ + OH- (C) Na+ + HCO3-

Which solution is acidic? 
(A) H2O + H+ + Cl- 
(B) H2O + Na+ + OH- 
(C) Na+ + HCO3-
Transcript text: Which solution is acidic? (A) $\mathrm{H}_{2} \mathrm{O}+\mathrm{H}^{+}+\mathrm{Cl}^{-}$ (B) $\mathrm{H}_{2} \mathrm{O}+\mathrm{Na}^{+}+\mathrm{OH}^{-}$ (C) $\mathrm{Na}^{+}+\mathrm{HCO}_{3}^{-}$
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Solution

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Solution Steps

Step 1: Analyze the Composition of Each Solution

To determine which solution is acidic, we need to analyze the composition of each option:

  • Option (A): H2O+H++Cl\mathrm{H}_{2} \mathrm{O}+\mathrm{H}^{+}+\mathrm{Cl}^{-}

    • This solution contains H+\mathrm{H}^{+} ions, which are characteristic of acidic solutions.
  • Option (B): H2O+Na++OH\mathrm{H}_{2} \mathrm{O}+\mathrm{Na}^{+}+\mathrm{OH}^{-}

    • This solution contains OH\mathrm{OH}^{-} ions, which are characteristic of basic (alkaline) solutions.
  • Option (C): Na++HCO3\mathrm{Na}^{+}+\mathrm{HCO}_{3}^{-}

    • This solution contains HCO3\mathrm{HCO}_{3}^{-}, which can act as a weak acid or a weak base, but in the presence of Na+\mathrm{Na}^{+}, it is more likely to be slightly basic.
Step 2: Determine the Nature of Each Solution
  • Option (A): The presence of H+\mathrm{H}^{+} ions indicates an acidic solution.
  • Option (B): The presence of OH\mathrm{OH}^{-} ions indicates a basic solution.
  • Option (C): The presence of HCO3\mathrm{HCO}_{3}^{-} in combination with Na+\mathrm{Na}^{+} suggests a slightly basic solution.
Step 3: Evaluate the Claim in Option D

Option D claims that all solutions are acidic because they contain hydrogen. However, the presence of hydrogen alone does not determine acidity. The presence of H+\mathrm{H}^{+} ions specifically indicates acidity.

Final Answer

The solution that is acidic is option (A): H2O+H++Cl\mathrm{H}_{2} \mathrm{O}+\mathrm{H}^{+}+\mathrm{Cl}^{-}.

A \boxed{\text{A}}

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