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) $\mathrm{Na}^{+}+\mathrm{HCO}_{3}^{-}$
Solution
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−
This solution contains H+ ions, which are characteristic of acidic solutions.
Option (B):H2O+Na++OH−
This solution contains OH− ions, which are characteristic of basic (alkaline) solutions.
Option (C):Na++HCO3−
This solution contains HCO3−, which can act as a weak acid or a weak base, but in the presence of Na+, it is more likely to be slightly basic.
Step 2: Determine the Nature of Each Solution
Option (A): The presence of H+ ions indicates an acidic solution.
Option (B): The presence of OH− ions indicates a basic solution.
Option (C): The presence of HCO3− in combination with 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+ ions specifically indicates acidity.
Final Answer
The solution that is acidic is option (A): H2O+H++Cl−.