Question

what is the concentration of the hydronium ions in an acidic solution?

\\(1.0 \times 10^{-7}\text{ m}\\)
\\(1.0 \times 10^{-14}\text{ m}\\)
\\(> 1.0 \times 10^{-7}\text{ m}\\)
\\(< 1.0 \times 10^{-7}\text{ m}\\)
\\(0.0\text{ m}\\)

Explanation:

🆕 New Concept Discovered: pH Scale and Hydronium Ion Concentration
Acids have more hydronium ions than neutral water.

Step 1: Understand the neutral reference point

In pure water at \(25^\circ\text{C}\), the water molecules self-ionize to form equal amounts of hydronium ions (\(\text{H}_3\text{O}^+\)) and hydroxide ions (\(\text{OH}^-\)).

This neutral concentration is:

$$ [\text{H}_3\text{O}^+] = 1.0 \times 10^{-7}\text{ M} $$

Step 2: Determine the effect of an acid

An acidic solution is defined by having a higher concentration of hydronium ions than pure water.

Therefore, for any acidic solution:

$$ [\text{H}_3\text{O}^+] > 1.0 \times 10^{-7}\text{ M} $$

Answer:

\(> 1.0 \times 10^{-7}\text{ M}\)