Question

part a
what is the concentration of the hydronium ions in a neutral solution?
0.0 m
1.0 ×10⁻¹⁴ m
< 1.0×10⁻⁷ m
1.0 ×10⁻⁷ m

1.0×10⁻⁷ m

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Explanation:

In a neutral solution at 25°C, the concentration of hydronium ions ($H_3O^+$) equals that of hydroxide ions ($OH^-$). The ion product constant of water ($K_w$) is $1.0 \times 10^{-14}$, so $[H_3O^+] = \sqrt{K_w} = 1.0 \times 10^{-7}\ M$.

Answer:

1.0 ×10⁻⁷ M