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In a solution whose [H⁺] = 1.9 x 10⁻⁵ M at 25°C, what is the [OH⁻]? Is this solution acidic, basic, or neutral?
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17. Acid and Base Equilibrium
The pH Scale
Scelta multipla
What is the pH of a neutral solution at 25°C?
A
14
B
1
C
0
D
7
Guida verificata passo dopo passo1
Understand that pH is a measure of the hydrogen ion concentration in a solution, defined as \( \text{pH} = -\log[\text{H}^+] \).
Recognize that a neutral solution at 25°C has equal concentrations of hydrogen ions \( [\text{H}^+] \) and hydroxide ions \( [\text{OH}^-] \).
Recall that in pure water at 25°C, the concentration of hydrogen ions \( [\text{H}^+] \) is \( 1 \times 10^{-7} \) M.
Apply the pH formula: \( \text{pH} = -\log(1 \times 10^{-7}) \).
Calculate the pH value, which is 7, indicating a neutral solution at 25°C.
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