Answer:
Solution is acidic with [H⁺] = 1 x 10⁻⁴M => pH = 4; [OH⁻] = 1 X 10⁻14/1 x 10⁻⁴ = 1 x 10⁻¹⁰
Step-by-step explanation:
Acidity and Alkalinity of an aqueous solution is defined relative to the relationship between the concentrations of Hydronium ions (H₃O⁺) vs Hydroxide ions (OH⁻) in solution. That is, for pure water at 25°C it is known that [H₃O⁺] = [OH⁻] = 10⁻⁷M for 'neutral' solutions. However, if ...
[H₃O⁺] > 10⁻⁷M => [OH⁻] < 10⁻⁷M => the solution is classified as acidic, and if
[H₃O⁺] < 10⁻⁷M => [OH⁻] > 10⁻⁷M => the solution is classified as alkaline or basic.
Relating this to pH values where pH = - log[H₃O⁺]
for [H₃O⁺] = 10⁻⁷M => pH = -log(10⁻⁷) = 7 for neutral solutions
for [H₃O⁺] > 10⁻⁷M => pH < -log(10⁻⁷) < 7 for acidic solutions
for [H₃O⁺] < 10⁻⁷M => pH > -log(10⁻⁷) > 7 for basic solutions