Question

The concentration of propionic acid solution was found to be 5.0 × 10⁻² M at 25°C. Calculate:

a) Hydrogen (H⁺) ion concentration, (H₃O⁺ = H⁺)
b) Hydroxide (OH⁻) ion concentration
c) pH of the propionic acid solution
- A. ( [H^+] = 5.0 times 10^(-2) ) M, ( [OH^-] = 2.0 times 10^(-13) ) M, pH = 1.301
- B. ( [H^+] = 2.0 times 10^(-13) ) M, ( [OH^-] = 5.0 times 10^(-2) ) M, pH = 12.699
- C. ( [H^+] = 5.0 times 10^(-2) ) M, ( [OH^-] = 2.0 times 10^(-13) ) M, pH = 2.301
- D. ( [H^+] = 2.0 times 10^(-13) ) M, ( [OH^-] = 5.0 times 10^(-2) ) M, pH = 11.301

Answer 1

The concentration of propionic acid solution is 5.0 × 10⁻² M at 25°C. The [H⁺] is 5.0 × 10⁻² M, [OH⁻] is 2.0 × 10⁻¹³ M, and the pH is 1.301.

Step-by-step explanation:

The concentration of propionic acid solution is 5.0 × 10⁻² M at 25°C. To calculate the hydrogen (H⁺) ion concentration, we can use the fact that propionic acid is a weak acid and the concentration of hydronium ions is equal to the concentration of the acid. So, the [H⁺] is 5.0 × 10⁻² M.

To find the hydroxide (OH⁻) ion concentration, we can use the fact that water is neutral and the product of [H⁺] and [OH⁻] is constant at 25°C. Since [H⁺] is 5.0 × 10⁻² M, [OH⁻] can be calculated as 1.0 × 10^{-14} / 5.0 × 10⁻² M, which is 2.0 × 10⁻¹³ M.

The pH of the propionic acid solution can be calculated using the equation pH = -log[H⁺]. So, the pH is -log(5.0 × 10⁻²) which is approximately 1.301.