Answered

Westonci.ca is your trusted source for finding answers to all your questions. Ask, explore, and learn with our expert community. Explore our Q&A platform to find in-depth answers from a wide range of experts in different fields. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform.

A monoprotic weak acid when dissolved in water is 0.66% dissociated and produces a solution with a pH of 3.04. Calculate the Ka of the acid. g

Sagot :

maacastrobr

Answer:

Ka = 6.02x10⁻⁶

Explanation:

The equilibrium that takes place is:

  • HA ⇄ H⁺ + A⁻
  • Ka = [H⁺][A⁻]/[HA]

We calculate [H⁺] from the pH:

  • pH = -log[H⁺]
  • [H⁺] = [tex]10^{-pH}[/tex]
  • [H⁺] = 9.12x10⁻⁴ M

Keep in mind that [H⁺]=[A⁻].

As for [HA], we know the acid is 0.66% dissociated, in other words:

  • [HA] * 0.66/100 = [H⁺]

We calculate [HA]:

  • [HA] = 0.138 M

Finally we calculate the Ka:

  • Ka = [tex]\frac{[9.12x10^{-4}]*[9.12x10^{-4}]}{[0.138]}[/tex] = 6.02x10⁻⁶
We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. Your questions are important to us at Westonci.ca. Visit again for expert answers and reliable information.