3 posts • Page 1 of 1
What's the difference when you're calculating the pH of a strong versus a weak acid? I'm very confused with the Ka and the pKa equilibrium and how to calculate the pH when you're given a certain number of grams of a molecule and the molarity of it in a solution.
To calculate the pH of a weak acid solution, you need to use Ka and set up an equilibrium equation, which is beyond the scope of this quarter. For questions involving strong acids and baes, you can solve them stoichiometry as a neutralization reaction and then calculate the pH using the remaining H+ in solution.
Who is online
Users browsing this forum: No registered users and 1 guest