The pH of 0.5 M mono basic acid, HCl is 4.50. Calculate the acidity constant (Ka) and pKa , concentration of H+ and HCl at equilibrium.
Question
Solution 1
To solve this problem, we need to use several equations related to pH, pKa, and the equilibrium of acids in solution. Here are the steps:
- Calculate the concentration of H+ ions: The pH is given as 4.50. The pH is defined as pH = -log[H+], where [H+] is the concentration of H+ ions. So, we can re Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI
Similar Questions
The pH of 0.5 M mono basic acid, HCl is 4.50. Calculate the acidity constant (Ka) and pKa , concentration of H+ and HCl at equilibrium.
What is the pH of a buffer that contains 0.5 M ammonia(base) and 0.8 M ammonium chloride(acid)? (pKa = 9.248).
An unknown weak acid with a concentration of 0.097 M has a pH of 1.80. What is the Ka of the weak acid?
What is the net charge of an amino acid (possessing two pKA values) at the isoelectric pH? A. 0.5 B. 1 C. 0 D. -1
37) If the value of POH for weak acid equal 10 and its equilibrium constant Ka= 5.1x104, So the degree of ionization of the acid equals
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.