Calculate the pH and concentration of H3O of a 0.285M HCl solution.
To calculate the pH and concentration of H3O+ in a 0.285 M HCl solution, we need to understand the properties of the HCl molecule and its ionization in water.
HCl is a strong acid, meaning it almost completely dissociates into H+ (Hydrogen) ions and Cl- (Chloride) ions in aqueous solutions. Therefore, in the given 0.285 M HCl solution, the concentration of H+ ions will be 0.285 M.
The concentration of H3O+ ions is equivalent to the concentration of H+ ions in water. Therefore, the concentration of H3O+ ions in the 0.285 M HCl solution is also 0.285 M.
Now, let's calculate the pH of the solution using the formula:
pH = -log[H+]
where [H+] represents the concentration of H+ ions.
In this case, the pH of the solution is:
pH = -log(0.285) ≈ 0.546
Therefore, the pH of the 0.285 M HCl solution is approximately 0.546, and the concentration of H3O+ ions is also 0.285 M.