HCI is a strong acid. What is the ion concentration, (H+), of a 0.0015M solution of HCI? What is the pH of a 0.0015M solution of HCI?
I have looked in my book but it not making sense. I am not sure where to even start the problem. A little guidance please
Not much else to do than to work the problem. The point you are missing is that it's a strong acid. Strong acids ionize 100% so ALL of the HCl molecules end up as ions and NONE are in the form of HCl molecules. It isn't necessary to do an ICE chart but that might help a little.
.........HCl --> H^+ + Cl-
I.....0.0015.....0.....0
C....-0.0015....0.0015..0.0015
E........0......0.0015..0.0015
So the (H^+) = (Cl^-) = 0.0015M and you convert that to pH.
To find the ion concentration (H+) of a solution of HCl (hydrochloric acid) with a concentration of 0.0015M, you need to understand the concept of dissociation of acids.
When HCl dissolves in water, it dissociates into H+ ions and Cl- ions. Since HCl is a strong acid, it dissociates completely in water.
The concentration of H+ ions in the solution is equal to the concentration of the acid itself. In this case, the concentration of H+ ions would also be 0.0015M.
Now, to find the pH of a solution, you need to use the equation pH = -log[H+]. The log is the base 10 logarithm.
In this case, the concentration of H+ ions is 0.0015M. Taking the negative logarithm (-log) of 0.0015, you get:
pH = -log(0.0015)
Calculating this value, you should get a pH value of approximately 2.82.
So, the ion concentration (H+) of a 0.0015M solution of HCl is 0.0015M, and the pH of this solution is approximately 2.82.