Passage talks about chlorinating water in swimming pools, and gives the following reaction equation:
Cl2(g) + H2O <> HCl (aq) + HOCl (aq), Keq=(1E-3)
Q:If the pH of swimming pool water is 5, what is the concentration of HOCl?
A: If the pH is 5, then the [HCl] must be (1E10-5), and this equals the [HOCl] as well because they are formed in a 1:1 ratio.
I attempted to answer this question a little differently though. I used the Keq given, and used it as the dissociation constant for HClO <> H+ + ClO- and calculated the [HOCl] needed to have produced pH 5, if all the H+ ions were from HOCl. Since this gives a value of [HOCl] much larger than what it actually would have been if I had used the real Keq for the reaction, I chose the only answer that was smaller than what I calculated, which was incorrect.
While I understand the answer given, I don't understand where exactly my logic fails, though clearly it does! Any help appreciated
Cl2(g) + H2O <> HCl (aq) + HOCl (aq), Keq=(1E-3)
Q:If the pH of swimming pool water is 5, what is the concentration of HOCl?
A: If the pH is 5, then the [HCl] must be (1E10-5), and this equals the [HOCl] as well because they are formed in a 1:1 ratio.
I attempted to answer this question a little differently though. I used the Keq given, and used it as the dissociation constant for HClO <> H+ + ClO- and calculated the [HOCl] needed to have produced pH 5, if all the H+ ions were from HOCl. Since this gives a value of [HOCl] much larger than what it actually would have been if I had used the real Keq for the reaction, I chose the only answer that was smaller than what I calculated, which was incorrect.
While I understand the answer given, I don't understand where exactly my logic fails, though clearly it does! Any help appreciated