Posted by **Jonah** on Friday, March 22, 2013 at 12:35pm.

A tank contains exactly 10^(6)liters of pure water. 1.0*10^(-6) moles of HCl (g) is bubbled into this tank. What is the resulting pH?

The answer is 7, but I was only able to deduce that based on the fact that water has a neutral pH, but there's a mathematical way to do it and I'm not sure how to go about it.

- Chemistry -
**Simon Mai**, Friday, March 22, 2013 at 4:54pm
I don't know.

- Chemistry -
**DrBob222**, Friday, March 22, 2013 at 6:30pm
HCl is a strong acid meaning that it dissociates 100%; therefore, 1E-6 mol/1E6L = 1E-12M HCl.

HCl ==> H^ + Cl^-

1E-12...0.....0

-1E-12..1E-12..1E-12

..........HOH ==> H^+ + OH^-

I...............1E-12....0

C..................x......x

E..............1E-12+x....x

(H^+)(OH^-) = Kw = 1E-14

(1E-12+x)(x) = 1E-14

Solve the quadratic. I get all of these numbers on the calculator like

9.99995E-8

pH = -log(H^+) = 7.00000.

With no temperature listed I couldn't look up the correct value for Kw at that particular temperature but I think this will do the trick.

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