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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: kimi85 on September 01, 2007, 10:46:56 PM

Title: calculating pH and
Post by: kimi85 on September 01, 2007, 10:46:56 PM
Calculate [H3O+] and pH in saturated Ba(OH)2 (aq), which contains 3.9 g Ba(OH)2 . 8 H2O per 100 ml solution.

What I did I first find the molarity then multiplied it to two. The I calculated the H+ using the ionization constant of water. But my answer is wrong. I calculated pH from pOH and my answer is wrong too. What is wrong with my computation?

The correct answer is 4 x 10-3 M H3O+ and pH is 12.4.

Thank you.
Title: Re: calculating pH and
Post by: enahs on September 01, 2007, 11:21:26 PM
Quote
The correct answer is 4 x 10-3 M H3O+ and pH is 12.4.

That is impossible.

You either typed it wrong or read the answer wrong.

What would be a pH of a solution with 4x10-3 M H3O+?
Title: Re: calculating pH and
Post by: Borek on September 02, 2007, 04:21:48 AM
Show your numbers, approach (through pOH) seems correct. The only obvious mistake I can think off is molar mass of hydrated hydroxide - have you forgot water, or not?
Title: Re: calculating pH and
Post by: kimi85 on September 02, 2007, 09:16:10 PM
I'm sorry for the error. It should be 4 x 10-13 M H3O+

I also included the molecular weight of the hydrate but I'm still wrong

Here's what I did:

(3.9/315.46)/0.1 L = 0.1236 x 2 = 0.24725 pOH = 0.60686 pH = 14-pOH = 13.39

3O+:

1 x 10-14/0.24724 = 4 x 10-14

Title: Re: calculating pH and
Post by: enahs on September 02, 2007, 09:37:57 PM
The answer you are giving as the correct answer for the conditions you are giving are for 0.39 g of Ba(OH)2.


However 3.6 g is much closer to the real solubility value.


It looks like when working the solution they forgot to divide by 0.1L.


Title: Re: calculating pH and
Post by: kimi85 on September 02, 2007, 10:05:12 PM
okay. thank you. :)