Homework Help: Chemistry

Posted by Summer on Tuesday, January 10, 2012 at 1:44pm.

Consider the titration of 80.0 mL Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.

a.) 0.0 mL
*Which molecular equation do I use?

b.) 20.0mL

Ba(OH)2__+2HCl_+=>+_BaCl2_+____2HOH
80.0 mL__20.0mL
0.100M___0.400M
.008 mol_.008 mol
.004 left_ 0 left__.004 mol produced

pH = pKa
pH = -Log(1.05x10^-12)
pH = 11.98

*Did I do this one correctly?

Chemistry - DrBob222, Tuesday, January 10, 2012 at 4:09pm
You didn't include the molarity of the Ba(OH)2.
Chemistry - Summer, Tuesday, January 10, 2012 at 8:24pm
0.100 M

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