HCL is added to a solution containing 0.5 N sodium acetate until its concentration reaches 0.51 M HCL. What is the pH of the solution? NOTE: Chegg has responded twice to this post, and both have different answers. so my question then is what does "until its concentration reaches 0.51 M HCL. " mean? To me, it means it is above and beyond in excess of another .5 M HCL that reacted with acetate. so a total of 1.01 M HCL/.....and need to get to soln of 1.89 pH. I'd appreciate your time and HELP!
0.5 M HCl will react with 0.5 M sodium acetate to form 0.5 M acetic acid.
Additional 0.51 M HCl is added.
Now solution contains 0.51 M HCl and 0.5 M acetic acid.
0.51 M HCl on dissociation gives 0.51 M ions.
0.5 M acetic acid on dissociation gives x M ions and x M acetate ions. 0.5-x M of acetic acid remains.
Total
Approximation: 0.5-x is approximately equal to 0.5 as x is much smaller than 0.5 due to small value of Ka.
This is quadratic equation with solution
or
The negative value is discarded as concentration cannot be negative.
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