What is the pH of a solution of 1 M acetic acid after addition of 0.1 equivalents of base (sodium hydroxide)?

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rona	Open Questions What is the pH of a solution of 1 M acetic acid after addition of 0.1 equivalents of base (sodium hydroxide)? Posted 205 day ago Report Abuse

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Answers (3)

MFB13

Hi Rona. You can reach me by first calling the people in charge of this website then asking to contact me personally by telling them my user name which is mfb13. They should be able to connect you with me. You can also call my business-work number which is 203-787-6662. Explain your reason for calling, ask to speak with Mike and leave your email address, phone number and a fax number if you have one so that I can contact you. My fax number is 203-787-6668 if you also need that. I hope that was helpfull.

Posted 202 day ago

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rona

Hi

Thank you very much for your answer I will try to understand what you wrote, I am trying to send you an email but I do not know from where I can send .I am really have terrible with calculation for the PH,PKA and so on and I want help from somebody please if you could .

Posted 204 day ago

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MFB13

Hi, here we are dealing with the titration of a weak acid with a strong base, hydroxide ion. Let us assume based upon what you mentioned in the problem that the volume did not increase after adding the base to the acetic acid solution. Before the titration, or before adding any base, the pH of a 1 M or 1 mol/L aqueous solution of acetic acid can be easily calculated to be at a pH of 2.38. This means that the hyrogen ion or hydronium ion concentration is the negative base ten anti-log of 2.38 which is 0.00417 mol/L or 4.17x10^-3 mol/L.

Now, when you add 0.1 eq of base to the weak acid, acetic acid, you are adding 0.1 eq. or 0.1 mol of hydroxide ion which neutralizes only 0.1 eq. or 0.1 mol of hydrogen ion which forms water. After this addition or titration step, you are left with 1.0 - 0.1 = 0.9 eq. or mol of hydrogen ion in solution. Assuming there is no volume change, the concentration of hydrogen ion left in solution is 0.9 eq/L or 0.9 mol/L. This final concentration of hydrogen ion in one liter corresponds to a pH of 2.40. So the change in pH was only about 0.02 units. Not very much change indeed. I did not have time to show my calculations here but if you email me, I will be happy to show you how I calculated the new pH.

Note that in this problem, eq/L is the same as mol/L because we are talking about a monoprotic acid and a monobasic base. That is for example, NaOH dissociates only one OH- ion only so 1 eq/L = 1 mol/L OH- ion. On the other hand, a strong base such as Ca(OH)2 or calcium hydroxide will dissociate into two hydroxide ions for every molecule of calcium hydroxide. So for example 1 mol/L of calcium hydroxide will generate 2 eq/L of OH- ion. Let me know if you need more assistance.

Posted 205 day ago

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