Calculate the pH for a titration of 0.20M CH3COOH (aq) with 0.20 M NaOH (aq)?

Answer 1

Can you say the volume of CH3COOH and NaOH?

Answer 2

NH3 is a weak base. when we titr a sol. with yet another, a trademark is used to reveal the top aspect of titration. we upload sufficient volume of HCl till inicator colour adjustments and the most suitable pH relies upon on the indicator. at that aspect each of the NH3 is titred regardless of it really is equilibrium consistent. the purpose for titration is asking the quantity of titrant mandatory 25*0.02=x(ml)*.0.5 --> x=33.3ml

Answer 3

First when you ask such a question give, please the pKa of the weak acid. I found on the webb, it is 4.77

for a buffer such as yours you neutralize your acid by NaOh since they have the same molarity and are monovalent both.

when you have pure acid the pH =( pk -logc)/2

here pH = (4.77-log0.2)/2 =(4.77-(/0.7))/2 =5.44/2 =2.72

this the pH without addition of NaOH

when you add half of NaOH you have pH =pKa= 4.77

and at the end you nautralize the acetic acid where the

pKb is 14-4.77 = 9.23