Do I need to first figure out the PH?
I believe that a= 3
and b=2.87
therefore it will require more naoh to titrate the acetic acid.
I am not sure i figured the ph of acetic acid correctly, or if i am on the correct path here...
Suppose you have two solutions to titrate with NaOH: (a) 10 ml of.1M HCL (b) 10 ml of .1M CH3COOH
would you expect either of the solutions to require different volumes of NaOH in order to reach an end point? Explain
3 answers
No, you don't need to calculate pH. What is the concept of titrating an acid with a base; i.e., when does the indicator show you have reached the end point? The answer to that is that when moles of acid = moles base the indicator tells you to quit adding base. So how many moles are in the 10 mL of 0.1M HCl? That is 0.01 x 0.1 = 0.001 moles HCl.
How many moles are in the 10 mL of 0.1M CH3COOH? That is 0.01 x 0.1 = 0.001. So the end point will be the same no matter which acid is used. What counts is how many moles of the acid you have.
How many moles are in the 10 mL of 0.1M CH3COOH? That is 0.01 x 0.1 = 0.001. So the end point will be the same no matter which acid is used. What counts is how many moles of the acid you have.
YES ,Due to hydro chloric acid being a strong acid it would require large volume of sodium hydroxide in order to reach the end point , while acetic acid acid requires smaller amount of volume due to it being a weaker acid than hydro chloric acid
0 answers