[planke]

Can someone please help me with this problem?

You dissolve 0.34 g of KHP in 20 mL of water and titrate with the NaOH solution. To the nearest mL, calculate the volume of NaOH solution expected assuming that the NaOH concentration is ~0.1 M.

[Sev]

How many moles of KHP do you have?  How many moles of NaOH will this react with?

[planke]

But... I don't know what the reaction would be in order to find the no. of moles of NaOH to make the conversion from moles KHP to moles NaOH.

[Sev]

They react 1:1

KC₈H₅O₄ +NaOH → KNaC₈H₄O₄ + H₂O

[planke]

Thanks a lot!
I was just having trouble setting up the reaction.

[planke]

Do you know how to solve this problem?

You transferred 20. mL of acetic acid solution to an Erlenmeyer flask and added 2 drops of phenolphthalein solution. You filled your buret with 0.10 M NaOH so that the initial buret reading was 1.47 mL. After titrating your sample to the faint-pink phenolphthalein endpoint, the final buret reading was 17.41 mL.
a) How many moles of NaOH were delivered to the flask?

 
b) What is the concentration of the acetic acid solution?
 

[Sev]

a) How many moles of NaOH were delivered to the flask?

15.94mL of 0.1M NaOH is how many moles?

b) What is the concentration of the acetic acid solution?

Hint: Rxn is 1:1 again.

[planke]

I keep getting part B wrong for some reason. Isn't it just 1mole acetic acid divided by 0.01594 Liters?

[planke]

Never mind... I think I figured it out.