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Chemistry problem help, titration?
I have been working on this for hours and still feel like I have no idea what is going on. Please explain how I can get the answer too. I need to understand this. Thanks!
Suppose exactly 25.00 mL of water was pipetted into a flask containing 25.00 mL of a stock solution of a weak monoprotic acid. The solution was titrated with 0.1025 M NaOH(aq). Estimate the equivalence point volume from the data below. Calculate the molarity of the acid solution (total volume=50.00 mL).
Volume of NaOH added pH
28.40 mL 5.05
28.50 5.22
28.60 5.49
28.70 6.40
28.80 10.06
28.90 10.40
29.00 10.58
29.10 10.71
29.20 10.81
1 Answer
- Simonizer1218Lv 77 years agoFavorite Answer
When you titrate a weak acid with a strong base (NaOH), the pH at the equivalence point will be >7. This is because the salt formed will be a basic salt.
Equivalence point volume = 28.80 ml
moles NaOH at this volume = 0.02880 L x 0.1025 mol/L = 0.002952 moles NaOH
moles weak acid = 0.002952
volume of weak acid = 25 ml = 0.025 L
molarity of original acid solution = 0.002952 mol/0.025 L = 0.1181 M
The concentration of weak acid in the 50 ml (after adding 25 ml water) = 0.05904 M
