Part a before you begin, you collect and determine the following information: molarity of acid 0.141 m volume of acid (ml) 25.00 ml volume of acid (l) 0.025 l imagine your flask contains hcl (hydrochloric acid) and your burette contains koh (potassium hydroxide). you can add the base in large or small increments. you stop when the color inside the flask is a faint pink color. remember, you want the color to be a faint pink color, not dark pink. if you notice the color changing but then returning to colorless, that tells you that you are getting close to the equivalence point. you continue titrating until the faint pink color remains. and you enter your data in the table below: volume of base (ml) 35.38 ml volume of base (l) 0.03538 l write a balanced equation for this reaction. part b from your data above, fill in the following values: molarity of acid volume of acid molarity unknown volume of base part c calculate the number of moles of hcl that were in your flask. part d how many moles of naoh will there be? part e calculate the concentration of the naoh in the titration.