When setting up their experiment, a student discovered that the solution in their flask turned bright pink upon adding 2 drops of the indicator, even before beginning the titration. What do you suspect was the mistake that the student made?
3 answers
I have no idea what experiment you are doing; therefore, I can't answer the question AND I don't even know the name of the indicator you were using. IF phenolphthalein was the indicator, that meant the solution in the flask was pH 8.5 or greater.
You are not giving us enough information to answer your question.
Speculating a bit, if you are supposed to use a standard NaOH solution is the buret, and an acid solution of unknown concentration in the flask with phenolphthalein indicator, could you have reversed where you placed the two solutions?
Placing the NaOH in the flask would account for what you observed.
Tell us more if my assumptions about the procedure are incorrect.
Speculating a bit, if you are supposed to use a standard NaOH solution is the buret, and an acid solution of unknown concentration in the flask with phenolphthalein indicator, could you have reversed where you placed the two solutions?
Placing the NaOH in the flask would account for what you observed.
Tell us more if my assumptions about the procedure are incorrect.
Describe how you would weigh your KHP samples, if you didn’t know about weighing by differences. Mentioning any differences between your method and the method we made you use, explain why we use the technique of weighing by difference.