1-What is the difference between the end point and equivalence point in a titration? How can you tell them apart?
2- If you have 15 mL of 2 M HCl, how many moles are present in solution?
3-Student 1 is titrating NaOH into HCl, the student pours 10.00 mL of 2 M HCl into an erlenmeyer flask and adds 2 drops of phenolphthalein indicator and 15 mL of deionized water. The student places the burette with NaOH inside of it above the acid solution and records that there are 30 mL of 1 M NaOH in the burette. The student turns the stopcock to begin the titration. The solution in the flask turns pink and the student stops the titration. The student records that the volume of 1 M NaOH is now at 9 mL. How many moles of HCl were there? How many moles of NaOH were added to the flask during the titration? What is the experimental molar ratio of NaOH:HCl? What is the theoretical ratio? What is the percent error?
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