Question
For the H2SO4 and NaOH titration, the endpoint is ideally reached when a green color is observed. If your solution ends up a very dark blue colour, you have over titrated. In this case, will your calculated concentration of H2SO4 be lower or higher than the true value?
Question 1 options:
Higher because more volume of NaOH is being used to titrate the moles of H2SO4.
No effect because the moles of H2SO4 titrated does not change.
Lower because more volume of NaOH is being used to titrate the moles of H2SO4.
Lower because more volume of H2SO4 is being used to titrate the moles of NaOH.
Higher because more volume of H2SO4 is being used to titrate the moles of NaOH.
Question 1 options:
Higher because more volume of NaOH is being used to titrate the moles of H2SO4.
No effect because the moles of H2SO4 titrated does not change.
Lower because more volume of NaOH is being used to titrate the moles of H2SO4.
Lower because more volume of H2SO4 is being used to titrate the moles of NaOH.
Higher because more volume of H2SO4 is being used to titrate the moles of NaOH.
Answers
GPT-4o mini
In a titration, you determine the concentration of an unknown solution (in this case, H2SO4) by using a titrant (NaOH) to neutralize it. The endpoint is indicated by a color change due to the indicator used.
If you over-titrate (i.e., you continue adding NaOH past the endpoint), you will be using more NaOH than necessary to reach the equivalence point. As a result, you will calculate a higher volume of NaOH used in the calculation of the concentration of H2SO4. Since the amount of NaOH used (which should be equal to the amount of H2SO4 neutralized at the equivalence point) is now inaccurately high, the calculated concentration of H2SO4 will be lower than its true concentration:
- The moles of NaOH used are greater than they should be, which leads to a falsely low calculated concentration of H2SO4.
Therefore, the correct answer is:
**Lower because more volume of NaOH is being used to titrate the moles of H2SO4.**
If you over-titrate (i.e., you continue adding NaOH past the endpoint), you will be using more NaOH than necessary to reach the equivalence point. As a result, you will calculate a higher volume of NaOH used in the calculation of the concentration of H2SO4. Since the amount of NaOH used (which should be equal to the amount of H2SO4 neutralized at the equivalence point) is now inaccurately high, the calculated concentration of H2SO4 will be lower than its true concentration:
- The moles of NaOH used are greater than they should be, which leads to a falsely low calculated concentration of H2SO4.
Therefore, the correct answer is:
**Lower because more volume of NaOH is being used to titrate the moles of H2SO4.**