1. What is the difference between equivalence point and endpoint?
2. In a titration with a strong acid and a strong base, why used phenolphthalein as the indicator?
3. If the color remains clear, then is the solution acidic or basic?
Data.
Trial Initial volume Final volume moles of base moles of acid concentration of acid
1 0.14mL 15.74mL
2 0.02mL 14.40mL
3 0.05mL 15.11mL
Average of the acid concentration:
Procedure.
A student added 20.00mL of acid to a Erlenmeyer flask along with 2-3 drops of indicator. Then using a 0.106 M base, the student titrated the solution. The color will change from clear to pink as you add the base. Once, you observe a faint pink color for 10 seconds, then you are complete. The data above is taken from 3 trials of titrations after adding the necessary base. (HCl - acid and NaOH -base) This neutralization is a 1:1 mole ratio.
1. What is the difference between equivalence point and endpoint?
2. In a titration with a strong acid and a strong base, why used phenolphthalein as the indicator?
3. If the color remains clear, then is the solution acidic or basic?
Data.
Trial Initial volume Final volume moles of base moles of acid concentration of acid
1 0.14mL 15.74mL
2 0.02mL 14.40mL
3 0.05mL 15.11mL
Average of the acid concentration:
Procedure.
A student added 20.00mL of acid to a Erlenmeyer flask along with 2-3 drops of indicator. Then using a 0.106 M base, the student titrated the solution. The color will change from clear to pink as you add the base. Once, you observe a faint pink color for 10 seconds, then you are complete. The data above is taken from 3 trials of titrations after adding the necessary base. (HCl - acid and NaOH -base) This neutralization is a 1:1 mole ratio.
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