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Questions
1. Answer the following questions using your experimental data. Label your answers in order according to and designated with the letters given below. Where applicable, you must show ALL WORK to receive credit.

(a) What was the equivalence point (mL of C6H8O7 needed to reach the end point) for Trial 1?

(b) What was the equivalence point (mL of C6H8O7 needed to reach the end point) for Trial 2?

(c) How many moles of NaOH reacted in Trial 1?

(d) How many moles of NaOH reacted in Trial 2?

(e) What was the experimental molarity (M) for NaOH in Trial 1?

(f) What was the experimental molarity (M) for NaOH in Trial 2?

(g) What was the average molarity (M) of the two trials?

2. (a) According to your experimental data, what volume of C6H8O7 represents the half-equivalence (a.k.a. half-neutralization) point in this titration?

(b) What is the pH of the solution at the half-neutralization point?

3. The NaOH used in this lab should have been 0.1M, since you were to make it as such (see Step 15 in lab document). Compare your standardized average molarity of NaOH in this lab to 0.1M. How do the values compare? How close was your NaOH dilution to actually being 0.1M NaOH? Calculate your percent error against the average standardized value from this lab. (You must show all work to receive credit.)

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Questions

1.Answer the following questions using your experimental data. Label your answers in order according to and designated with the letters given below. Where applicable, you must show ALL WORK to receive credit.
(a) What was the equivalence point (mL of C6H8O7 needed to reach the end point) for Trial 1?

4.0 ml

(b) What was the equivalence point (mL of C6H8O7 needed to reach the end point) for Trial 2?

4.0 ml

(c) How many moles of NaOH reacted in Trial 1?

Moles of NaOH = 3 · (concentration(citric acid)·volume added) = 3·(0.139M·0.0040L) = 0.0017 mol...

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