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18 Dec 2019

Vitamin C is ascorbic acid, HC6H7O6. It will react with sodium hydroxide as shown in the following equation: HC6H7O6(aq) + NaOH(aq) yields NaC6H7O6(aq) + H2O(l). A 3.632g vitamin pill is crushed, dissolved in 100.0mL water and titrated with sodium hydroxide. Calculate the moles of ascorbic acid titrated if the equivalence point is reached when 39.98mL of 0.0116M NaOH is added. Calculate the mass percent of ascorbic acid in the vitamin pill.

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Vitamin C (also called ascorbic acid) is a weak organic acid whose formula is HC6H7O6. Only one hydrogen is acidic. A pharmacist suspects that the Vitamin C tablets just received are not pure. When a single 500 mg tablet is dissolved in 200mL of water and tiltrated with standard barium hydroxide solution that is 0.1045M, it requires 12.23mL for complete tiltration. What is the percent vitamin C in these tablets? (write chemical equation).

 
Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg).  =?

A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NaOH solution. From 
the results of this titration, the mg of ascorbic acid in the tablet was calculated.
Molecular formulas:
Potassium hydrogen phthalate: HKC8H4O4
Acetic acid: C2H4O2
Ascorbic acid: C6H8O6
Assume that all 3 acids are monoprotic acids.



Mass of KHP used for standardization (g) 0.5464
Volume of NaOH required to neutralize KHP (mL) 13.31
Volume of vinegar sample titrated (mL) 5.00
Volume of NaOH required to neutralize vinegar in (mL) 8.40
Molecular weight of ascorbic acid (g/mol) 176.1271
Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 13.85

What is the Molecular Weight of KHP (HKC8H4O4) in g/mol? 204.2220 
How many moles of KHP were used in the standardization of the NaOH solution? 0.002595
Calculate the concentration of NaOH solution in (mol/L). 0.188433
Calculate the molarity of the vinegar solution (mol/L). 0.303377

Consider the titration of 80.0 mL of 0.0200 M C5H5N (a weak base; Kb = 1.70e-09) with 0.100 M HNO3.

Calculate the pH after the following volumes of titrant have been added:

(a) 0.0 mL pH =

(b) 4.0 mL pH =

(d) 12.0 mL pH =

(e) 16.0 mL pH =

(f) 25.6 mL pH =

PART TWO:

A buffer solution contains 0.14 mol of ascorbic acid (HC₆H₇O₆) and 0.84 mol of sodium ascorbate (NaC₆H₇O₆) in 2.80 L.
The K_a of ascorbic acid (HC₆H₇O₆) is K_a = 8e-05.

(a) What is the pH of this buffer?

pH =

(b) What is the pH of the buffer after the addition of 0.07 mol of NaOH? (assume no volume change)

pH =

(c) What is the pH of the original buffer after the addition of 0.21 mol of HI? (assume no volume change)

pH =

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