Table arity of NaOH Initial Volume on burette 0.00 mL 46.20m Final Volume of Bur
ID: 1038168 • Letter: T
Question
Table arity of NaOH Initial Volume on burette 0.00 mL 46.20m Final Volume of Burette Volume of NaOH used Volume of Ascorbic Acid solution used 20.00mL Calculate the number of moles of NaOH used in the titration. Use the balanced chemical equation to calculate the number of moles of ascorbic acid in the 20.0 mL sample Use the chemical formula to calculate the molar mass of ascorbic acid. Calculate the mass of ascorbie acid in the 20.0 mL sample in mg. Use a simple proportion to calculate the mass of ascorbic acid in a tablet if one tablet was used to make 200.0 mL of solution. Calculate the percent error of your measured value compared against the manufacturer's reported value of 200 mg of Ascorbic Acid per tablet Page 4 of 5Explanation / Answer
Molarity = number of moles of solute / volume of the solution in litter
therefore ; number of moles of NaOH in 48.2 ml of 0.1 Molar solution = 0.1 x 48.2x10-3 L = =0.00482 moles
2.
HC6H7O6 + NaOH ? NaC6H7O6 + H2O
vitamin c
balanced equation is also same as above
NaOH + C6H8O6? C6H7O6Na + H2O
Molar mass of ascorbic acid = 6x 12 + 7x1 + 6x 16 = 175g
4.
volume of NaOH = 48.2 mL
molarity of NaOH = 0.1 M
volume of ascorbic acid used = 20 mL
molarity of ascorbic acid = ?
M1V1 = M2V2
M2 = (M1V1) / V2 => (48.2 x 0.1 ) / 20 = 0.241 Molar solution of ascorbic acid
Molarity = number of moles of solute / volume of the solution in litter
no. of moles of ascorbic acid = 0.241 x 20x10-3 = 0.00482 moles
molar mass of ascorbic acid = 175g
therefore, 175x 0.00482 moles of ascorbic acid = 0.8435 g = 0.0008435 mg of ascorbic acid present in it.
5.
need to known the data of tablet you have used
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