Question

For a tablet containing 500. mg of vitamin C, calculate how many ml of 0.095 M NaOH is required to reach the equivalence point.

Answer 1

Answer:

mL of NaOH required =29.9mL

Explanation:

Let us calculate the moles of vitamin C in the tablet:

The molar mass of Vitamin C is 176.14 g/mole

$moles=\frac{mass}{molarmass}=\frac{500mg}{176.14}=\frac{0.5}{176.14}=0.0028$

Thus we need same number of moles of NaOH to reach the equivalence point.

For NaOH solution:

$moles=MolarityXvolume=0.095Xvolume$

$0.00283=0.095Xvolume$

$volume=0.0299L=29.9mL$