Students performed a procedure similar to Part II of this experiment (Analyzing Juices for Vitamin C Content) as described in the procedure section. Three 10.00mL samples of juice were titrated with DCP that had a standardized concentration of 9.98x10-4M. The three titrations took an average of 16.34mL of DCP. Calculate the mass (in mg) in 50.00mL of juice. (MM Ascorbic Acid = 176.124 g/mol)

Students performed a procedure similar to Part II of this
experiment (Analyzing Juices for Vitamin C Content) as described in the
procedure section. Given that molarity of DCP is 9.98x10-4 M, it took 16.34 ml
of DCP to titrate 10 mL of sample.

Amount of ascorbic acid = 0.050 L sample (0.01634 L DCP/0.01
L sample)( 9.98x10-4 mol DCP/L DCP)(1 mol Ascorbic acid/ 1mol DCP)(176.124
g/mol)(1000mg/1g)= 14.36 mg ascorbic acid

Answer Link

sebassandin sebassandin · Answer 2 · 2020-01-19T13:27:52-05:00

Answer:

\(m_{AA}=14.36mgAA\)

Explanation:

Hello,

In this case, the titration is based of the equality between the moles of the titrant and the analyte, then, in terms of molarity we define it as shown below:

\(M_{DCP}*V_{DCP}=M_{juice}*V_{juice}\)

As the ascorbic acid is the substance reacting with the DCP, we infer that the 16.34 mL of DCP completely neutralized the ascorbic acid; in such a way, solving for the molarity of the neutralized acid, one obtains:

\(M_{juice}=\frac{M_{DCP}*V_{DCP}}{V_{juice}}=\frac{9.98x10^{-4}M*16.34mL}{10.00mL} \\M_{juice}=1.63x10^{-3}M\)

Finally, by using the molar MASS of the ascorbic acid and applying the proper units conversion, the result is shown below:

\(m_{AA}=1.63x10^{-3}\frac{molAA}{L}*0.05000L*\frac{176.124gAA}{1molAA} *\frac{1000mgAA}{1gAA} \\m_{AA}=14.36mgAA\)

Therefore, 14.36 mg of ascorbic acid are contained into 50.00mL of juice.

Best regards.