Answer:
2.80 × 10⁻³ M
Explanation:
There is some info missing. I think this is the original question.
One cup of fresh orange juice contains 127 mg of ascorbic acid (vitamin C, C₆H₈O₆). Given that one cup = 257.6 mL, calculate the molarity of vitamin C in orange juice.
Express your answer to an appropriate number of significant figures with the appropriate units.
Step 1: Convert the mass of ascorbic acid to grams
We will use the relationship 1 g = 1,000 mg.
[tex]127mg \times \frac{1g}{1,000mg} = 0.127g[/tex]
Step 2: Calculate the moles corresponding to 0.127 g of ascorbic acid
The molar mass of ascorbic acid is 176.13 g/mol.
[tex]0.127g \times \frac{1mol}{176.13g} = 7.21 \times 10^{-4} mol[/tex]
Step 3: Convert the volume of the solution to liters
We will use the relationship 1 L = 1,000 mL.
[tex]257.6mL \times \frac{1L}{1,000mL} = 0.2576L[/tex]
Step 4: Calculate the molarity of the solution
[tex]M = \frac{7.21 \times 10^{-4} mol}{0.2576L} = 2.80 \times 10^{-3} M[/tex]
