Question

orange juice can be considered as an aqueous solution in which one of the solutes is vitamin C. either any orange juice in which the concentration of vitamin C is 0.00214 mol/La) you drink 250 ml of this orange juice. how much vitamin C did you consume?b) adults are recommended to consume approximately 80mg of vitamin C per day. How much of this orange juice will you need to drink to consume this mass of vitamin C? note that the chemical formula of vitamin C is C6 H8 O6.

Answer 1

Explanation:

a) First, let's find out how many moles are there into 250 mL of orange juice:

0.00214 mol ---- 1000 mL (1L)

x mol ---- 250 mL

1000x = 250 * 0.00214

x = 0.535/1000

x = 5.35 x 10^-4 mol

Now let's transform it to grams. For this, we need to use the molar mass of vitamin C and the following formula: m = n*MM

MM of vitamin C = 176 g/mol

m = 5.35 x 10^-4 * 176

m = 0.09416 g

m = 94.16 mg

Answer a): 94.16 mg of vitamin C

b) Let's transform 80 mg of vitamin C into moles using the formula: n = m/MM

m of vitamin cC = 80 mg = 0.08 g

MM = 176 g/mol

n = 0.08/176

n = 4.54 x 10^-4 moles

Now let's calculate the quantity in mL:

0.00214 mol ---- 1000 mL (1L)

4.54 x 10^-4 moles ---- x mL

0.00214x = 4.54 x 10^-4 * 1000

x = 0.4545/0.00214

x = 212 mL

Answer b): 212 mL

Calculation of the molar mass of C6H8O6:

(6*12)+(8*1)+(6*16) = 176 g/mol