Question

Suppose you are a food chemist working for a company that makes and manufactures soda. Your job is to create a new soft drink with the ingredients available to you. There is one problem—you need 1 liter of phosphoric acid solution, and the phosphoric acid available to use has a concentration of 0.01 M. This is much too high to add to your soda without distorting the flavor. Typically, there are about 45 milligrams of phosphoric acid per 12 ounce can of soda. Here is your task:

Convert the 45 milligrams of phosphoric acid (H3PO4) into grams and then into moles.
0.00046 moles or 4.6×10-4 moles
Given that 12 ounces is equal to about 0.35 liter, find the molarity of the phosphoric acid in a typical can of soda (45 milligrams). 0.0013 M or 1.3×10-3 M
Using the dilution equation, determine how much of the stock solution (0.01 M H3PO4) you will need to make 1 liter of the concentration typically used in soda.
0.13 liter or 130 milliliters

Answer 1

45 mg × 1 g/1000 mg = 0.045 g

0.045 g × 1 mol/98 g = 0.00046 mol

0.00046 mol/0.35 L = 0.0013 M

0.01 M × x = 0.0013 M × 1 L

Solution: 130 milliliter

Answer from Edmentum

Answer 2

The answer to your question is given after the questions so I just explain how to get it.

Step-by-step explanation:

a)

Get the molecular weight of Phosphoric acid

H₃PO₄ = (3 x 1) + (31 x 1) + (16 x 4)

= 3 + 31 + 64

= 98 g

98 g ----------------- 1 mol

0.045 g --------------- x

x = (0.045 x 1) / 98

x = 0.045 / 98

x = 0.00046 moles or 4.6 x 10 ⁻⁴

b)

Molarity =
`(moles)/(volume)`

Molarity =
`(0.00046)/(0.35)`

Molarity = 0.0013 or 1.31 x 10⁻³

c)

Formula C₁V₁ = C₂V₂

V₁ = C₂V₂ / C₁

Substitution

V₁ = (0.0013)(1) / 0.01

Simplification and result

V₁ = 0.0013 / 0.1

V₁ = 0.13 l = 130 ml