Question

Barium sulfate, BaSO4, is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A barium sulfate solution, sometimes called a cocktail, is ingested by the patient, whose stomach and intestines can then be visualized via X-ray imaging. If a patient ingests 200 mL of a saturated barium sulfate solution, how much toxic Ba2+ ion has the patient consumed?

The solubility product Ksp of BaSO4 is 1.10×10−10.

Express your answer to three significant figures and include the appropriate units.

Please help! Please show steps if possible! THANK YOU!!

Answer 1

Ksp = [Ba2+][SO42-]

1.1*10^-10=(s)*(s)

1.1*10^-10= 1(s)^2

s = 1.049*10^-5 M

This is molarity of BaSO4 saturated solution.

volume , V = 200 mL

= 0.2 L

use:

number of mol,

n = Molarity * Volume

= 1.049*10^-5*0.2

= 2.098*10^-6 mol

Mol of Ba2+ = mol of BaSO4

= 2.098*10^-6 mol

Molar mass of Ba = 137.3 g/mol

use:

mass of Ba2+,

m = number of mol * molar mass

= 2.098*10^-6 mol * 137.3 g/mol

= 2.881*10^-4 g

Answer: 2.88*10^-4 g