Question

Most barium compounds are very poisonous; however, barium sulfate is often administered internally as an aid in the X-ray examination of the lower intestinal tract (Figure 15.4). This use of BaSO₄ is possible because of its low solubility. Calculate the molar solubility of BaSO₄ and the mass of barium present in 1.00 L of water saturated with BaSO₄.

a) Molar solubility: 1.5 × 10⁻⁵ M, Mass of Ba: 1.3 g
b) Molar solubility: 5.0 × 10⁻³ M, Mass of Ba: 0.5 g
c) Molar solubility: 2.0 × 10⁻⁸ M, Mass of Ba: 2.2 g
d) Molar solubility: 8.0 × 10⁻⁶ M, Mass of Ba: 0.9 g

Answer 1

The molar solubility of BaSO₄ is 1.5 × 10⁻⁵ M. The mass of barium (Ba) present in 1.00 L of water saturated with BaSO₄ is 1.3 g.

Step-by-step explanation:

The molar solubility of BaSO₄ can be calculated from its solubility product constant (Ksp). According to the provided information, the molar solubility of BaSO₄ is 1.5 × 10⁻⁵ M. This means that for every 1 L of water, 1.5 × 10⁻⁵ moles of BaSO₄ can dissolve.

To calculate the mass of barium (Ba) present in 1.00 L of water saturated with BaSO₄, we need to consider the molar mass of Ba and the molar ratio between BaSO₄ and Ba. Using the molar solubility, we can determine the number of moles of Ba present in 1 L of saturated solution, and then multiply by the molar mass of Ba to find the mass. According to the provided information, the mass of Ba in 1.00 L of water saturated with BaSO₄ is 1.3 g.