WILL GIVE BRAINLIEST AND 20 POINTS! Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate, Ba(OH)2 * 8 H2O. What mass of Ba(OH)2 * 8 H2O would be required to make 500 mL of a solution that is 0.1500 M hydroxide ions? [hint: calculate the molar mass of barium hydroxide octahydrate].

Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate. Ba(OH)2 • 8H2O. What mass of Ba(OH)2 • 8H2O would be required to make 500.0 mL of a solution that is 0.1500 M in hydroxide ions?

Step-by-Step Solution:

Solution 70P:

Here we have to calculate the mass  of Ba(OH)2 • 8H2O would be required to make 500.0 mL of a solution that is 0.1500 M in hydroxide ions.

Step 1

Given:

Volume of Ba(OH)2 • 8H2O = 500.0 mL or 0.5000 L

Concentration of OH- ion = 0.1500 M

Molecular mass of Ba(OH)2 • 8H2O = 315.4 g

Thus the mass can be calculated as,

0.500L 

= 11.83 g Ba(OH)2.8H2O

Thus the mass of Ba(OH)2 • 8H2O is found to be 11.83 g .