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Making a 0.150 M Ba(OH)? Solution: A Step-by-Step Guide
Chapter 4, Problem 70P(choose chapter or problem)
Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate. \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\). What mass of \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\) would be required to make 500.0 mL of a solution that is 0.1500 \(M\) in hydroxide ions?
Questions & Answers
QUESTION:
Barium hydroxide, often used to titrate weak organic acids, is obtained as the octahydrate. \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\). What mass of \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\) would be required to make 500.0 mL of a solution that is 0.1500 \(M\) in hydroxide ions?
ANSWER:Step 1 of 3
Here we have to calculate the mass of \(\mathrm{Ba}(\mathrm{OH})_{2} \cdot 8 \mathrm{H}_{2} \mathrm{O}\) would be required to make 500.0 mL of a solution that is 0.1500 \(M\) in hydroxide ions.
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Making a 0.150 M Ba(OH)? Solution: A Step-by-Step Guide
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Learn how to calculate the amount of Barium hydroxide, Ba(OH)?, needed to prepare a specific molar concentration. This tutorial breaks down the relationship between moles of hydroxide ions and moles of Ba(OH)?, guiding users through each step for precise results. Embrace the essence of molarity in solution preparation.