0.100g of Cu (OH) 2 was added to a beaker which was filled to the 3.00L mark with water. what is the pOH of the solution

Question

Jenkins

Chemistry

23 February, 03:40

0.100g of Cu (OH) 2 was added to a beaker which was filled to the 3.00L mark with water. what is the pOH of the solution

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Answers (1)

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Morgan · Answer 1

3.466

Explanation:

First calculate the molarity using mass and volume

Mass = 0.100 g of Cu (OH) 2

Volume = 3.00 L

Find molar mass of solute as : 63.546 + (15.9994+1.00794) * 2 = 97.56068 g/mol

Convert grams to moles as; 0.100/97.56068 = 0.0010250031 moles

Determine molarity = 0.0010250031/3.00 = 0.0003416677 M Cu (OH) 2

pOH = - log [OH⁻]

pOH = - log [0.0003416677]

pOH = 3.466