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Nickel(II) Nitrate Solution Composition Analysis
Chapter 10, Problem 1(choose chapter or problem)
A solution is prepared by dissolving 12.15 g of nickel(II) nitrate in 175 mL of water (d = 1.00 g/mL). Calculate
(a) the mass percent of nickel(II) nitrate in the solution.
(b) the mole fraction of nickel(II) ions in the solution.
Questions & Answers
QUESTION:
A solution is prepared by dissolving 12.15 g of nickel(II) nitrate in 175 mL of water (d = 1.00 g/mL). Calculate
(a) the mass percent of nickel(II) nitrate in the solution.
(b) the mole fraction of nickel(II) ions in the solution.
ANSWER:Step 1 of 3
a.
Mass of the water = product of density and volume.
So, the mass of the water in the solution is as follows:
\(1.00\;\frac{{\rm{g}}}{{{\rm{mL}}}} \times 175\;{\rm{mL}} = 175\;{\rm{g}}\)
The total mass of the solution is:
\(12.15\;{\rm{g}} + 175\;{\rm{g}} = 187.15\;{\rm{g}}\)
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Nickel(II) Nitrate Solution Composition Analysis
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In this analysis, we determine the composition of a solution prepared by dissolving 12.15g of nickel(II) nitrate in 175mL of water (density 1.00 g/mL). The mass percent of nickel(II) nitrate is found to be approximately 6.50%, and the mole fraction of nickel(II) ions in the solution is calculated as 0.00672.