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snow_tiger [21]
3 years ago
7

An aqueous solution is prepared by dissolving 15.6 g of Cu(NO3)2 ⋅ 6 H2O in water and diluting to 345 mL of solution. What is th

e molarity of the NO3- ion in this solution?
A. 0.417 M
B. 0.121 M
C. 0.306 M
D. 0563 M
E. 0.834 M
Chemistry
1 answer:
Vladimir [108]3 years ago
3 0

<u>Answer:</u> The molarity of NO_3^- ions in the solution is 0.306 M

<u>Explanation:</u>

To calculate the molarity of solution, we use the equation:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

We are given:

Mass of solute (Cu(NO_3)_2.6H_2O) = 15.6 g

Molar mass of (Cu(NO_3)_2.6H_2O) = 295.6 g/mol

Volume of solution = 345 mL

Putting values in above equation, we get:

\text{Molarity of }Cu(NO_3)_2.6H_2O=\frac{15.6g\times 1000}{295.6g/mol\times 345mL}\\\\\text{Molarity of }Cu(NO_3)_.6H_2O=0.153M

As, 1 mole of (Cu(NO_3)_2.6H_2O) produces 1 mole of copper (II) ions and 2 moles of nitrate ions.

So, molarity of NO_3^- ions = (2 × 0.153) = 0.306 M

Hence, the molarity of NO_3^- ions in the solution is 0.306 M

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