What is the molarity of a solution that contains 5.80 grams of nickel(II) nitrate (Ni(NO_3)_2) dissolved in 500. mL of solution?

• A. 0.116 M
• B. 0.058 M
• C. 0.040 M
• D. 0.020 M

Answer: (D)

Verified step by step guidance

1. Identify the formula of the compound: nickel(II) nitrate is Ni(NO\_3)\_2.
2. Calculate the molar mass of Ni(NO\_3)\_2 by summing the atomic masses of all atoms in the formula: Ni + 2 × (N + 3 × O).
3. Convert the given mass of nickel(II) nitrate (5.80 g) to moles using the molar mass: moles = mass / molar mass.
4. Convert the volume of the solution from milliliters to liters: 500. mL = 0.500 L.
5. Calculate the molarity (M) using the formula: \(M = \frac{\text{moles of solute}}{\text{liters of solution}}\).