What is the mass (g) of nickel(II) nitrate (182.71 g/mol) dissolved in 160.4 mL of 0.100 M Ni(NO3)2 solution?
To determine the mass (g) of nickel(II) nitrate dissolved in the solution, we can use the formula:
mass (g) = concentration (mol/L) × volume (L) × molar mass (g/mol)
Given:
Molar mass of nickel(II) nitrate (Ni(NO3)2) = 182.71 g/mol
Volume of solution (V) = 160.4 mL = 0.1604 L
Concentration (C) = 0.100 mol/L
Substituting the given values into the formula:
mass (g) = 0.100 mol/L × 0.1604 L × 182.71 g/mol
Calculating this equation:
mass (g) = 2.941 g
To find the mass of nickel(II) nitrate dissolved in the solution, we need to use the concentration and volume of the solution along with the molar mass of nickel(II) nitrate. Here are the steps to solve the problem:
Step 1: Convert the volume of the solution from milliliters (mL) to liters (L). We know that 1 L is equal to 1000 mL, so:
Volume (L) = Volume (mL) / 1000
Volume (L) = 160.4 mL / 1000 = 0.1604 L
Step 2: Determine the number of moles of nickel(II) nitrate in the solution using the formula:
Moles = Concentration (M) x Volume (L)
Since we have the concentration (0.100 M) and volume (0.1604 L), we can calculate the moles:
Moles = 0.100 M x 0.1604 L = 0.01604 mol
Step 3: Calculate the mass of nickel(II) nitrate using the molar mass (182.71 g/mol) and the number of moles:
Mass (g) = Moles x Molar mass
Mass (g) = 0.01604 mol x 182.71 g/mol
By carrying out the calculation, we get:
Mass (g) = 2.931 g
Therefore, the mass of nickel(II) nitrate dissolved in 160.4 mL of 0.100 M Ni(NO3)2 solution is 2.931 grams.