if you dissolve 1.60g of Cu(No3)2 in 100mL of water, calculate the molarity of the resulting solution ?
To calculate the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters). Here's how you can calculate the molarity using the given information:
1. Convert the mass of the solute to moles. To do this, you need to know the molar mass of Cu(NO3)2, which is the sum of the atomic masses of its constituent elements. The atomic masses (from the periodic table) are:
- Cu: 63.55 g/mol
- N: 14.01 g/mol (two nitrogen atoms)
- O: 16.00 g/mol (six oxygen atoms)
To calculate the molar mass of Cu(NO3)2:
Molar mass = (63.55 g/mol) + (14.01 g/mol × 2) + (16.00 g/mol × 6)
= 63.55 g/mol + 28.02 g/mol + 96.00 g/mol
= 187.57 g/mol
Now, convert the given mass of Cu(NO3)2 to moles:
Moles of Cu(NO3)2 = mass / molar mass
= 1.60 g / 187.57 g/mol
≈ 0.00853 mol
2. Convert the volume of the solution to liters. The given volume is 100 mL, so to convert it to liters:
Volume = 100 mL × (1 L / 1000 mL)
= 0.100 L
3. Calculate the molarity using the formula:
Molarity (M) = moles of solute / volume of solution (in liters)
= 0.00853 mol / 0.100 L
= 0.0853 M
Therefore, the molarity of the resulting solution is approximately 0.0853 M.