Find the molarity of solution in which 69g nitric acid is present in 500ml of solution ?
Your School SUBJECT is CHEMISTRY.
mols HNO3 = grams/molar mass = ?
M HNO3 = mols HNO3/L solution = ?
Approximately 2 M but that's an estimate.
To find the molarity (M) of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
First, let's calculate the number of moles of nitric acid (HNO3) present in 69g:
1. Find the molar mass of nitric acid (HNO3):
- Mass of 1 hydrogen atom (H) = 1g/mol
- Mass of 1 nitrogen atom (N) = 14g/mol
- Mass of 3 oxygen atoms (O) = 3 * 16g/mol = 48g/mol
- Molar mass of HNO3 = 1g/mol + 14g/mol + 48g/mol = 63g/mol
2. Calculate the number of moles of nitric acid using the formula:
- Moles = Mass / Molar mass
- Moles of HNO3 = 69g / 63g/mol = 1.1 mol
Next, we need to convert the volume of the solution from milliliters (ml) to liters (L):
3. Volume of solution = 500ml = 500/1000L = 0.5L
Now, we can calculate the molarity of the solution using the formula:
Molarity (M) = Moles of solute / Volume of solution in liters
4. Molarity (M) = 1.1 mol / 0.5 L = 2.2 M
Therefore, the molarity of the solution in which 69g of nitric acid is present in 500ml of solution is 2.2 M.