A chemist added 3.15 grams of HNO3 to a solution of the same acid with concentration of 9 mol/L. dilutes the resulting solution up to the 100ml volume. The resulting solution will have what concentration?
mols solid HNO3 = grams/molar mass = ?
How much of the 9 M HNO3 did you use?
Are you neglecting the volume of the 3.15 g HNO3?
Did you make up this problem yourself or did it come to you by another path?
To find the resulting concentration of the solution, we need to use the concept of molarity, which is a measure of the concentration of a solute in a solution. The formula for molarity is:
Molarity (M) = moles of solute / volume of solution (in liters)
First, we need to calculate the moles of HNO3 added to the solution. We can use the equation:
moles = mass / molar mass
The molar mass of HNO3 is equal to the sum of the atomic masses of its elements: hydrogen (H), nitrogen (N), and oxygen (O). By looking up the atomic masses, we find:
H = 1 g/mol
N = 14 g/mol
O = 16 g/mol
Adding these together, we get:
molar mass of HNO3 = (1 * 1) + (14 * 1) + (16 * 3) = 63 g/mol
Now, divide the mass of HNO3 added (3.15 grams) by the molar mass to find the moles:
moles = 3.15 g / 63 g/mol = 0.05 mol
Next, we need to calculate the total volume of the resulting solution. The chemist diluted the solution up to 100 mL, which is 0.1 liters.
Finally, use the formula for molarity to find the resulting concentration:
Molarity = moles / volume
Concentration = 0.05 mol / 0.1 L = 0.5 M
Therefore, the resulting solution will have a concentration of 0.5 mol/L (or 0.5 M) of HNO3.