How to make 10% nitric acid? wouldnt it be 10 mL nitric acid + 100 mL of solvent, making it 10%? What molarity is used it to make 10% nitric acid?
10% v/v is 10 mL/100 mL soln but I think 10% HNO3 means 10g HNO3/100 mL solution unless you want 10% HNO3 mass percent which is 10 g HNO3/100 g solution. To any of these, however, you must know the concn of the HNO3 you're starting with.
To make 10% nitric acid, you would need to mix a certain volume of nitric acid with a solvent. However, it is important to note that the concentration of nitric acid is typically given in terms of molarity (mol/L), not as a percentage.
If you want to make a solution of 10% nitric acid, you would need to know the molarity of the nitric acid you have on hand. The molarity represents the number of moles of solute (nitric acid) dissolved in 1 liter of solution. You can use the following equation to calculate the required volume of nitric acid:
Volume (L) = (Desired concentration (%) * Volume of solution (L)) / Molarity
Let's assume you have nitric acid with a molarity of 16 M and you want to prepare a 100 mL solution of 10% nitric acid. Plugging in the values into the equation, it becomes:
Volume (L) = (10% * 0.1 L) / 16 M
Simplifying this, you would get:
Volume (L) = 0.01 L / 16 M = 0.000625 L
So, to make a 10% nitric acid solution, you would measure 0.000625 L (or 0.625 mL) of 16 M nitric acid and add enough solvent (e.g., water) to make a total volume of 100 mL.
To make a 10% nitric acid solution, you would indeed mix 10 mL of nitric acid with 90 mL of solvent, resulting in a total volume of 100 mL. This calculation is based on the assumption that the % concentration is in terms of volume/volume (% v/v).
However, it's important to note that the 10% concentration refers to the weight/volume (% w/v) concentration in this case – specifically, 10 grams of nitric acid dissolved in 100 mL of solvent. This calculation assumes the density of nitric acid is approximately 1 g/mL.
To determine the molarity of the solution, you first need to know the molar mass of nitric acid, which is approximately 63 g/mol.
Given that you have a 10% weight/volume solution, you have 10 grams of nitric acid in 100 mL of solution. To convert this to moles, you divide by the molar mass:
10 grams / 63 g/mol = 0.1587 moles
Since you have 0.1587 moles of nitric acid in 0.1 L (100 mL) of solution, you can calculate the molarity as:
Molarity (M) = moles / volume (in liters)
Molarity = 0.1587 moles / 0.1 L = 1.587 M
Therefore, a 10% nitric acid solution (weight/volume) corresponds to approximately 1.587 M.