If a procedure calls for 2mL of a concentrated nitric acid, what are the mass and moles of the HNO3 actually used in the reaction?
How concentrated is the "concentrated" HNO3?
If you are talking about commercial grade conc HNO3, it has a density of about 1.4 g/mL and it is about 68% by weight HNO3. You need to confirm these values from your text or notes and use those numbers instead of these estimates.
mass soln = 1.40g/mL x 2 mL = ?
mass HNO3 = ?g mass soln x 0.68 = ? g HNO3
mols HNO3 = grams HNO3/molar mass HNO3.
To determine the mass and moles of nitric acid (HNO3) used in the reaction, we need to know the concentration of the acid. The concentration is usually given in units of moles per liter (mol/L) or molarity (M).
Please provide the concentration of the nitric acid so that I can help you calculate the mass and moles used in the reaction.
To determine the mass and moles of HNO3 used in the reaction, we need to know the concentration of the nitric acid solution. The concentration is typically given in terms of molarity (M), which represents moles of solute per liter of solution.
Assuming we are given the concentration of the nitric acid solution, we can follow these steps to calculate the mass and moles of HNO3 used:
1. Convert the volume of the solution (2 mL) to liters:
2 mL = 2 * 10^(-3) L
2. Use the concentration of the nitric acid solution to calculate the moles of HNO3:
moles = concentration * volume
For example, if the concentration is 6 M:
moles = 6 mol/L * (2 * 10^(-3) L)
3. Finally, to calculate the mass of HNO3, you need to know the molar mass of HNO3, which is:
HNO3 = 1(atomic mass of hydrogen) + 14(atomic mass of nitrogen) + 3(atomic mass of oxygen)
Using the periodic table, you can find the atomic masses and calculate the molar mass of HNO3.
Once you have the molar mass, multiply the moles of HNO3 by the molar mass to get the mass of HNO3 used.
Note: If the concentration is given as a weight/volume percentage, you would need to convert it to molarity by considering the density of the solution.