How many grams of HNO3 are required to prepare 500Ml of a 0.6601M HNO3 Solution?

Answer 1

To solve this problem, we can use the formula:

moles = concentration x volume

First, we need to calculate the number of moles of HNO3 required to prepare the solution:

moles = 0.6601 mol/L x 0.5 L = 0.33005 mol

Next, we can use the molar mass of HNO3 to convert moles to grams:

molar mass of HNO3 = 63.01 g/mol

grams = moles x molar mass = 0.33005 mol x 63.01 g/mol = 20.79 g

Therefore, 20.79 grams of HNO3 are required to prepare a 500 mL of 0.6601 M HNO3 solution.