Approved Tutor Answer1 Year agoTo determine how many grams of concentrated nitric acid solution are needed to prepare 250 mL of a 2M HNO3 solution, we can break down the problem into a few logical steps. First, we need to understand the definitions and relationships involved in molarity, mass, and concentration.
Molarity (M) is defined as the number of moles of solute per liter of solution. In this case, we want a 2M solution of HNO3, which means we need 2 moles of HNO3 in every liter of solution. Since we are preparing 250 mL (or 0.250 L), we can calculate the number of moles required:
Next, we need to find the mass of HNO3 required to obtain 0.5 moles. The molar mass of HNO3 is approximately 63.01 g/mol. Therefore, the mass can be calculated as follows:
Now that we know we need 31.505 grams of pure HNO3, we must consider that the concentrated nitric acid solution is 70% (w/w) HNO3. This means that in every 100 grams of the solution, there are 70 grams of HNO3. To find out how much of the concentrated solution we need, we can set up the following relationship:
Now, we can solve for x:
Thus, to prepare 250 mL of a 2M HNO3 solution, you would need approximately 44.29 grams of the concentrated nitric acid solution. This calculation ensures that you have the correct amount of HNO3 to achieve the desired molarity in your final solution.
Always remember to handle concentrated acids with care, using appropriate safety equipment and procedures, as they can be hazardous.
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