Calculate the number of grams of NH4C2H3O2 in ×2.00104mL of a 9.30% massvolume solution. Round your answer to 3 significant figures.

To solve this problem, we need to understand that a 9.30% mass/volume solution means that there are 9.30 grams of solute (in this case, NH4C2H3O2) in every 100 mL of solution.

Step 1: Convert the volume of the solution from mL to L: 2.00104 mL = 0.00200104 L

Step 2: Calculate the total mass of the solution using the percentage concentration. Since the concentration is given as a percentage per 100 mL, we need to find out how many "100 mL"s there are in 0.00200104 L:

0.00200104 L = 2.00104 mL = 20.0104 "100 mL"

Step 3: Multiply the number of "100 mL"s by the mass of solute per "100 mL" to find the total mass of solute:

20.0104 * 9.30 g = 186.09672 g

Step 4: Round the answer to three significant figures: 186 g

So, there are approximately 186 g of NH4C2H3O2 in 2.00104 mL of a 9.30% mass/volume solution.