I need to prepare 500 ml of a 37% w/w solution of sulfuric acid using 96% sulfuric acid in deionized water. I have been shown a bunch of different ways and they all give a different answer and I'm getting frustrated
.37* 500 = .96 x
where x is the amount of strong stuff you put in
500 - x is the amount of water
I don't think there is enough information to answer this question. I believe the answer posted is for a 500 GRAM solution but it won't be 500 mL. The density of a 37% H2SO4 solution is right at 1.05 g/mL so the volume will be about 476 mL. Have I missed the boat? I solved the problem privately but for question like this in the past the student has insisted on not using density. I don't know how to do it without knowing(using) density.
This problem cannot be done without density. 500ml of a solution at 37Percent w/w is Not 500grams. Now if that solution was 37 w/v, this problem of needing density goes away.
One cannot assume density is the same as water.
Thank you Bob Pursley.
Preparing a 37% w/w solution of sulfuric acid requires some calculations and understanding of the concepts of weight/weight percent and dilution. I'll guide you through the process step-by-step to ensure accuracy.
First, let's define some terms:
1. W/W (weight/weight percent): It represents the weight of the solute (sulfuric acid) divided by the total weight of the solution, expressed as a percentage.
2. Dilution: It's the process of reducing the concentration of a solute in a solution by adding more solvent (in this case, deionized water).
Now, let's calculate the amount of sulfuric acid and deionized water needed:
Step 1: Determine the desired final volume of the solution (500 ml).
Step 2: Calculate the required weight of sulfuric acid:
- Since we are using a 96% sulfuric acid solution, it means that in 100 ml of the solution, we have 96 g of sulfuric acid.
- We need 37% w/w sulfuric acid. This means that in 100 g of the 37% w/w solution, 37 g is sulfuric acid.
- To calculate the weight of sulfuric acid needed for 500 ml, we just need to set up the following proportion:
(37 g sulfuric acid / 100 g solution) = (x g sulfuric acid / 500 g solution)
Cross-multiplying, we get:
x = (37 g sulfuric acid / 100 g solution) * 500 g solution
x = 185 g sulfuric acid
Step 3: Determine the amount of deionized water needed:
- Since the weight of the solution is the sum of the weights of sulfuric acid and water, we can calculate it as follows:
(Weight of solution) = (Weight of sulfuric acid) + (Weight of water)
500 g = 185 g (sulfuric acid) + (Weight of water)
Weight of water = 500 g - 185 g
Weight of water = 315 g
Now, to summarize:
To prepare a 37% w/w solution of sulfuric acid with a total volume of 500 ml, you'll need 185 g of 96% sulfuric acid solution and 315 g of deionized water.
Please keep in mind that these calculations assume the densities of sulfuric acid and water are both 1 g/ml, and that the volume of the solution after mixing is equal to the sum of the volumes of the individual components. If your specific requirements or chemicals differ, adjustments to these calculations may be necessary.