Final answer:
To calculate the mass of solute in a 0.2500L of 0.1135 M K2CrO4 solution, one should find the number of moles of K2CrO4 and then multiply by its molar mass. The calculation results in a mass of approximately 5.51 g of K2CrO4 solute.
Step-by-step explanation:
The question asks for the mass of solute in a given volume and molarity of a solution, specifically for potassium chromate (K2CrO4). To find this, we need to:
- Calculate the number of moles of K2CrO4 using the molarity and volume of the solution.
- Determine the molar mass of K2CrO4.
- Multiply the moles of K2CrO4 by its molar mass to get the mass of the solute.
Here's the calculation:
Moles of K2CrO4 = 0.2500 L × 0.1135 mol/L = 0.028375 mol
Now, the molar mass of K2CrO4 is approximately 194.19 g/mol. So:
Mass of K2CrO4 = 0.028375 mol × 194.19 g/mol = 5.51 g