We’re being asked to calculate the volume of concentrated HCl needed to prepare a 2.90 L of 0.505 M HCl.
Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters).
In other words:
We’re given the mass percent of concentrated HCl which is 37.0%.
Recall that mass percent is given by:
This means in 100 g of solution, we have 37 g HCl.
The steps we need to do for this solution are:
Step 1: Calculate the moles of HCl
Step 2: Calculate the volume of the solution (in L).
Step 3: Calculate the molarity of the solution.
Step 4: Calculate the volume of solution needed (in L) using dilution equation.
Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL.
How much concentrated solution would you take to prepare 2.90 L of 0.505 M HCl by mixing with water?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Calculate Molarity concept. You can view video lessons to learn Calculate Molarity. Or if you need more Calculate Molarity practice, you can also practice Calculate Molarity practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Maxwell's class at UCF.