🤓 Based on our data, we think this question is relevant for Professor Randles' class at UCF.
Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.
A) 13.9 M
B) 12.8 M
C) 10.7 M
D) 9.35 M
E) 7.79 M
We’re being asked to calculate the molarity (M) of hydrochloric acid (HCl) in a solution. Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:
We first need to determine the number of moles of HCl. We’re given the mass percent of HCl in water, 39.0%. Recall that mass percent is given by: