what is the molarity of concentrated hydrogen fluoride if the solution is 48% by mass and has a density of 1.17 gram per milliliter.
To find the molarity of a solution, you need to know the concentration of the solute in terms of moles per liter (mol/L). In this case, the solute is concentrated hydrogen fluoride (HF).
First, let's determine the mass of the solution. We know that the solution is 48% by mass, so if we assume we have 100 grams of the solution, 48 grams of it is HF.
Next, let's calculate the volume of the solution. We are given that the density of the solution is 1.17 grams per milliliter. Since the density is in grams per milliliter, and we have 48 grams of HF, we can divide the mass by the density to find the volume:
Volume = mass / density
Volume = 48 g / (1.17 g/mL)
Now, let's convert the volume from milliliters to liters by dividing by 1000:
Volume = (48 g / 1.17 g/mL) / 1000
Volume = 0.0410 L
Now we have the volume of the solution in liters, and we know the mass of HF in grams. To calculate the molarity, we need to convert the mass of HF to moles. The molar mass of HF is 20.01 g/mol.
Moles of HF = mass of HF / molar mass of HF
Moles of HF = 48 g / 20.01 g/mol
Now, we can calculate the molarity by dividing the moles of HF by the volume of the solution in liters:
Molarity = moles of HF / volume of solution
Molarity = (48 g / 20.01 g/mol) / 0.0410 L
Now we can evaluate the expression:
Molarity ≈ 59.11 mol/L
Therefore, the molarity of the concentrated hydrogen fluoride solution is approximately 59.11 mol/L.