The mass percentage of hydrochloric acid within a solution is 22.00%. Given that the density of this solution is 1.110 g/mL, find the molarity of the solution.
consider 100 grams of solution
now
we know that
% mass = mass of solute x 100 / mass of solution
so
22 = mass of HCl x 100 / 100
mass of HCl = 22
now
we know that
moles = mass / molar mass
so
moles of HCl = 22 / 36.46
moles of HCl = 0.6034
now
volume = mass / density
given
density of solution = 1.11 g / ml
so
volume of solution = 100 / 1.11
volume of solution = 90.09 ml
now
molarity = moles of HCl x 1000 / volume of solution (ml)
so
molarity = 0.6034 x 1000 / 90.09
molarity = 6.7
so
the molarity of the solution is 6.7 M
The mass percentage of hydrochloric acid within a solution is 22.00%. Given that the density of...
An aqueous solution is 36.0° by mass hydrochloric acid, HCl, and has a density of 1.18 g ml. The molarity of hydrochloric acid in the solution is M Subrnit Answer Try Another Version 1 item attempt remaining
what is the molarity of a hydrochloric acid solution that is 21.2% HCI by mass and has a density of 2.19 g/ML
20.2 percent by mass hydrochloric acid with a density of 1.096 g/ml, calculate the molarity of the HCl solution
40. What is the molality of a 30.0% by mass hydrochloric acid solution? The density of the solution is 1.1493 g/mL. a. 0.300 m b. 9.46 m 11.8 m 0.0345 m e. 9.30 m work?
A solution is made by adding 42.0 mL of concentrated hydrochloric acid (37.3 wt%, density 1.19 g/mL) to some water in a volumetric flask, and then adding water to the mark to make exactly 250 mL of solution. Calculate the concentration of this solution in molarity
Part A How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/ml) are required to produce 16.0 L of a solution that has a pH of 2.197
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.22?
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 36 mL of the concentrated HCI, adding it to water, and diluting to 0.500 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density. Answer:
Hydrochloric acid is usually purchases in concentrated form with a 37.4% concentration by mass and a density of 1.19 g/mL. What is the molarity of concentrated HCI(aq)?
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 67 mL of the concentrated HCl, adding it to water, and diluting to 0.800 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density.