A certain hydrochloric acid solution has a mole fraction of 0.23 HCI. the density of this solution is 1.18g/mL
a. how many moles of HCI are in 1 mole of solution?
b. what is the weight percent of HCI in this solution?
c. what is the molarity of HCI in this solution?
d what is the molality of HCI in this solution?
e. what is the weight percent of water in this solution?
f. what is the mole fraction of water in this solution?
A certain hydrochloric acid solution has a mole fraction of 0.23 HCI. the density of this...
I. (6 pts) A certain supply of concentrated hydrochloric acid has a concentration of 40.0% HCI in water solution. The density of the solution is 1.19 g/mL. Calculate the molality and molarity of HCl in the solution. Molan Mase
Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. (Assume 750 mL of solution.) What is the molarity of the solution? What is the molality? (At 20 ° C, the density of phosphoric acid is 1.1462 g/mL and the density of water is 0.99823 g/mL.)
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 sold as a concentrated aqueous solution. If the concentration of commercial is 12M and its density is 1.18g/cm3 , calculate the following: (a) the molality of the HCl solution (b) the weight percent of HCl in the solution. Please show the work on how to arrive at these answers - a. 16.2m b. 37.1%
- 3 Calculate the molality and the mole fraction of HCI of a 10.0% (by mass) aqueous solution of hydrochloric acid.
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
A certain supply of concentrated hydrochloric acid has a concentration of 36.0% HCl in water solution. The density of the solution is 1.19 g/mL. Calculate the molarity of HCl in the solution.
Vitamin C or Ascorbic acid (C6H8O6) is a water soluble vitamin. A solution is prepared by dissolving 80.5 g of Ascorbic acid in 210 g of water. The resulting solution has a density of 1.22 g/ml. Calculate the concentration of Ascorbic acid in terms of a) Mass Percent b) Mole fraction c) Molality d) Molarity
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.
A 5.431 m formic acid (HCO2H) solution in water has a density of 1.047g/ml. Find the molarity of the solution and the percent by mass and mole fraction of formic acid.