Concentrated aqueous HCl contains 38% by mass HCl. Calculate the mass of water present in 2.50 x10^2g of this solution.
Concentrated aqueous HCl contains 38% by mass HCl. Calculate the mass of water present in 2.50...
Calculate the mass of HCl in 1.5 L concentrated solution that contains 37.11% (w/w) HCl, the density of the solution is 1.178 g/mL. Calculate the molarity (M) of HCl solution which has a molality(m) of 2.37 m and density of 1.185 g/mL. Calculate K for the following reaction at 25°C, N2 (g) + 3 H2(g) = 2 NH3(g) Kp = 5.8 x 105
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.
An aqueous solution contains 31% HCl by mass. Calculate the molality of the solution. Express your answer using two significant figures. Calculate mole fraction of the solution. Express your answer using two significant figures.
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 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 3.05 L of 0.545 M HCl by mixing with water?
#29 25.0 milliliters of an aqueous solution of hydrochloric acid, HCl (molec. wt = 36.5) contains 11.0 grams of HCl and 18.7 grams of H2O. Calculate the mass percentage of HCl in the solution. a. 63.0 b. 37.0
Commercial concentrated aqueous ammonia is 28.0% NH3 by mass. What volume of this solution contains 150. g of NH3? (Density = 0.900 g/mL) 0 595 mL O 536 mL O 150. mL O 28.0 mL O 397 mL
TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
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Calculate the percent by mass of the solute in the following aqueous solution. 2.50 g of NaBr in 88.2 g of solution Be sure to answer all parts. An old sample of concentrated sulfuric acid to be used in the laboratory is approximately 98.4 percent H2SO4 by mass. Calculate the molality and molarity of the acid solution. The density of the solution is 1.83 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.