calculates the density (g / ml) and the molality of an aqueous solution of HF at 48.0% by mass whose concentration is 27.60M
HF at 48.0% by mass means 48.0 g HF remain in 100 g solution.
mass of solvent = (100 - 48) = 52.0 g = 0.052 kg.
48.0 g HF = mass / molar mass = 48.0 g / 20.01 g/mole = 2.399 mole.
thus
molality = 2.399 mole / 0.052 kg = 46.13 m
concentration is 27.60 M means 27.60 mole HF remain in 1000 ml solution.
27.60 mole HF = mole * molar mass = 27.60 mole * 20.01 g / mole = 552.276 g
thus
density = mass / volume = 552.276 g / 1000 ml = 0.552 g / ml
calculates the density (g / ml) and the molality of an aqueous solution of HF at...
What is the molality of a 0.735 M aqueous ZnCl2 solution with a density of 1.102 g solution/mL solution. Assume the density of pure water is 1.00 g/mL. The molar mass of ZnCl2 is 136.29 g/mol.
An aqueous solution is 0.500% by mass ammonia, NH3, and has a density of 0.996 g/mL. The molality of ammonia in the solution is m.
1a. An aqueous solution has a Molarity of 1.632 M. The density of the solution is (1.150x10^0) g/mL and the solute has a molar mass of (1.33x10^2) g/mol. What is the molality of this solution? 1b. An aqueous solution has a mass percent of solute of 18.4%. The density of the solution is (1.400x10^0) g/mL and the solute has a molar mass of (1.77x10^2) g/mol. What is the molality of this solution? 1c. An aqueous solution has a molality of...
An aqueous solution is 0.467 M in HCl. What is the molality of the solution if the density is 1.23 g/mL? Show work please. Answers are a) 0.374 m b) 0.115 m c) 0.268 m d) 0.574 m
An aqueous solution is 0.447 M in HCl. What is the molality of the solution if the density is 1.23 g/mL? An aqueous solution is 0.447 M in HCl. What is the molality of the solution if the density is 1.23 g/mL? 0.275 m 0.318 m 0.115 m 0.363 m 0.550 m
A 2.78 L aqueous solution of KOH contains 183 g of KOH. The solution has a density of 1.29 g/mL. Calculate the molarity (M), molality (m), and mass percent concentration of the solution. molarity: 1.175 M molality: m mass percent:
An aqueous NaCl solution contains 1.343x10* ppm NaCl. The density of water is 1.000g/ml. The density of the solution is 1.08 g/mL. The molar mass of NaCl is 58.44g/mol. Keep the correct number of significant figures. a) What is the molality of NaCl? b) What is the molarity of NaCl? c) What is the (mass/volume)% is unit of (kg/L)%? d) What is mass percent? e) What is mole fraction of NaCl?
What is the molality of a 50% by mass aqueous solution of glucose (molar mass = 180 g/mol) Assume the density of water = 1.00 g/mL 0.00554 m 1.00 m 5.56 m 2.34 m
Calculate the molality of a 11.4% by mass aqueous solution of iron (II) nitrate with a density, ρ = 1.099 g/mL. Report your answer to THREE significant figures.
1. An aqueous solution is 2.65M in tartaric acid (H,C,H,0). The solution's density is 1.016 g/ml. Calculate the solution's: (a) molality (b) mole fraction of tartaric acid (c) percent by mass