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What are the mole fraction and molality of ethanol -C2H5OH in an aqueous solution that is 45.0 percent ethanol by volume-The density of water is 1.00g per mL and that of ethanol is 0.789 grams per mL?
TaylorHigh
The mole fraction and molality of ethanol -C2H5OH in an aqueous solution that is 45.0 percent ethanol by volume and the density of water is 1.00g per mL that of ethanol is 0.789 grams per mL and 70/18. A mole fraction in chemistry is the amount that is divided by the total amount of all constituents.
Wiki User
∙ 10y ago
First, calculate the volume percentages of ethanol and water in the solution. Since we know the density of both solvents, convert the percentages to mass (using density and volume). Then calculate the mole fraction of ethanol by dividing the moles of ethanol by the total moles of all components in the solution. Finally, calculate molality using the moles of solute (ethanol) and the mass of the solvent (water).
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Calculate the mole fraction of HCl in 20 percent aqueous solution?
The mole fraction of HCl in a 20% aqueous solution can be calculated by converting the percentage to a molarity concentration. Assuming the density of the solution is 1 g/mL, a 20% solution means 20g of HCl in 100g of solution. If the molar mass of HCl is 36.5 g/mol, we can calculate the molarity and then use it to find the mole fraction of HCl in the solution.
Water is a solvent in a(n) what solution?
'An Aqueous' solution. NB The word 'aqueous' comes from Latin ; 'aqua' meaning 'water'.
What is the term for a solution made in water?
The term for a solution made in water is an aqueous solution.
What solutions in which water is the solvent are called?
Solutions in which water is the solvent are called aqueous solutions.
What concentration of aqueous CaCl2 solution freezes at -10.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC m?
To calculate the molality of the solution, we first need to determine the change in freezing point. ΔTf = 0.0°C - (-10.2°C) = 10.2°C. Next, use the formula ΔTf = Kf * m to find molality. Rearrange the formula to solve for molality: m = ΔTf / Kf = 10.2°C / 1.86°C m^-1 = 5.48 m. Thus, the concentration of the solution is 5.48 mol/kg.
What are the molality and mole fraction of solute in a 25.5 percent by mass aqueous solution of formic acid (HCOOH)?
The molality is 5,54.
Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid.Group of answer choices4.33 m3.05 m0.274 m2.74 m?
2.74m
What is the boiling point of an aqueous solution that has a vapor pressure of 18.5 at 25 degrees Celsius?
The boiling point of an aqueous solution can be calculated using the formula: ΔT = iKbm, where ΔT is the boiling point elevation, i is the van't Hoff factor, Kb is the ebullioscopic constant, and m is the molality of the solution. Given the vapor pressure of 18.5 mmHg, you can determine the molality of the solution and then calculate the boiling point elevation.
Calculate the mole fraction of HCl in 20 percent aqueous solution?
The mole fraction of HCl in a 20% aqueous solution can be calculated by converting the percentage to a molarity concentration. Assuming the density of the solution is 1 g/mL, a 20% solution means 20g of HCl in 100g of solution. If the molar mass of HCl is 36.5 g/mol, we can calculate the molarity and then use it to find the mole fraction of HCl in the solution.
Water is a solvent in a(n) what solution?
'An Aqueous' solution. NB The word 'aqueous' comes from Latin ; 'aqua' meaning 'water'.
Is the boiling point of a 0.5 m aqueous solution of KOH higher than the boiling point of a .5m aqueous solution of KCL?
Yes, the boiling point of a 0.5 m aqueous solution of KOH would be higher than the boiling point of a 0.5 m aqueous solution of KCl. This is because KOH is a strong electrolyte that dissociates into more ions in solution compared to KCl, leading to a greater increase in boiling point due to the colligative properties of the solution.
What is the term for a solution made in water?
The term for a solution made in water is an aqueous solution.
What concentration of aqueous CaCl2 solution freezes at -10.2ºC The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºC m?
To calculate the molality of the solution, we first need to determine the change in freezing point. ΔTf = 0.0°C - (-10.2°C) = 10.2°C. Next, use the formula ΔTf = Kf * m to find molality. Rearrange the formula to solve for molality: m = ΔTf / Kf = 10.2°C / 1.86°C m^-1 = 5.48 m. Thus, the concentration of the solution is 5.48 mol/kg.
What solutions in which water is the solvent are called?
Solutions in which water is the solvent are called aqueous solutions.
Is a aqueous solution a solution that contains all the solute that it can hold?
the solution itself, yes. it must contain water to be called an aqueous solution. the term aqueous designates water as the solvent/diluent.
How do you use the word aqueous in a sentence?
an aqueous solution is a solution made of water.
How is an aqueous solution different from other solutions?
In an aqueous solution the solvent is water.
