molality - number 2. The boiling point of methanol is approximately 72.0°C. What is the boiling...
What would be the freezing point of a solution that has a molality of 1.413 m which was prepared by dissolving biphenyl (C12H10) into naphthalene? Relevant information is provided below. Provide your response to three digits after the decimal. freezing point (C)K(°C/m) boiling point (C)Kb (°C/m) solvent naphthalene C10H8) 80.6 6.9 218
2. A solution was prepared by dissolving 0.817g of a substance in 100.0g of acetic acid, HC2H302. The solution then froze at 14.50 degrees Celcium. Calculate the molecular weight of the substance. The freezing point for pure acetic acid is 16.60 °C. K = 3.59 C/m.
Review Constants Periodic Table The changes in boiling point (AT) or freezing point (AT) in degrees Celsius from a pure solvent can be determined from the equations given here, respectively: Value Units moles of solute AT = mx Kb = 7 Submit kilograms of solvent XRb moles of solutex Kf Part B AT: = mx Kf = kilograms of solvent where m is the molality of the solution, and K and K the boiling-point-elevation and freezing-point-depression constants for the solvent,...
An aqueous solution of a covalent compound has a boiling point of 101.74 °C. What is the molality of the solute
An aqueous sucrose solution freezes at -0.210 degree C. Calculate the normal boiling point and the molality of an aqueous glucose solution having the same vapor pressure. Assume ideal solution behavior and kf and kb for water are 1.86 and 0.52 K-kg/mol, respectively.
The boiling point of an aqueous 1.83 m (NH4)2SO4 (molar mass = 132.15 g/mol) solution is 102.5°C. Determine the value of the van't Hoff factor for this solute if the Kb for water is 0.512°C/m. Answer's 2.7 but I have no idea how to solve for this, can someone show me how to solve with LOTS of steps? Thanks.
8. What is the final boiling point of a 1.25 molal solution of sugar in water? The Kb for water is 0.512 C/m. (For sugar i = l.) 9. A solution was prepared by dissolving 0.52 mol hexane into 400g CCl4. What is the change in freezing point of this solution? Carbon tetrachloride has a freezing point depression constant of 29.8 Cm,and freezes at-23。. 10. A solution was prepared by dissolving 0.26 moles of ethanol (C2HsOH) into 750g Diethyl ether....
1a: Approximately what will be the total solute molarity for a 0.07 M solution of NaOH? 1b: Compute the boiling point elevation of a salt water solution that contains 4.75 g of NaCl dissolved in 103 mL of water. Enter the number of degrees celsius that the boiling point will be elevated. 1c: Compute the molar mass of vitamin C if a solution containing 25.0 g in 104 g of water freezes at -2.58°C. (Assume vitamin C does not ionize...
1. What is the boiling point of a 3.0 m Ca(NO3)2 solution in water? Where: the change in boiling point (ΔTb) = mKb m is the molality of the solution Kb (the boiling point constant) for water is 0.512 2. The freezing point of ethanol (C2H5OH) is -114.6 °C. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g of glycerin a nonelectrolyte) in 200.0 g of ethanol? Where: ΔTf = mKf The molal freezing point depression...
PART 1- 8 points each) Please show all your work. 21. What is the boiling point in °C) of a solution prepared by dissolving 11.5 g of Ca(NO3)2 (formula weight -164 g/mol) in 150 g of water? (K) for water is 0.52°C/m)