What is the freezing point of a solution that contains the following quantity of solute in 1.00 kg of water?
4.2 mol of KI:
What is the freezing point of a solution that contains the following quantity of solute in...
What is the freezing point of a solution that contains the following quantity of solute in 1.00 kg of water? 5.3 mol of KI:
attempts left Check my work Enter your answer in the provided box. What is the freezing point of a solution that contains each of the following quantities of solute in 1.00 kg of water? 4.4 mol of Na3PO4
molecular weight moles of solute kg owater insolution molality of solution change in freezing point Naci KCI CaCl, Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) 9 9 9 g/mole g/ mole mole mole kal kg m m -31°C 3 °C...
What is the freezing point of a solution of ethyl alcohol, that contains 31.3 g of the solute (C2H5OH), dissolved in 800 g of water?
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
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,...
A solution is made by dissolving 0.745 mol of nonelectrolyte solute in 853 g of benzene. Calculate the freezing point and boiling point of the solution. The normal freezing point of benzene is 5.49 °C and the normal boiling point of benzene is 80.1 °C. Assuming 100% dissociation, calculate the freezing point and boiling point of 0.570 mol of AgNO3 in 1.00 kg of water.
Molar Mass Determination by Freezing Point Depression Calculate and enter the freezing point depression of a solution of 57.6 g ethylene glycol (C2H602) in 734 g H20. Kffor H20 is 1.86 °C kg/mol. °C -2.53 1 homework pts Submit Answer Incorrect. Tries 3/5 Previous Tries A solution which contains 71.9 g of an unknown molecular compound in 363 g of water freezes at -3.85°C. What is the molar mass of the unknown? g/mol 1homework pts Submit Answer Tries 0/5 Molar...
Part B. Initial Freezing Point of Water Mass of water Mass of Solute Molecular Weight of solute moles of solute kg of water in solution molality of solution Final Freezing Point of solution Change in Freezing Point kr from part A i for the solute(theoretical) i for the solute(experimental) NaCl 0°C 10.0 g 0.58 9 g/mole mole kg KCI oºch 10.0 g 0.75 g g/mole mole kg CaCl2 0°C 10.09 1.11 g g/mole mole kg m -5.6°C °c C/m -3.7°C...
A 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: AT) = m x K = moles of solute XK K. kilograms of solvent Since pure water boils at 100.00 °C, and since the addition of solute increases boiling point, the boiling point of an aqueous solution, Th, will be T - (100.00+AT) 'C Since pure water freezes at...