Which of the following solute amounts, when dissolved in 1.00 kg of water, would produce a solution with a freezing point of -1.86 oC?
Group of answer choices
2.00 moles of sugar
0.50 moles of KBr
2.00 moles of NaI
1.00 mole of NaCl
Which of the following solute amounts, when dissolved in 1.00 kg of water, would produce a...
What is the freezing point for a solution containing 1.00 mole of NaCl (an ionic component) dissolved in 1.00 kg of water? Group of answer choices +3.72 oC -3.72 oC -1.86 oC +1.86 oC
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...
4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solu- tion decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why. 5. Calculate the freezing point of a 0.2 m CaCl, aqueous solution, assuming it dissociates completely to form ions in solution.
17) Methanol, CH3OH, is sometimes used as an antifreeze for the water in automobile windshield washer fluids. How many moles of methanol must be added to 6.50 kg of water to lower its freezing point to -13.0 ∘C? For each mole of solute, the freezing point of 1 kg of water is lowered 1.86 ∘C. 18.) The following table gives the solubility of solute X in water at two different temperatures: You have prepared a saturated solution of X at...
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...
Which of the following compounds when dissolved in water, would form an aqueous solution that would not conduct an electric current? Group of answer choices KOCl LiOH NaCl C12H22O11
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...
12. Molarity, M, is defined as A. moles of solute dissolved in 1 mol of solvent. B. moles of solute dissolved in 1 kg of solvent. C. moles of solute dissolved in 1 L of solvent. D. moles of solute dissolved in 1 L of solution. E. moles of solute dissolved in the solution. 13. What volume of 2.50 M NaOH (40.00 g/mol) contains 0.100 mole of NaOH? A. 0.250 L D. 0.250 mL B. 40.0 mL E. 0.0400 mL...
A 93.728 grams sample of compound ionized into one cation and three anions when dissolved in 125.214 grams of water. The freezing point of the resulting solution was found to be -6.26 °C. The freezing point constant of water is 1.86 °C /m. (a) Calculate the concentration of dissolved solutes, in molality. (b) Calculate the molar mass of the solute, in grams/mole.
Which solid, when dissolved in water, would cause the solution to have the greatest change in boiling point?" A. CaCl2 B. Sugar C. Na3PO4 D. NaCl