0
What is the freezing point of a solution that contains 0.550 moles of Nal in 615 g of water?
Wiki User
∙ 9y ago
3.33 degrees Celsius is the freezing point of a solution that contains 0.550 moles of Nal in 615 g of water.
Wiki User
∙ 9y ago
Add your answer:
Earn +20 pts
What is the freezing point of a solution that contains 2.0 mol of CaCl2 in 800.0 g of water Kf for water equals 1.86Cm?
2.0 mol of CaCl2 releases 2.0 mol of Ca+2 ions & 4.0 mol of Cl- ions = 6 moles of ions find molality: 6 moles / 0.800 kg water = 7.5 molal solution dT = kf (molality) dT = 1.86 C (7.5m) dT = 14 Celsius drop in freezing temp the new freezing point is - 14 C
Which would lower the freezing point more 100 moles of sugar or 100 moles of NaCl?
100 moles of NaCl
The freezing point of a solution containing 4.12 g of unknown solute in 100 grams of camphor is 166.2 degrees C what is the freezing point depression?
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
What is the freezing point of an aqueous solution if the boiling point of an aqueous solution is 101.34 degree Celsius?
nobody knows
What is the solution's freezing point depression?
To solve freezing point depression problems, you need to know the following things:-- the identity of the solute (the thing you are adding to the liquid)-- the identity of the solvent (the liquid)-- whether the solute is molecular or ionic, and if ionic, how many ions it forms-- the amount of solute (in grams or moles)-- the amount of solvent (in kilograms)-- the value of Kf of the solvent (for water, it is -1.858 K·kg/mol (or -1.858 °C molal-1)Then you use the following equation:∆T = i * Kf * mwhere ∆T is the change in the freezing point, "i" is the number of molecules or ions formed upon addition to the solvent, Kf is the freezing point depression constant, and "m" is the molality of the solution.The Kf of water for a freezing point depression is known and is equal to -1.858 °C·kg/mol (or -1.858 °C molal-1)The value of "i" has to do with what you add to the water. If you added sugar, a molecular compound the value of "i" is 1.0. If you add a ionic compound like NaCl, the value of "i" is 2.0 because for every 1 molecule of NaCl, you make 2 ions: one Na+ and one Cl- in water. For MgCl2, the value of "i" is thus 3.0 (for each MgCl2 you get one Mg2+ and two Cl- ions, so a total of 3 ions).To find "m," the molality of a solution you need to know the number of moles of solute and the number of kilograms of solvent (m = moles/kg). If you are given the number of grams of solute, the number of moles is found from the mass and the molar mass of the solute.grams of solute ÷ molar mass of solute = moles of soluteTo find the molality, just divide the moles of solute by the kilograms of solvent moles of solute ÷ kilograms solvent = molality Note: If you are given the volume of the solvent instead of the mass, use the density of the solvent to convert -- the density of water is 1 kilogram per liter)Liters of solvent * density of solvent = kilograms of solventNow just plug all the numbers into the equation at the top of the answer!
What is the freezing point of a solution that contains 0.550 moles of NaI in 615 g of water?
The freezing point of a solution that contains 0.550 moles of NaI in 615 g of water is -3.33 degrees Celsius.
What is the freezing point of potassium hydroxide?
48% KOH freezing pt -11deg C 45% KOH freezing point -28 deg C The change in freezing point (always a decrease) = (number of ions in solution per molecule) x (Kf - the freezing point constant of the solvent) x (m - the molality of the solution, i. e. moles solute per kg solvent) For KOH in water, Freezing pt = 0 - 2(1.86)(molality of solution)
Which solution containing 1 mole of solute dissolved in 1000 grams of water has the lowest freezing point- KOH C2H5OHC6H12O6C12H22O11?
The lowest freezing point is observed for 1 mole of KOH, because its one moles produce 2 moles of ions in solution, 1 mole of cation K+ and 1 mole of anion OH-.
How does the number of moles affect the freezing point?
Higher the concentration of the solute, lower is the freezing point.
What is the freezing point of a solution that contains 2.0 mol of CaCl2 in 800.0 g of water Kf for water equals 1.86Cm?
2.0 mol of CaCl2 releases 2.0 mol of Ca+2 ions & 4.0 mol of Cl- ions = 6 moles of ions find molality: 6 moles / 0.800 kg water = 7.5 molal solution dT = kf (molality) dT = 1.86 C (7.5m) dT = 14 Celsius drop in freezing temp the new freezing point is - 14 C
The solution has a freezing point of -2.79 . The freezing point depression constant for water is 1.86 K m-1. What is the nitrate concentration in the solution?
The solution has a freezing point of 2.79 and this is the frezzing point of mercury
When a solute is added to solvent the freezing point of the solution is?
The freezing point is lowered.
Which would lower the freezing point more 100 moles of sugar or 100 moles of NaCl?
100 moles of NaCl
What colligative property is responsible for antifreeze?
Freezing point depression. When a solution is formed the molecules of the solute prevent the solution from freezing at its normal freezing point, it must be colder.
How do you solve freezing depression?
You need to know the solute and the solvent and whether the solute is molecular or ionic and how many ions it contains. The formula is the change in freezing point equals the number of ions times the freezing point depression constant times the molality of the solution.
The freezing point of a solution containing 4.12 g of unknown solute in 100 grams of camphor is 166.2 degrees C what is the freezing point depression?
f.p depression = (freezing point of pure solvent)-(freezing point of solution) -------> 178.4-166.2=12.2
Does alcohol have a freezing point?
it does have a freezing point it just contains a chemical that makes it hard to freeze
