23) 22.22 g of MgBr, are dissolved in in 1000 g of water solution. What is...
A quantity of 78.2 g of CaCl2 was dissolved per 1000. g of water. What is the freezing point in ºC?
Which of the following solutes, dissolved in 1000 g of water, would provide a solution with the lowest freezing point? 0.045 mol of barium chloride, MgCl2 0.045 mol of ammonium nitrate, NH Br 0.045 mol of acetic acid, CH3COOH 0.045 mol of urea, CO(CH3)2 0.045 mol of calcium sulfate, BaSO4
35 g of Na2CO3 is dissolved in 150 mL of water to produce a solution with a total volume of 157.2 mL. If the water is at 33∘C, what would be the freezing point of this solution (in ∘C)
if 52.5 g of LiF is dissolved in 306 g of water, what is the expected freezing point of the solution? (Assume the van’t Hoff factor, i, for LiF is 2)
steps of solving please 33. Which of the following solutes, dissolved in 1000 g of water, would provide a solution with the lowest freezing point? a. 0.030 mol of barium chloride, BaCl2 b. 0.030 mol of urea, CO(NH)2 c. 0.030 mol of calcium sulfate, CaSO4 d. 0.030 mol of ammonium nitrate, NH4NO3 e. 0.030 mol of acetic acid, CH2COOH
Determine the freezing point of a solution that contains 29.5 g of iodine dissolved in 109 mL of ethanol (d = 0.789 g/mL). Pure ethanol has a melting point of -114.0 degree C and a freezing point depression constant of -1.99 degree C/m.
A 2.00 g samples of benzoic acid (mw = 122.2 amu) is dissolved in 50.0 g of lauric acid acid, which has a normal melting point of 45.0 oC. If the new solution has a depressed freezing point of 43.7 oC, what is the freezing point depression constant for lauric acid? A.0.251 oC/m B.3.97 oC/m * C.3.25 oC/m D.0.307 oC/m E.None of the above
A solution contains 10.35 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -3.26 ∘C. The mass percent composition of the compound is 60.98% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?
The freezing point of water is 0.00°C at 1 atmosphere. If 11.84 grams of calcium bromide, (199.9 g/mol), are dissolved in 288.8 grams of water ... The molality of the solution is m. The freezing point of the solution is °C.
A 12.5855 g sample of an unknown compound (X) is dissolved in 32.0000 g of water. The resulting solution has a freezing point of – 4.3oC. What is the molar mass of X? Kf = 1.858 oC/m.