The normal freezing point of a certain liquid X is -2.6°C, but when 59. g of urea ((NH2)2CO) are dissolved in 550. g of X, it is found at the solution freezes at -6. Zero instead uses information to calculate the molal freezing point depression of Kf of X and round your answer to 2 sig figs

An experiment was conducted to determine the effect of glucose on the freezing point of water. Experimental data showed thatthe freezing point depression of water in solution was –2.6°C when 1.0 g of glucose was dissolved in 10g of solvent. Calculatethe expected freezing point for such solution and compare the expected freezing point to the value found experimentally. Give aplausible explanation for any discrepancies. (M.W. of glucose= 180.16g/mol; i=1). Show all your work.

Given the following mixture of two compounds 45.00 mL of X (MW =80.00 g/mol)(density 0.893 g/mL) and 885.00 mL of Y (55.00 g/mol))(density 1.280 g/mL). The freezing point of pure Y is 54.00 degrees C. The molal freezing constant is 4.757 degrees C/m. What is the freezing point of the solution.

With correct sig figs

When 127. mg of a certain molecular compound X are dissolved in 55.0 g of dibenzyl ether point of the solution is measured to be 1.6 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. ((C6H₂CH₂)₂0), 2 the freezing OO B olo Xu

If dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.

Help with the following question

A sports drink formulation can be prepared by mixing the ingredients in the quantities shown in the table below. Calculate the freezing point of this drink formulation. (Kffor water is 1.86 °C kg mol-1 and the molar mass of sucrose is 342.3 g mol-¹). Ingredient Mass (g) NaCl 1.2 0.49 KCI Sucrose (C12H22011) 60 1000 water O a. -0.38 °C O b.-0.43 °C O c. -0.10 °C O d. -0.32 °C O e. -0.75 °C Which ONE of the following saturated aqueous salt solutions will contain the highest total concentration of ions at 25°C? a. AgCl = 1.8 x 10-10) (Ksp (Ksp = 3.9 × 10-11) O b. CaF2 OC. Ag2CO3 O d. COCO3 (Ksp (Ksp = 1.0 x = 8.1 x 10-12) 10-10) The highest amount of solid Cul2 will dissolve in 1.0 L of an aqueous solution of: a. 0.5 M CaCl2 b. 0.5 M Cu(NO3)2 O c.0.5 M Cul2 O d. 0.5 M NH4I O e. 0.5 M CuCl2

When 52.3 g of alanine (C;H,NO,) point of pure X. On the other hand, when 52.3 g of iron(III) nitrate (Fe(NO;),) are dissolved in 600. g of a certain mystery liquid X, the freezing point of the solution is 3.3 °C lower than the freezing are dissolved in the same mass of X, the freezing point of the solution is 4.3 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i =

When 4.59 g of a certain molecular compound X are dissolved in 35. g of dibenzyl ether ((C%H,CH,),°). the freezing point of the solution is measured to be 0.9 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 1 significant digit. 0 00 0.0 X x10