21. What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the...

Question

Question

science chemistry

Answer 1

Similar Homework Help Questions

The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved...

The freezing point depression constant of water is -1.86 C/m. If 7.50 g NaCl is dissolved in 45.0 g H, O, the freezing point is changed by -9.71 *C. Calculate the van't Hoff factor for Naci. Select one: O a. 1,00 . OOOO c. 1.83
Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...

Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute. Experimental Results Mass of solvent (water) Freezing point of water Freezing point depression constant (Kf) of water Mass of solution Freezing point of solution 8.515 g 0.00°C 1.86°C/m 9.3589 -5.45°C a. What mass of solute was used? b. What is the...
13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by...

13. A 0.230 m solution of an unknown electrolyte depresses the freezing point of water by 0.821°C. What is the Van't Hoff factor for this electrolyte? The freezing point depression constant for water is 1.86 °C/m. a. 0.521 b. 1.92 c. 2.00 d. 2.30 e. 4.41

When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the...

When 0.60 grams of a non-electrolyte unknown compound is dissolved in 10 grams of water, the freezing point of the solution is -1.86o C. Given that the freezing point of pure water is 0o C and that the freezing-point depression constant for water is 1.86 o C/mol/kg, calculate the molecular mass (g/mol) of the unknown compound.
I asked this question before but I didn't really understand what was the answers for EACH...

I asked this question before but I didn't really understand what was the answers for EACH of the blanks listed in my question, so I am asking it again. A 1.24 M solution of KI has a density of 1.15 g/cm3. Assume 1.00 liter of 1.24 M KI solution. The mass of 1.00 L of solution is ______grams. The number of grams of KI in the 1 liter is _____ grams. The number of grams of water in the 1...
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of aluminum nitrate...

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of aluminum nitrate (213.0 g/mol), must be dissolved in 279.0 grams of water to raise the boiling point by 0.450°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02

When 81.4 g of alanine C3H7NO2 are dissolved in 650.g of a certain mystery liquid X,...

When 81.4 g of alanine C3H7NO2 are dissolved in 650.g of a certain mystery liquid X, the freezing point of the solution is 8.90°C less than the freezing point of pure X. Calculate the mass of sodium chloride that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor =i1.56 for sodium chloride in X.
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of zinc chloride...

The boiling point of water is 100.0°C at 1 atmosphere. How many grams of zinc chloride (136.3 g/mol), must be dissolved in 209.0 grams of water to raise the boiling point by 0.400°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g zinc chloride.
מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water...

מו Calculate the mass of glucose (C6H606) that must be added to 100 g of water to give a solution whose freezing point is -3.8°C. The freezing point depression constant of water is 1.86 °C/m. The molar mass of glucose is 180.16 g/mol Give your answer in grams to 3 significant figures

What mass of water is required to give an aqueous solution containing 0.265 mol of MgCl2...

What mass of water is required to give an aqueous solution containing 0.265 mol of MgCl2 with a freezing point of -3.8°C? (Van't Hoff factor of MgCl2 is 2.7). Kf of water 1.86 C/m A) 1.25 kg B) 0.538 kg C) 0.113 kg D) 0.882 kg E) 0.350 kg