What mass of water must be used to prepare a solution of 25.5 g of CaCl2 dissolved in water if the mole fraction of the CaCl2 in solution is 0.105?
What mass of water must be used to prepare a solution of 25.5 g of CaCl2...
What mass of glucose, C&H12O6, must be dissolved in 150.0 g of water so that the mole fraction of glucose is 0.125?
Find the mass of urea (CH4N2O) needed to prepare 51.3 g of a solution in water in which the mole fraction of urea is 7.53×10−2.
Find the mass of urea (CH4N2O) needed to prepare 51.3 g of a solution in water in which the mole fraction of urea is 7.66×10−2.
Naci КСІ CaCl2 °C g 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) g/mole mole kg| m g g g/mole mole kg m g/mole mole kg m -37°C -3.7°C -55 °C °C "C/ml cl "C/m 'cl "Clm
1. When 5.0 g CaCl2 is dissolved in enough water to make a 0.500 L solution, what is the molarity of ions in solution? 2. How many formula units are in 0.25 mole of Na2O? 3. How many nitrate ions are present in 0.200 mol of Zn(NO3)2?
How much water must be added to 40.0 g of CaCl2 to produce a solution that is 35.0 wt% CaCl2?
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...
A solution of CaCl2 in water forms a mixture that is 29.0 % calcium chloride by mass. If the total mass of the mixture is 263.8 g, what masses of CaCl2 and water were used?
If 10.1 g of CaCl2 is added to 200.g of water, calculate the mass percent of CaCl, in the solution. Mass percent = % CaCl2
2. 25.5 g of NHCl is dissolved in enough water to make 750.0 mL of solution What is the molarity of the solution? b. How many moles of ammonium chloride are contained in 237 mL of solution? c. What volume in mL of this solution would contain 0.059 moles of ammonium chloride?