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11.Calculate the mass of sodium chloride, NaCl, required to lower the freezing temperatu re of ice...
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride...
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water by calculating the freezing point depression of solutions containing 230. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is, it absorbs...
An aqueous solution containing sodium chloride has a freezing point that is -1.28 degrees C at...
An aqueous solution containing sodium chloride has a freezing point that is -1.28 degrees C at 1.0 atm. What is the % by mass of NaCL in this solution? HINT: The Kf for water = 1.86 degrees C kg/mol
4. What is the freezing point of high fructose corn syrup? Assume a content breakdown by mass of 24% water, 68.4% fruct...
4. What is the freezing point of high fructose corn syrup? Assume a content breakdown by mass of 24% water, 68.4% fructose, and 7.6% glucose. Fructose is an isomer of glucose with a molecular formula of C6H1206. (total solution- 100 g water, Freezing-Point Depression Constants(Kf) of water -> textbook, table 11.5) TABLE 11.5 Molal Boiling-Point Elevation Constants (K,) and Freezing-Point Depression Constants (K) for Several Solvents Boiling Freezing Point Point Ke Solvent (°C) (°C . kg/mol) rc-kg/mol) rc) Water (H20)...
Freezing points are lowered as a function of the number of moles of solute particles per...
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of...
A solution of ethylene glycol in water at 20 degrees celsius has a mass percent of 9.78% of ethylene glycol with a density of 1.0108 g/mL. The freezing point depression constant for water (solvent for all solutions) is Kf=-1.86 percent celsius kg/mol and the boiling point elevation constant is Kb=0.512 degrees celsius kg/mol. The density of neat water at 20.0 degrees celsius is 0.9982 g/mL. Answer the following: 1. What is the molarity of the solution? 2. What is the...
PHARMACEUTICS CLASS Question 1: The activity of sodium ions in a 0.10 M solution is 0.079M....
PHARMACEUTICS CLASS Question 1: The activity of sodium ions in a 0.10 M solution is 0.079M. What percentage of ions in this solution is free? Write numerical answer only; round to nearest percentage. Question 2: Calculate the ionic strength of a solution that contains 0.184 M NaCl, 0.318 M CaCl2, 5% w/v dextrose (mw = 180.16 g/mol), and 0.021 M FeCl3. Report answer to three decimal places (with leading zeros as appropriate). Do not type units into answer field (assume...
Hello guys I want help to solve those question please ! Calculate the mole fraction of...
Hello guys I want help to solve those question please !
Calculate the mole fraction of phosphoric acid (H3PO4) in a
26.6% (by mass) aqueous solution.
What is the freezing point (°C) of a solution prepared by
dissolving 11.3 g of Ca(NO3)2 in 115 g of water?
The molal freezing point depression constant for water is
The concentration of CO2 in a soft drink bottled with a partial
pressure of CO2 of 4.0 atm over the liquid at 25 °C...
Above is the data source (CH,N,O) When 59.1 g of urea are dissolved in 1100. g...
Above is the data source
(CH,N,O) When 59.1 g of urea are dissolved in 1100. g of a certain mystery liquid X, the freezing point of the solution is 3.10 °C less than the freezing point of pureX of X to produce the same depression in freezing point. The van't Hoff factor Calculate the mass of potassium bromide that must be dissolved in the same mass i 1.70 for potassium bromide in X Be sure your answer has a unit...
4. What is the freezing point of high fructose corn syrup? Assume a content breakdown by mass of 24% water, 68.4% fructose, and 7.6% glucose. Fructose is an isomer of glucose with a molecular formula of C6H1206. (total solution- 100 g water, Freezing-Point Depression Constants(Kf) of water -> textbook, table 11.5) TABLE 11.5 Molal Boiling-Point Elevation Constants (K,) and Freezing-Point Depression Constants (K) for Several Solvents Boiling Freezing Point Point Ke Solvent (°C) (°C . kg/mol) rc-kg/mol) rc) Water (H20)...
Freezing points are lowered as a function of the number of moles of solute particles per kilogram of solvent. This is expressed mathematically with the following equation ATt Xkxi (mgolvending) where AT, is the amount by which the freezing point is lowered, Toute is the number of moles of solute, m ening is the mass of the solvent (in kilograms). ke is the freezing point depression constant which is specific to the solvent, and, i is the number of particles...
Hello guys I want help to solve those question please !
Calculate the mole fraction of phosphoric acid (H3PO4) in a
26.6% (by mass) aqueous solution.
What is the freezing point (°C) of a solution prepared by
dissolving 11.3 g of Ca(NO3)2 in 115 g of water?
The molal freezing point depression constant for water is
The concentration of CO2 in a soft drink bottled with a partial
pressure of CO2 of 4.0 atm over the liquid at 25 °C...
Above is the data source
(CH,N,O) When 59.1 g of urea are dissolved in 1100. g of a certain mystery liquid X, the freezing point of the solution is 3.10 °C less than the freezing point of pureX of X to produce the same depression in freezing point. The van't Hoff factor Calculate the mass of potassium bromide that must be dissolved in the same mass i 1.70 for potassium bromide in X Be sure your answer has a unit...
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