Isopropanol (molar mass = 60.1 g/mol) is present in most commercial hand sanitizers. What mass of isopropanol must be added to 10.0 mL H2O to provide a solution with a boiling point of 100.500 °C? Show your work, and provide your answer in grams
Isopropanol (molar mass = 60.1 g/mol) is present in most commercial hand sanitizers. What mass of...
When 780 g of benzene (Molar mass = 78 g/mol) reacts with 750 mL of concentrated HNO3 (16 M) and 750 mL of H2SO4 (18 M), 1000 g of nitrobenzene (molar mass = 123 g/mol) and 250 g of an unknown compound with a high boiling point are obtained. c. Give the name of the most probable side product with the high melting point. Explain why. e. Supposing the crystalline compound (250 g) has the formula C6H4N2O4, calculate the yield...
Problem: A 1.523 gram sample of KHP (molar mass=204.22 g/mol) was dissolved in 20.00 mL of distilled water. Titrating this solution to the phenolphthalein end point required 15.30 mL with the NaOH solution. The balanced titration reaction is as follows: NaOH(aq) + KHC4H8O4(aq) -> KNaCgHO(aq) + H2O(1) Calculate the molarity of the NaOH solution. Show your work.
1.A solution that contains 15.581 grams of benzene (molar mass = 78.1 g/mol) in 420 g of cyclohexane freezes at a temperature 9.50 ºC below the freezing point of pure cyclohexane. Calculate the molar freezing point depression constant, Kf, for cyclohexane. 2. The molar boiling point elevation constant for water is 0.512 ºC/m. What is the boiling point of a solution containing 673 g of water and 78.0 g of CaCl2? 3. A solution containing 32.0 g of an unknown...
The molar mass of a nonelectrolyte is 58.0 g/mol. Compute the boiling point of a solution containing 16.9 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.725 °C.
Pure benzene, C6H6, has a molar mass of 78.114 g mol-1, a density of 0.8765 g mL-1, a freezing point of 5.45°C, and a boiling point of 80.2°C. Its freezing point depression and boiling point elevation constants are: Kf = 5.07°C m-1; Kb = 2.53oC m-1. A solution was made by taking 33.88 g of an unknown nonelectrolyte and dissolving it in 175.0 g of benzene. The measured freezing point of the solution was 1.65oC. Calculate the molar mass of...
How many grams of MgCl2 (molar mass = 95.2 g/mol) should be added to 300 grams of water to give a solution that freezes at -3.00°C? Kf of H2O is 1.86°C/m.
A solution made by dissolving 85.0 g f sucrose (Molar mass. 342.3 g/mol) in 515 go acetic acid at 25 degree C froze at 14.95degreeC. Freezing point of the pure acetic acid is 16.90degreeC.Density of acetic acid is 1.05 g/ml. at 25 degree C. Answer the following and show your work in the space provided. Molality of sucrose solution = K_i of acetic acid = 93.42 g of an unknown non-volatile, non-electrolyte solute was dissolved in 850.g of acetic acid....
#16 Find the molarity of 12.5 g of NaOH in 125 ml of water (molar mass of NaOH= 40.00 g/mol) #17 A solution is prepared by dissolving 15.0g of NaCl in 85.0 g of H2O. Find mass % (m/m) 16. Find the molarity of 12.5 g of NaOH in 125 ml of water (molar mass of NaOH = 40.00 g/mol: Show your work below in order to receive credit) 17. A solution is prepared by dissolving 15.0 g of NaCl...
How many grams of nickle (II) sulfate NiSO4(molar mass of 154.8g/mol) must be dissolved in 288.0g of water to raise the boiling point by 0.350 C Kbp 0.51 Please Provide step by step solution
The molar mass of a nonelectrolyte is 58.0 g/mol. Compute the boiling point of a solution containing 22.7 g of this compound and 600.0 g of water. The barometric pressure during the experiment was such that the boiling point of pure water was 99.725 °C.