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O SOO mol Al is dissolved in 1000 g of pure water at 25. The density...
3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures. 3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the...
0.6573 g of potassium iodate is dissolved and diluted to a volume of 100.0 mL. Then 25.00 mL of this stock solution is pipetted into a 100.0 mL volumetric flask which is filled to the mark with water. What is the concentration of the final standard solution in mol/L? Include units in your answer, and round the final answer to the correct number of significant figures.
579.5 g of Al(NO3)3 (molar mass = 212.996g/mol) was dissolved in 17.89 kg of water. What is the boiling point of this solution? Boiling point of pure water is 100.00 C and the boiling point constant is 0.510 C
1. A sample of hydrochloric acid (HCI), which is an acid, with a mass of 0.7302 g is dissolved in water and used to standardize a solution of barium hydroxide. An endpoint is reached when 47.81 mL of barium hydroxide has been added. Determine the molarity (in mol/L) of the barium hydroxide solution. Report your answer to four significant figures. Submit Answer Tries 0/13 2. The standardized barium hydroxide solution is then used to titrate 13.86 mL of a solution...
22.3 g of fructose, C6H12O6, are dissolved completely in 75.5 mL of pure water at 20.0 oC. Calculate the molarity and the molality of the solution. The density of pure water at 20.0 oC is 0.9982 g/cm3.
Given 15.0 g of NaCl (MM of NaCl = 58.44 g/mol) is dissolved in 100.0 g of water: a. Determine the mass percent of this solution. b. Assume the density of the solution is 1.00 g/ml, calculate the molarity of the solution.
Calculate the vapor pressure depression of a solution that 218 gram glucose (180.2 g/mol) is dissolved in 460 mL of water (18.01 g/mol). The temperature of the solution is 30°C. Assume the density of solution and water as 1.00 g/mL, the vapor pressure of pure water at 30°C 31.82 mm Hg.
5.3307 g of Na2CrO4 (MW 161.97 g/mol) is dissolved in 1000.0 mL of water. Assuming the solution has a density of 1.00 g/mL, what is the concentration of Na (MW 22.9898 g/mol) in the solution in units of a) molarity (M)? Number b) parts per thousand (ppt)? Number ppt c) 25.0 mL of the solution is then diluted to a final volume of 500.0 mL. What is the concentration of Na* in the diluted solution in units of parts per...
A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base indicator added. The solution requires 33.78 mL of 0.256 M NaOH solution to reach the end point. What is the molar mass of the acid? HA(aq) + NaOH(aq) LaTeX: \longrightarrow⟶ NaA(aq) + H2O(aq) Group of answer choices 81.4 g/mol 199 g/mol 145 g/mol 20.0 g/mol
6: Suppose 50.0 g of pure potassium hydroxide is dissolved in 250.00 mL water ( Solvent: -0.9987 g/mL). Given the density of the solution is 1.020 g/mL, what will be the molarity of the solution. (Hint: You need to find the volume of the solution)