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1. An aqueous solution is 2.65M in tartaric acid (H,C,H,0). The solution's density is 1.016 g/ml....
1a. An aqueous solution has a Molarity of 1.632 M. The density of the solution is (1.150x10^0) g/mL and the solute has a molar mass of (1.33x10^2) g/mol. What is the molality of this solution? 1b. An aqueous solution has a mass percent of solute of 18.4%. The density of the solution is (1.400x10^0) g/mL and the solute has a molar mass of (1.77x10^2) g/mol. What is the molality of this solution? 1c. An aqueous solution has a molality of...
an aqueous solution is 4.30m lithium chloride. the density of the solution is 1.127 g/mL calculate a) molarity b) mole fraction c) percent by mass
Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. (Assume 750 mL of solution.) What is the molarity of the solution? What is the molality? (At 20 ° C, the density of phosphoric acid is 1.1462 g/mL and the density of water is 0.99823 g/mL.)
We have an aqueous solution with a mass percent of
44.2 % for C2H5OH (C2H5OH is the only solute). The density of this
solution is 0.947 g/mL. Calculate the molarity, molality, and mole
fraction of C2H5OH in this aqueous solution.
We have an aqueous solution with a mass percent of 44.2% for C2H5OH (C2H5OH is the only solute). The density of this solution is 0.947 g/ml. Calculate the molarity, molality, and mole fraction of C2H5OH in this aqueous solution.
Question 10 We have an aqueous solution with a mass percent of 41.9 % for CHOH (C,H,OH is the only solute). The density of this solution is 0.958 g/mL. Calculate this aqueous solution Question 10: We have an aqueous solution with a mass percent of 41.9 % for C2H5OH (CH3OH is the only solute). The density of this solution is 0.958 g/mL. Calculate the molarity, molality, and mole fraction of CH5OH in this aqueous solution.
An aqueous NaCl solution contains 1.343x10* ppm NaCl. The density of water is 1.000g/ml. The density of the solution is 1.08 g/mL. The molar mass of NaCl is 58.44g/mol. Keep the correct number of significant figures. a) What is the molality of NaCl? b) What is the molarity of NaCl? c) What is the (mass/volume)% is unit of (kg/L)%? d) What is mass percent? e) What is mole fraction of NaCl?
3.) Quinine (C,H,N,0) (Molar Mass = 324.42 g/mol) is an anti-malaria drug. An aqueous solution was mixed containing 88.8 mg (milligrams) of quinine and 1.5 liters of H.O. (assume a total volume of 1.5 L of the solution) (Density of H,0 = 1.01 g/mL) Given this data calculate the following: (Show ALL Work) a.) Mole Fraction of Quinine in Water: (5 pts) b.) The molality of quinine: (again 1.5 L of solution / solvent) (5 pts) c.) ppm of quinine:...
A.) An aqueous solution of sulfuric acid is made by dissolving 585.0 g of sulfuric acid in enough distilled water to make a one liter solution. Calculate the molarity, the molality, the mass% and the mole fraction of sulfuric acid in this solution. The density of this solution is 1.350 g/mL. MW H2SO4 = 98.00 g/mol. Please explain!! Thank you B.) Which substance(s) is (are) miscible in water? CH3CH2OH CI4 C6H6 CH3(CH2)13CH2OH CH3OH HOCH2CH2OH
Question to We have an aqueous solution with a mass percent of 42.7% for CH OH (CH OH is the only solute). The density of this solution is 0.959 g/mL. Calculate the molarity, molality, and mole fraction of C,H,OH in this aqueous solution
The density of a 1.96 M solution of LiBr in acetonitrile (CH3CN) in 0.826 g/mL. Calculate the concentration of this solution in (a) molality, (b) mole fraction of LiBr, and (c) mass percent of CH3CN.