A 22.9 % (by mass) solution of ferrocene (FW = 186.04 g/mol) dissolved in hexane (FW = 86.18 g/mol) has a density of 1.421 g/mL. What is the mole fraction (Χ) of ferrocene? Ferrocene is a non-electrolyte.
A 22.9 % (by mass) solution of ferrocene (FW = 186.04 g/mol) dissolved in hexane (FW...
0.4556 g of Na2CO3 (FW = 105.99 g/mol) was dissolved in water and titrated with a solution H2SO4 of unknown Normality. 20.35 mL of H2SO4 solution was required to reach the final endpoint. What is the Normality of the H2SO4 solution? (Answer in 4 sig figs)
a. Calculate the mass of iodine, I2, that must be dissolved in 725 mL of carbon disulfide, CS2(d= 1.261 g/mL) to produce a 0.236 msolution. b. Calculate the molality of a solution consisting of 34.0 mL of benzene (C6H6, 78.11 g/mol, d= 0.877 g/mL) in 187 mL of hexane (C6H14, 86.18 g/mol, d= 0.660 g/mL).
10.00 grams of KH2PO4 (FW = 136.086 g/mol) are dissolved in 500 mL of deionized H2O. How many grams Na2HPO4 (FW = 141.96 g/mol) need to be dissolved to create a solution with a pH of 6.90? For H3PO4, pKa1 = 2.15 , pKa2 = 7.20, and pKa3 = 12.37.
5. What mass of bacta (FW: 192.095 g/mol), a nonelectrolyte, must be dissolved in 5000.0 g of ambori to give a solution with a freezing point of -1.50°C? What is that solution's boiling point? The normal boiling point of ambori is 84°C. The K of ambori is 39.7°C/m and the Ko of ambori is 2.34°C/m. (10 points)
A solution of NaCl (MW = 58.5 g/mol) in water (MW = 18.0 g/mol) has the molality of 3.01 molal and the density of 1.112 g/mL. Consider mass of solvent 1 Kg A) What is the mass percent of the solute? (B) What is the molarity of the solution? (C)What is the mole fraction of H2O?
Answer all please What is the mole fraction of I_2 in a solution made by dissolving 55.6 g of I_2 in 245 g of hexane, C_6H_14? (MM I_2 = 253.81 g/mol and MM Hexane = 86.18 g/mol) A) 0.0715 B)0.0770 C) 0.133 D) 0.154 What is the mole fraction of oxygen in a gas mixture that is 3.7g in oxygen (MM O_2 = 32.0 g/mol) and 6.3g in nitrogen (MM N_2 = 28.0 g/mol) by mass? A) 0.34 B) 0.37...
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...
A solution contains 10.35 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -3.26 ∘C. The mass percent composition of the compound is 60.98% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?
You have a solution which is 43.9% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. What is the molality of the isopropyl alcohol in the solution? What is the molarity of the isopropyl alcohol in the solution? What is the mole fraction of the isopropyl alcohol in the solution? What intermolecular forces are shared between isopropyl alcohol and water?
29 You have a solution which is 43.4% by mass isopropyl alcohol (MM = 60.11 g/mol) in water. The density of this solution is 0.905 g/mL. a What is the molality of the isopropyl alcohol in the solution? > 1 point b What is the molarity of the isopropyl alcohol in the solution? > 1 point с What is the mole fraction of the isopropyl alcohol in the solution? > 1 point