A sample of an ionic solid is dissolved in 1.00 kg of water. The freezing point of the water is -0.01 °C. If three times the mass of ionic solid is dissolved in 1.00 kg of water and the resulting freezing point of the solution is -0.09 °C, which of the following would be possible formulas for the solid: MX, MX2, or MX3, where M represents a metal cation and X an anion with a 1- charge? Explain your reasoning.

Assume that all solutions were prepared at 25 degrees celcius and the solutes are conpletely dissolved. The solution is acetic acid solution. 23. 2 mL of glacial acetic acid (CH3COOH) dissolved in water to form a 50.0 mL solution. What is the molarity?

Calculate the mass percent of a solution that is prepared by adding 75.0 g of N 2 OH to 485 g of H 2 O

17.1 g of a nonelectrolyte was dissolved in 33 g of a solvent.  The pure freezing point of the solvent was 2.5 C and the Kf value was 3.21 C/m.  The freezing point after the nonelectrolyte was dissolved was -4.55 C.  What is the molar mass of the nonelectrolyte? Round your answer to the ones position.

Choose the answer that shows the following solutions in order by their decreasing freezing points from the highest freezing point to lowest freezing point: 0.1 m Na,PO, 0.1 m C,H,OH, 0.01 m CO,, 0.15 m NaCl, and 0.2 m CaCl,. 0.01 mol CaCl,>0.1 mol C,H,OH>0.15 mol Na,PO,>0.1 mol NaCI>0.2 mol CO, 0.01 mol CaCl, >0.1 mol C,H,OH>0.I5 mol NaCl>0.1 mol Na,PO,>0.2 molCO, B © 0.1 mol Na, PO,>0.2 mol CaCl, >0. 15 mol NaCI>0.1 mol CH,OH>0.01 mol CO, D 0.01 mol CO,>0.I mol C,H,OH>0.15 mol NaCl>0.1 mol Na, PO,>0.2 mol CaCl,

An aqueous solution of isopropanol (MM = 60.10 g/mol) has a molality of 7.91 m and a density of 1.18 g/mL. What is the molarity of isopropanol in the solution?

A solution is prepared by dissolving 11.622 g sulfuric acid, H2SO4, (Molar Mass = 98.07848 ) in enough water to make 100.0 mL of solution. If the density of the solution is 1.115 g/mL, what is the molality? Report your answer using three decimal places.

A student dissolves 14. g of sucrose (C,,H,,0,1) in 450. mL of a solvent with a density of 0.85 g/mL. The student notices that the volume of the solvent 22 does not change when the sucrose dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity = | x10 molality %3D Continue Submit O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center MacBook Air 20 888 DD F3 F4 F5 F6 F7 F8 34 00

An aqueous CaCl2 solution has a vapor pressure of 81.6 mmHg at 50 degrees celsius. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent?

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