Express the 1% Sodium Lauryl Sulfate (NaC 12 H 25 SO 4; ρ=1.01 g/ml) solution in the following concentrations. 1. mg % 2. Mole percent of solute 3. Molarity Please show complete solution. Tnx

Concentration is the amount of solute dissolved in a certain amount of solution: Solution concentrations are usually given as one of the following: ● Mass percent (m/m)-the mass of the solute in grams for exactly 100 g of solution • Volume percent (v/v)-the volume of solute in exactly 100 mL of solution • Mass/volume percent (m/v)-the mass of solute in grams for exactly 100 mL of solution ● Molarity (M)-the number of moles of solute in exactly 1 L of solution Part A Calculate the mass percent (m/m) of a solution prepared by dissolving 43.37 g of NaCl in 171.3 g of H₂O. Express your answer to four significant figures. ► View Available Hint(s) Mass percent (m/m) = concentration of a solution = _amount of solute amount of solution Submit Π| ΑΣΦ ? % P Pearson Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us |

A solution is made by dissolving 0.900g of compound Y into 11.000g of cyclohexane. The solution freezes at 3.9 oC. What is the molar mass of compound Y in g/mol?   The Freezing Point of Cyclohexane is 6.6oC. and the freezing point depression constant is kf = 20.0 oC/m. (m=molality). Group of answer choices 0.091 g/mol 606.06 g/mol 303.03 g/mol 1212.12 g/mol

How many grams of KCl will be undissolved when 50g of KCl is dissolved in 100g of water at 20.0oC?

If 100 mL of a 0.15 M Mg(NO3)2(aq) solution has a density of 1.09 g/mL, which of the following statements is false? The mass of the water in this solution is 109 g The mass of Mg(NO3)2 in this solution can be determined from this information. If the solution density was not given, it is usually reasonable to assume 1.00 g/mL It is possible to determine the mole fraction of water in this solution.

Match the following aqueous solutions with the appropriate letter from the column on the right

The freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 48.78 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute). Be sure to use the appropriate number of sig figs What is the molality of the solution?  How many moles of solute are present?   What is the molecular weight of the solute?

A student dissolves 6.7 g of biphenyl (C12H10) in 425. mL of a solvent with a density of 1.05 g/mL. The student notices that the volume of the solvent does not change when the biphenyl dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity Ox10 olo Ar molality 미

A solution of 4.55 % phenol (C6H6O) solution by mass in carbon tetrachloride, CCl4.  The density of the solution is 1.602g/mL.  What are the molality, mole fraction, and molarity of phenol in the solution?   a. Fill in the summary table as you determine different parts of the problem – the first few columns are labeled – it is up to you to decide what is important information:   Molar mass mole         Solute             Solvent             Solution               b. Molality:   c. Mole Fraction:     d. Molarity:

A solution contains 1.75 g of a non–volatile, non–electrolyte solute dissolved in 23.47g stearic acid.  The freezing point of the solution is 67.2⁰C.  The freezing point of pure stearic acid is 69.3⁰C and its freezing point constant, Kfp, is 4.5⁰C kg/mol.  What is the molar mass of the solute