A student dissolves 20. g of urea not change when the urea dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity = 0 0 ((NH,),CO) CO in 175. mL of a solvent with a density of 0.81 g/mL. The student notices that the volume of the solvent does molality= ola X 0x0 S

Determine the percent by mass of MgCl2 if 3.1 g of MgCl2 is dissolved in 41.1 g of water.

At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute can dissolve in 125.5 g of water at the same temperature?

Calculating molality.

A solution containing 25.0 g of protein per liter has an osmotic pressure of 8.3 mmHg at 37°C. What is the molar mass of the protein? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a b с d e 5.8 X 104 g mol-1 7.3 X 104 g mol-1 9.3X 104 g mol-1 1.2 X 105 g mol-1 3.2 X 105 g mol-1

The solubility of heptanol, CH3(CH₂)6OH, is 0.16 g per 0.10 L. What is the molarity of the solution? 0.073 0.013 0.0073 0.133 0.16

An aqueous solution of ethanol (molar mass = 46.07 g/mol) has a molality of 12.15 m and a density of 1.100 g/mL. What is the molarity of ethanol in the solution?

Use the solubility curve below to answer the following questions: 150 140 130 120 110 100 NANO3 90 80 70 60 NH&Cl KCI NaCi 50 40 30 20 KCIO3 10 Ce2(SOals O 10 20 30 40 50 60 70 80 90 100 Temperature (c) Q1) As the temperature increases, the solubility of the NH3 in water Q2) The solute, NH3, is MOST likely a (increases/decreases/stays the same). (solid, liquid, or gas). Q3) How many grams of NH4CI are dissolved in 500 g of water at 90 °C? Q4) If you had 50 grams of NH4CI in 100 g of water at 40 °C, would the solution be saturated, unsaturated, or supersaturated? Q5) You heat a solution of KCIO3 to 80°C and saturate the solution. You then allow the solution to cool down to 50°C. How many grams of solute would precipitate out of the solution? NH3 per 100 g H,0 Grams of solute ONO CON

Determine the freezing point (in °C) of a solution that contains 204 g of C6H1206 dissolved in 234 mL of acetic acid (density = 1.05 g/mL). Pure acetic acid has a freezing point of 16.6°C and a K = 3.90°C/m.

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 |