Enter your answer in the provided box. The solubility of CO, in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility at a partial pressure in air of 0.00035 atm? Assume that CO, obeys Henry's law. mol /L

The freezing point of 59.49 g of a pure solvent is measured to be 44.96 ºC. When 2.18 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 42.65 ºC. If the freezing point depression constant of the pure solvent is 7.66 ºC·kg solvent/mol solute calculate the molar mass of the solute. ?=g/mol

Calculate the solubility of carbon dioxide in water at an atmospheric pressure of 0.480 atm (a typical value at high altitude). Atmospheric Gas Mole Fraction kH mol/(L*atm) N2 7.81 x 10-1 6.70 x 10-4 O2 2.10 x 10-1 1.30 x 10-3 Ar 9.34 x 10-3 1.40 x 10-3 CO2 3.33 х 10-4 3.50 x 10-2 CH4 2.00 x 10-6 1.40 x 10-3 H2 5.00 x 10-7 7.80 x 10-4 M

178. Subject  :- Chemistry

The solubility in acetone of organic compound O is measured and found to be 0.762 that would contain 38.0 g of O at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits. 0 x10 0.0 X μ 010 at 25. °C. Calculate the volume of a saturated solution of O in acetone mL

g at 10. °C. Calculate the volume of a saturated solution of X in water that mL The solubility in water of ionic compound X is measured and found to be 0.339 would contain 360. mg of X at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits.

Help with the following question round the answer to 2 sig figs

Which of the following phenomena is best described by Henry’s Law?a. Increasing temperature favors an endothermic process.b. The solubility of NaCl(s) in water increases with increasing temperature.c. The solubility of MgCl2(s) in water is unaffected by pressure.d. The vapor pressure of an aqueous solution of glucose, C6H12O6, is lower than the vapor pressure of pure water.e. The solubility of O2(g) in water increases with increasing pressure.

A solution is prepared by adding 425g of AgNO3 to 0.150L of water at 40.0∘C. The solubility of AgNO3 at 40.0∘C is 311g100.mL. How many grams of AgNO3 are expected to precipitate if the temperature is dropped to 0.00∘C where the solubility of AgNO3 is only 122g100.mL? Give the answer with three significant figures.

The molar mass of an enzyme was measured by dissolving the 3.221 grams of the enzyme in 1.00 liter of water. The osmotic pressure of the solution was 5.746 cm of solution at 20°C (assume the density of the solution is 1.00 g/mL and the density of mercury is 13.56 g/mL). What is the molar mass of the enzyme?