Determine the solubility of CO2 in soda water at 25°C if the pressure of CO2 is 5.6 atm. The Henry's law constant for carbon dioxide in water at this temperature is 3.4 x 102 M/atm. O 0.53 M O 0.16 M O 0.78 M O 0.61 M O 0.19 M

3. a. A solution contains 1.75 g of a non-volatile, non-clectrolyte solute dissolved in 23.47g stearic acid. The freezing point of the solution is 67.2°C. The freezing point of pure stearic acid is 69.3°C and its freezing point constant, Kp, is 4.5°C kg/mol. What is the molar mass of the solute? b. When a liquid is in a narrow tube, the surface of the liquid, the meniscus, may be either concave, A, or convex, B What does the shape of the meniscus tell you about the intermolecular forces of attraction between the liquid and the tube?

How to prepare these solutions? 250.0 mL 0.125 M stock Na2S2O3 solution from Na2S2O3·5H2O crystals 250 mL 0.10 M NaOHNOTE: Use the 1.0 M NaOH prepared250.0 mL standard 2500 ppm Cu(II) stock solutiona. Weigh and dissolve appropriate amount of Cu(NO3)2·5H2O crystals in enough distilled water.

Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?

If the concentration of sodium carbonate in water is 12.8 ppm, what is the molarity of Na2CO3(aq)? The molar mass of Na2CO3 is 106.0 g/mol. Assume the density of the solution is 1.00 g/mL.     28 × 10–6 M 21 × 10–4 M 36 × 10–3 M 136 M 121 M

Which of the following aqueous solituions will have the highest freezing point  0.2 m AgNO3 0.3 m CaCl2  0.1 m LiCl  0.4 m CH4O

Which temperature would allow the highest solubility of CO2 in water? 40C 50C 60C 70C

Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water.  imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in the solution are written in the second column of the table. Use the checkboxes to classify each compound. 

Which solution will have the highest freezing point?

Choose