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- A certain gaseous solute dissolves in water, evolving 12.0 kJ of heat. Its solubility at 25C and 4.00 atm is 0.0200 M. Would you expect the solubility to be greater or less than 0.0200 M at (a) 5C and 6 atm? (b) 50C and 2 atm? (b) 20C and 4 atm? (b) 25C and 1 atm?A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?6) A solution made by dissolving 173.0 g of an unknown compound in 650.0 mL benzene to make a solution which has a freezing point 26.6 °C lower than that of pure benzene. Kr=5.12 °C/m and d of benzene = 0.877 g/ml ку a. points) What was the molality of the solution? (173.09) (1000) (1000) = 0.173ky b.) If the molality of the solution is 5.67 m. How many moles of the unknown compound were dissolved in the solution? C. ) If the solution contains 4.67moles of the unknown. What is the molar mass of the unknown compound?
- If 110.1 mL of water is shaken with oxygen gas at 2.5 atm, it will dissolve 0.0041 g O2. Estimate the Henry's law constant for the oxygen gas in water in units of g mL-1atm1 kH = g mL 1atm-1 i eTextbook and Media GO Tutorial Save for Later Attempts: 0 of 15 used Submit Answer MacBook Air DII 888 F4 F5 F3 & 23 $(p... m 2 2 S College Search | Common... 3 2 Pretest: Unit 1 Question 10 of 30 What is the predicted change in the boiling point of water when 4.00 g of barium chloride (BaCl₂) is dissolved in 2.00 kg of water? Kb of water = 0.51°C/mol molar mass BaCl2 = 208.23 g/mol ivalue of BaCl₂ = 3 O A. -0.0049°C OB. -1.0°C OC. 0.0016°C OD. 0.015°C ← PREVIOUS b Write build | bartleby $ 4 C do 5 % < C 6 A Apex Learning & 7 * 8 SUBMIT ( 9 A Apex Learning - Courses 0(Q68) What mass (in grams) of ethylene glycol (C2H6O2) must be added to 1,296 grams of water to lower the freezing point to -1.10 °C? (3 sf)
- Chemistry I Laboratory Manual, 2021 Revision Questions: 0176(! 1) Calculate the theoretical percent water in the following hydrates. (a) nickel(II) sulfate heptahydrate 10 7H2O NiSO4 Th% 7(18.02) 154.75 X100% (=) (b) aluminum chloride hexahydrate NH4C1 6H20 NiSO4 = 154.159.000 10 Th=81.51% ofame stanbyde of boros 2) If iron(II) sulfate is heated too strongly, the following reaction will occur FeSO4(s)→ FeO(s) + SO3(g) If you are heating a sample of FeSO4 6H2O and this reaction occurs along with dehydration, what will happen to the experimental percent water? Explain your answer. Instag 3) A 8.416 g sample of CaCl2 xH₂O after heating gives an anhydrous residue of 5.624 What is the value of x? mass H₂O= 8.416g-5.624g = 2.792g4. (5 pts) When 0.258 g of a molecular compound, benzoic acid, was dissolved in 40.0 g of benzene, the freezing point of the solution was lowered to 5.23 °C. What is the molecular weight of the benzoic acid? Freezing point of pure benzene = 5.46 °Celsius Kf of benzene = 5.12 °C/molalChemistry Using the vale of 300 mOsmol.L-1 for plasma answer the following questions: A 2.0 L solution contains 18 mmol of sodium chloride (i = 1.8) 20 mmol of potassium chloride (i = 1.8) 10 mmol of calcium chloride (i = 2.5) a) Is the solution isotonic, hypotonic or hypertonic? b) If it is not isotonic, how could the solution be made isotonic with blood using either glucose or water? If using water to make the solution isotonic give the volume to be added in mL If using glucose to make the solution isotonic give the amount to be added in mmol. Please use water to make the solution isotonic
- Calculate the vapor pressure of water over a solution made by dissolving 225.0 g of glucose (C6H12O6) in 575 g water at 35°C. (At 35°C 42.2mmHg) P⁰ water ▸ Files ▬ a r D F7 I F8 FQ prt sc F10 home Bun F11 end F12 insert deleteThe partial pressure of the nitrogen is 0.7644 atm in water at 298K. What is the concentration of N2? Henry's Law Constant for N₂ = 6.1 x 10-4 mol/L.atm [N₂] = [? ] × 10¹?] mol Exponent (yellow) || Coefficient (green) Enter- 3 At 25.0 °C the Henry's Law constant for methane (CH,) gas in water is 1.4 x 10 °M/atm. Calculate the mass in grams of CH, gas that can be dissolved in 725. mL of water at 25.0 °C and a CH, partial pressure of 3.66 atm. 4 Be sure your answer has the correct number of significant digits.
