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- 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?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?How many grams of the following nonelectrolytes would have to be mixed with 100.0 g of p-dichlorobenzene to increase the boiling point by 3.0C? To decrease the freezing point by 2.0C? (Use Table 10.2.) (a) succinic acid (C4H6O4) (b) caffeine (C8H10N4O2)
- Which solute has the greatest effect on the boiling pointof 1.00 kg of water: 50.0 g of strontium chloride (SrCl2) or 150.0 g of carbon tetrachloride (CCl4) ? Justify youranswer.The Rast method uses camphor (C10H16O) as a solvent for determining the molar mass of a compound. When 2.50 g of cortisone acetate are dissolved in 50.00 g of camphor (k f =40.0C/m), the freezing point of the mixture is 173.44C; that of pure camphor is 178.40C. What is the molar mass of cortisone acetate?Part II. Determination of molecular weight for ethyl alcohol Freezing point, °C DTf Mass of solute, g mass of solvent, kg Calculated molecular weight, g/mol -2.30 0C ΔTf = T0f – Tf 0.0 °C -(-2.30 °C) = 2.30 0C 6.202 g 0.1kg Click or tap here to enter text.
- Boiling Point Elevation/Freezing Point DepressionT = m KWhere: T = T(solution) - T(pure solvent) * m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb (°C / m) Kf (°C / m) Water H2O 0.512 -1.86 Ethanol CH3CH2OH 1.22 -1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 -5.12 Diethyl ether CH3CH2OCH2CH3 2.02 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number.In regards to freezing point depression: The original experiment calls for 3 grams lauric acid and .4 g benzoic acid to be melted and then observed to crystalize to demonstrate freezing point depression. A student misreads the directions and adds 4.0 g of benzoic acid instead of 0.4 g. What do you expect to happen? Would the experiment still be valid? Explain your reasoning. I think that since the amount of lauric acid (3g) doesnt change that the solution may be too oversaturated with benzoic acid. I'm not sure if this would still demonstrate freezing point depression since it is a colligative property based on amount of solute....Test Tube Solute Mass of Deionized Water (g) Mass of solute (g) Freezing Point (C) 1 None 4.140g X 0.0 2 NaCl 4.021g 0.235g -3.8 3 Unknown A 4.000g 0.233g -.17 4 Unknown B 4.036g 0.231g -0.6 a. Determine the motlilty of each solution. Sample Calculation for Test Tube 2: Sample Calculation for Test Tube 3: b. Calculate the molar mass of the solute in each solution. Sample Calculation for Test Tube 2: Sample Calculation for Test Tube 3:
- An automobile anti freeze mixture is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL; M=62.07 g/mol)and water (d=1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as:(a) Volume percent(b) Mass percent(c) Molarity(d) Molality(e) Mole fractionGiven - Boiling point elevation A solution of: SOLVENT: Water (H2O) - 100mL or 100.00g SOLUTE: Salt (NaCl) - 11.60g What is the computed boiling point (in degrees Celsius) of the SOLUTION prepared in the experiment? Note: Answers must be numeric, not alphanumeric—42, not forty-two.Please indicate true (T) or false (F) as appropriate: Justify I) The vapor pressure of a solvent is reduced by the presence of a non-volatile solute II) In an ideal solution, the vapor pressure is increased by the presence of a solute Volatile. III) Sea water freezes at a lower temperature than sugar water. IV) In the laboratory, chemists use this effect to judge the purity of a component solid: if impurities are present, the freezing point of the compound is lower than the accepted value. A) TFTF B) TTFT C) FTFF D) TTTT