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I'm having trouble figuring out the last three:
Ions exhibiting significant Brønsted acid characteristics
Ions exhibiting significant Brønsted base characteristics
Ions exhibiting no significant Brønsted acid or base characteristics
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- Determine how ideal the following solutions are by calculating the mole fraction of solute in each solution, and comparing that to the expected mole fractions. All data are for 25.0C. a14.09 weight percent of I2 in C6H6, MP of I2 is 112.9C sublimes, and fusH=15.27kJ/mol b2.72 weight percent of I2 in C6H12, MP of I2 is 112.9C sublimes, and fusH=15.27kJ/mol c20.57 weight percent of para-dichlorobenzene, C6H4Cl2, in hexane, MP of C6H4Cl2 is 52.7C and fusH=17.15kJ/mola Convert the calculated mole fraction of naphthalene dissolved in toluene from Example 7.10 into molarity, assuming that the volumes are strictly additive. The density of toluene is 0.866g/mL and density of naphthalene is 1.025g/mL. b Estimate the solubility, in g/100mL and molarity, of naphthalene in n-decane, C10H22, which has a density of 0.730g/mL.The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
- A batch of 500 ?? of ??? dissolves in water to form a saturated solution at 350 ? (77 °?) where the solubility is 30% by weight of ??? in water. The solution cools at 293 ? (20 °?) at which the solubility is 25.4% by weight. Determine the number of crystals obtained if 3.5% of the original water evaporates on cooling. Also, determine the capacity of the container in which this solution is cooled if it is 1.20 times the volume of the solution. The density of the solution is ???? ??/??Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: 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 2.02A solution of common salt in water is prepared by adding 50kg of salt to 200kg of water tomake a liquid density of 1250kg/m3. Calculate the concentration of salt in this solution as a: i) Weight(w/w)fraction (Ans: weight fraction 20%)
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- according to wikipedia what is the solubility of benzoic acid in water at 25 degrees and 100 degrees? if you were given 1.55 grams of benzoic acid how much boiling water would you need to dissolve it all (show all work)? If you were to cool the solution to 25 degrees afterwards, would the solution be saturated? justifyA solution contains 3.86g of magnesium chloride and 250g of water. Compute for thefreezing point depression of the solution. (K, water: 1.86 °C/m)A. 0.16 ACB. 0.25 PCC. -0.25 PCD. -0.90 °0 Assume that a 1-L solution contains 35g of potassium chloride (MM: 74.6 g/mol).Compute for the osmotic pressure ifthe solution is at 298 K. (R=0.08206 L-atm/mol-K)A. 22.95 atmB. 24.50 atmC. 11.47 atmD. -11.47 atm Suppose that a 1 m sugar-water solution raises the boiling point of water by 0.51 °C.How much will the boiling point of water increase if the sugar-water solution amounts to 3 m?A. 0.51 °CB. 1.02 °CC. 1 53 POD. 101.53 °Cby watching this two video - https://www.youtube.com/watch?v=9FBpdaokLto - https://www.youtube.com/watch?v=1Twy1IQg-6c In general, what is the effect of temperature on the solubility of solid in liquid?