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- By the use of Henderson Hasselbalch equation; pH = pKa + log{[acetate ion]/[acetic acid]} 4.5 = 4.75 + log{[0.10 M]/[acetic acid]} -0.25 = log{[0.10 M]/[acetic acid]} [Acetic acid] = 0.10 M/ 10-0.25 [Acetic acid] = 0.10 M/0.56 [Acetic acid] = 0.1786 M Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L = 0.025 mol Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow; w100% = 0.025 mol × 82.0343 g/mol = 2.051 g Weight (w) of sodium acetate (purity 99%) is calculate as follow; w99% = 2.051 g× (100/99) = 2.072 g What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.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 mLFor an aqueous solution saturated in both AgCl and AgI, at 1 bar and at 298 K. The equilibrium constants for this system are given as follow: Ksp(AgCl) = 1.8*10^-10, Ksp(AgI) = 8.5*10^-17, and Kw = 1.0*10^-14. How many formalities must be given to get unique values for all the concentrations?
- Chloroform (1)/methyl ethyl ketone (2) form a solution in vapor liquid equilibrium at 330 K. The chloroform concentration in the liquid phase is x1 = 0.55. Assuming an ideal gas and an ideal solutionof liquids, what are y1 and P (in kPa), to 3 significant figures?Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.A 1.00-m solution of acetic acid, CH3COOH, in benzene has a freezing point of 2.96°C. Use the data in the Table to calculate the value of i and suggest an explanation for the unusual result. (Hint: If i is less than 1.0, each formula unit that dissolves yields less than one solute particle, an outcome suggesting aggregation of solute particles.) Answer is: i = 0.50; formation of dimers of composition (CH3COOH)2, need steps shown to understand though
- Consider an aqueous solution saturated in both AgCl and AgI, at 1 bar and at 298 K. The equilibrium constants for this system are Ksp(AgCl) = 1.8*10-10E-10, Ksp(AgI) = 8.5*10E-17 and Kw = 1.0*10E-14. Find the concentration of all the ionic species. If you need to specify any formalities, make them 1 M.Hexanoic acid was added to an immiscible biphasic solvent system, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D2) of hexanoic acid in water with respect to CCl4.What is the value of the equilibrium constant when ΔGorxn = 25 kJ·mol-1 and T=298 K?
- You have a calorimeter with a heat capacity of 0.426 kJ/ºC. You combine 50.0 mL 1.50 M NaA (A- = conjugate base of weak acid HA) with an equal volume of HCl of higher molarilty. The temperature changes from 18.6 ºC to 21.1 ºC. What is ΔHºdissoc for the dissociation reaction of HA, in kJ?Calculate the solubility at 25°C of PbCO3 in pure water and in a 0.0110M PbNO32 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0110 M Pb(NO3)2solution: gLIn the synthesis of hydrocarbons, the carbon source is carbon dioxide. Although the CO2 concentra?on in the atmosphere raises at a drama?c speed, point sources are probably the easier sources for a PtX process. Iden?fy 3 possible point sources, explain why CO2 is formed and what challenges each of the three CO2 streams presents