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- An acid solution containing 2 per cent by mass of NaNO3, and an unknown concentration of HNO3 is used to regenerate a strong acid resin. After sufficient acid had been passed over the resin for equilibrium to attained, analysis showed that 10 per cent of resin sites were occupied by sodium ions. What was the concentration of HNO3 in the solution, if its density were 1,030 kg/cu.m.?Is a Kd value of 10.16 reasonable for the extraction of benzoic Acid between methylene chloride and water? Please explain.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.
- Why is it necessary to use a buret for measuring standard AgNO3 solution in Volhard?Can someone help write a balanced equation showing products of the dissolution of In(ClO3)3. Including states of matter use the lowest possible whole number coefficients. At 250C, Ksp for AgBr is 5.0 x 10-13. Calculate the solubility of AgBr in g/L at 25 oC (a) in pure water; (b) In the presence of 0.2 mol L−1 NaBr solution
- Traces of aniline can be determined by reaction with an excess of electrolytically generated Br2: C6H5NH2 + 3Br2 =====è C6H2Br3NH2 + 3H+ + 3Br- The polarity of the working electrode is then reversed, and the excess bromine is determined by a coulometric titration involving the generation of Cu(I): Br2 + 2Cu+ ===è 2Br- + 2Cu2+ Suitbale quantities of KBr and copper (II) sulfate were added to a 25.0 ml sample containing aniline (C6H5NH2). Calculate the mass in micrograms of C6H5NH2 in the sample from the accompanying data. Working electrode Functioning as Generation Time (min) with a constant current of 1.00 mA Anode 3.76 cathode 0.2702 table spoon solution with 10% w/v were diluted to 1 quart with water, what be ratio strength (w/v) the dilution? explain easyCalculate ΔrH° (in kJ mol−1), ΔrS° (in J K−1 mol−1), ΔrG° (in kJ mol−1) at 298.15 K for the reaction below. C(gr.) + 12 N2(g) + 52 H2(g) ⟶ CH3NH2(g) ΔfH ° at 298.15 K / kJ mol−1 0 0 0 −22.97 S¯ ∘at 298.15 K / J K−1 mol−1 5.74 191.61 130.68 243.4 Give your answers in the specified units. Please double check your solution.
- A 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44V a. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00 and 90.00 mL of Cerium (IV). b. Draw a titration curve for these data. c. Generate a first- and second-derivative curve for these data. Does the volume at which the second-derivative curve crosses zero correspond to the theoretical equivalence point? Why or why not?The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.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.