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- A hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?Write the relevant chemical reaction and mass-balance expression for 0.1 M NaCl.. A student prepares a solution by dissolving 1.000 mol ofNa2SO4 in water. She accidentally leaves the containeruncovered and comes back the next week to find only awhite, solid residue. The mass of the residue is 322.2 g.Determine the chemical formula of this residue.
- Create the flowchart of qualititative analysis of Cations in Group 2 and explain.What is the pH of rainwater at 25°C in which atmospheric CO2 has dissolved, producing an initial [H2CO3] of 1.28×10-5 M ? Take into account the autoionization of water.What is the equilibrium constant value for NaC2H3O2 and how do you find its Kb?
- Write the balance equation of aqueous Pb(ClO3)2 with NaI. Include phases.After titration, weight percent of oxalate in K3[Fe(C2O4)3] (MW: 437.2 g/mol) sample was determined to be 55.8%. What is the percent error of oxalate content determination?During the titration of an HClO4solution with 0.10320M NaOH, a CHEM 3A student,Juan becamedistracted and overshot the endpoint. A fellow student Pedrosuggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000mL, the volume of NaOH added was 28.060mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH andcalculate the molar concentration of the original HClO4solution.
- A solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)An alkaline sample of sodium compounds weighing 1.196 g was dissolved in water, cooled to 15°C, treated with 2 drops of Pp indicator and titrated with 1.058 N H2SO4 requiring 6.8 ml to render the solution colorless. Upon adding 2 drops of MO and continuing the titration, 16.5 ml more of the acid were needed to complete the analysis. What is the quantitative composition of the sample? MW: NaOH = 40.0, Na2CO3 = 106.0, NaHCO3 = 84.01What weight of sample in gram containing 8.00 % Fe3O4 (MW= 231.53 g/mole) must be taken to obtain a precipitate of Fe (OH)3 (MW= 106.867 g/mol) that, when ignited to Fe2O3 (MW = 159.69 g/mole), weighs 150.0 mg