(1) A solution containing 8mmol Fe" is titrated by a standard solution of ceric sulfate Ce(SO4)2, the final volume is 500 ml. What weight of ferrous ions remains unoxidized at the equilibrium point.
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- 0.2219 g of pure iron wire was dissolved in acid nd iron reduced to+2 state. Then the solution required 34 65ml of cerium(4) in a titration . Calculate molar concentration of ce4+???A 0.3749 g soda ash sample is analyzed by titrating sodium carbonate with the standard 0.2388M HCl solution, requiring 49.38ml. The reaction is: CO32- + 2H+ → H2O +CO2Calculate the percent sodium carbonate in the sample.The chloride ion content of a 250.0-mL seawater sample was titrated against 0.1102 M silver nitrate, requiring 13.56 mL to reach end point. How many moles of chloride ion is present in the sample?
- You are presented with a white solid and told that due tocareless labeling it is not clear if the substance is bariumchloride, lead chloride, or zinc chloride. When you transferthe solid to a beaker and add water, the solid dissolves to givea clear solution. Next a Na2SO4(aq) solution is added anda white precipitate forms. What is the identity of the unknownwhite solid?100.0 mL of 0.60 M aqueous Pb(NO3)2 is mixed with excess aqueous KI. What mass of precipitate is formed?25 mL of a bleach (NaOCl) sample is diluted to 500 mL. An excessive amount of KI is added to the 20 mL solution taken from here, and the released I2 is titrated with 35.5 mL of 0.0409 M NaS2O3. Accordingly, calculate the weight percent by volume of NaOCl in the sample.(MaNaOC:74,4 g/mol)
- If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?The level of dissolved oxygen in a water sample can be determined by the Winkler method. In a typical analysis, a 100.0-mL sample is made basic, and treated with a solution of MnSO4, resulting in the formation of MnO2. An excess of KI is added, and the solution is acidified, resulting in the formation of Mn2+ and I2. The liberated I2 is titrated with a solution of 0.00870 M Na2S2O3, requiring 8.90 mL to reach the starch indicator end point. Calculate the concentration of dissolved oxygen as parts per million of O2.The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the sulfur in the sample to SO2 and bubbling this SO2 through a solution of H2O2 which converts it to H2SO4. The acid is titrated with a standard solution of NaOH (0.1251 M) until the end point with bromothymol blue, which changes color when both protons of the acid sulfuric have been neutralized. Calculate the purity of the preparation in % by weight given that a sample of 0.5136 g required 50.00 mL of the NaOH solution
