Briefly explain why the sparingly soluble product mustbe removed by filtration before you back-titrate the excesssilver ion in the Volhard determination of a) chloride ion.
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Briefly explain why the sparingly soluble product mustbe removed by filtration before you back-titrate the excesssilver ion in the Volhard determination of
a) chloride ion.
b) cyanide ion.
c) carbonate ion.
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Solved in 2 steps
- Gravimetric Analysis. Please include complete solution, thank you. In the gravimetric determination of sulfate in a 0.2841 g sample of pure Na2SO4, a BaSO4 precipitate weighing 0.4604 g was obtained. The weight of the precipitate was smaller than the theoretical one, since some BaSO4 was converted to BaS during the heating process. Calculate the percent of BaS in the precipitate and percent error of the analysis.A 0.7980-g sample of chloride was titrated using the Fajans method and required 45.32 mL of 0.1046 M AgNO3. Calculate for % Cl (MM=35.45).Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of these
- 3. The colorless solution of an unknown solid turned blue litmus red and emitted an odor of ammonia upon addition of NaOH. A pale yellow precipitate was observed upon reaction with AgNO, and a white precip- itate was observed the unknown from the list of possibilities in the Introduction to this experiment. upon addition of Pb(NO.),. Bubbles were not evident upon addition of HCl. Identify escribed. In this notati Anode Cathode ByBy ing of the anode comparment arewritten on left and the componens of the cathode comparment wnen on the right The componenn of the two half-cells are separated by a salt bridg represented by he ahle verical line. The single verticallines represent the phase boundary berween the solid clecrode and the lons olution This notion will beused to describe theactions you will study in this experiment aA pue) uopa Bpuodsaoo ad uopeppo ou half reactions, one epresent the processes occuring a the anode and cathode ina voltaic cell as sepa(a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NAOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c ) In analyzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to obtain greater accuracy by using a pH meter instead of using a color-change indicator such as phenolphthalein?What other factors do you need to consider when assessing feasibility of titration?
- I would like to prepare standards by conducting a serial dilution of 2mg/ml BSA down to 0.0625mg/ml BSA. How many standard solutions will I have? What are the concentrations of these standard solutions?Why is a lower concentration of NaOH or HCl used for titration while a solution with higher concentration is used for adjusting the pH of the remaining medium? [Answer in not more than 3 sentences]4. Carbonate System. An amount of NaHCO; was added to water such that the total carbonate concentration was 104 M. If it is assumed that no other constituents are present, a pC-pH diagram for this water-carbonate system is shown below. (a) What is the statement of mass balance for total dissolved carbonate in the system? (b) What is the charge balance for dissolved species in the system? (c) What is the proton condition for this system if NaHCO; was added to water?