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- A sample containing BaCl, 2H,0, KCI and inert material weighed 0.8417 g. After heating the sample at 160°C for 45 min, it weighed 0.8076 g. The sample was then dissolved in water and treated with a slight excess of AgNo,. The resulting precipitate was collected and found to weigh 0.5847 g. Calculate the % Bacl,-2H,0 and % KCI in the sample. 3.For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 4. Why is it necessary to carry out the reduction of iron and then the titration, before going on to the next sample 5. If you look carefully, there are pieces of tin metal on the bottom of the SnCl2 reagent solution. Why is it there?What is meant by non-stoichiometric defect? Ionic solids which have anionicvacancies due to metal excess defect develop colour. Explain with the helpof suitable example.
- For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 3. How would you prepare a complete anlaysis procedure using KMnO4 as the oxidant instead of K2CrO7? Include sample and solution preparation, approximate weights of samples and reagents, procedure and chemical reactions. In particular what is the purpose of the Zimmerman Reinhardt Reagent?For Redox Analysis of Iron... ~0.02 M of potassium dichromate is prepared as titrant for dried unknown. ~.3 g of sample, 50ml of 6M HCl, 20mL SnCl2, 10 mL of saturated HgCl2 solution, 60 mL of 3M H2SO4, 15mL of concentrated H3PO4, 100mL DI water. HCl (+ heat in fumehood until samples dissolves), SnCl2 (added with pipet until solution changes from yellow to colorless/light green with 3 drops in excess), HgCl2 (after cooling), H2SO4, H3PO4, DI Water, is added to the sample solution with 8 drops of diphenylamine sulfonate indicator then titrated with the potassium dichromate to a violet blue endpoint. 1. What is the purpose of the phosphoric acid in this experiment? Please be specific. 2. How does the Diphenylamine sulfonate indicator work? What chemical reaction causes the color change? How is an indicator chosen in a redox reaction?Please explain and define „supersaturation" supersaturation". What is the influence of this parameter on the and „relative precipitation process in gravimetric analysis and how can you influence this parameter during analysis?
- When a 100.0-mL portion of a solution containing 0.500 g of AgNO3 is mixed with 100.0 mL of a solution containing 0.300 g of K2CrO4, a bright red precipitate of Ag2CrO4 forms. (a) Assuming that the solubility of Ag2CrO, is negligible, calculate the mass of the precipitate. Ans. The limiting reagent is the mass of the precipitate is g. (b) Calculate the mass of the unreacted component that remains in solution. Ans. The mass of the unreacted component isThe concentration of CO in the air can be determined by passing a known volume of air through a tube containing I2O5, resulting in the formation of CO2 and I2. I2 is removed from the tube by distillation and collected in a solution containing excess KI, producing I3-. I3- is titrated with a standard solution of Na2S2O3. A 4.79 L air sample was sampled as described here, requiring 7.17 ml of 0.00329 M Na2S2O3 to reach the endpoint in a typical analysis. If the density of the air is 1.23×10^-3 g/ml, what is the amount of CO in the air in ppm? (CO: 28 g/ml)I am allowed to Work with someone but due to covid I have to work virtually and I am lost ....I provided the data that I have to go by Use the graphs in the file to determine the concentration of the unknown solution and to answer the other questions from the lab pack.
- 7. An impure sample of Na S04 weighed 1.562 g. A BASO, precipitate from this sample weighed 2.496 g. Calculate the percentage of sulfur and the percentage purity of the salt. Ans. 21.97% S; 97.25% Na S0. ore sample which weirbedFind Ecell = 0.48V. Use dhis regult along with the equilibrium conlentretion of Lu“ (mol/L) wheun 24. C[Cu (NH3), ) = 0.10 mol /L and [N H3] = 6.1 mol/h to calceulate the cqnillibriem Lonstant for the formation of [cu(NH3),]"]1.The max.% of carbon that can be add to iron is. 2.Medium alloy steel has atotal amount of alloying element about ........... 3. .reduces the brittleness of steel alloy by form ...