1) State if the following A student has already correctly identified his positive unknown tube. Ho pours some of his green, positive ion unknown into a clean centrifuge tube. He adds NaCl to this tubo and gets a precipitate. He centrifuges that precipitate and decants the clear liquid into a new clean testtube.. To that new tube, he adds Na,so and gets another precipitate. He centrifuges this tube, and decants the clear liquid into another clean, dry testtube. To this freshly decanted liquid, he adds NaOH and gets a third precipitate. This student concluded that he had Ag*, Ba*2 and Ni+2 in his positive ion unknown.
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- If the same mass of Na2SO4 (MW: 142 g/mol) and K2SO4 (MW: 174 g/mol) were weighed and used for the gravimetry experiment, which will yield a greater amount of precipitate? Assume that the experiment was done correctly. • Indeterminate, it will depend on the amount of BaCl2 used. • They will yield the same amount of precipitate because the same mass was initially weighed. • K2SO4 because it has a larger molecular weight.Table 1: Qualitative Analysis of Group II Cations Group II Cations Confirmatory Reagent Result/ Observation Substance Formed Inference Write the chemical equations involve in the analysis of group II cations. Guide Question: What are differences of the precipitates of each cation in group II? Reference video : https://www.youtube.com/watch?v=BZGZZx1lHKAD. Water Softening 1.For this part of the experiment, watch the video on the link(s) below: https://www.youtube.com/watch?v=jDgSohKVLio Question: Comparison between the relative amount of precipitates for soft vs. hard water. Comparison between the relative amount of bubbles for soft vs. hard water.
- 9. An aqueous solution of sulfuric acid is prepared by mixing a secondary standard of sulfuric acid with deionized water. The aforementioned acid is to be used as a titrant hence its concentration must be accurately determined. To do this, Engr. Polinar, standardized the titrant by titrating two liters of ammonia at 0.90 atm and 30 deg C. From the experiment, 134 mL of the titrant was necessary to neutralize the ammonia. Determine the concentration of the acid in terms of normality? 10. Engr. Forcadela is optimizing a plastic formulation by manipulating the phosgene concentration injected as a gas during the reaction. To obtain credible results, he considered the propensity of phosgene to dissociate into carbon monoxide and chlorine gas at 395 deg C. Performing an experiment at the aforementioned temperature, an equilibrium is reached amongst the species where the total pressure is at 3 atm. If the equilibrium constant expression in terms of concentration for the reaction at 395 deg C…Topic: Standardization of acid and base with back titration Note: Include up to 4 decimal places Kindly explain the process Thank you!In bromine water test Procedure: -Add 3 ml of phenol and ethanol in separate test tube-Add 10 ml of water to each test tubes-Transfer to bigger test tubes-For phenol and ethanol, Add bromine water drop by drop until bromine color persists MUST DO: Observe formation of precipitate P.s I provided photos for better visualization of the overall result procedure, I just need a further and detailed answer based on observation. If answered properly I will upvote, I promise tyyy. Please do focus on the formation of precipitate, thank youuu The first photo is the phenol one (colored one) and the second one is the ethanol (clear one)
- In bromine water test Procedure: -Add 3 ml of phenol and ethanol in separate test tube-Add 10 ml of water to each test tubes-Transfer to bigger test tubes-For phenol and ethanol, Add bromine water drop by drop until bromine color persists MUST DO: Observe formation of precipitate P.s I provided photos for better visualization of the overall result procedure, I just need a further and detailed answer based on observation. If answered properly I will upvote, I promise tyyy The first photo is the phenol one (colored one) and the second one is the ethanol (clear one)3. It is used to convert the known weight of the precipitate to the corresponding weight of the analyte. a. Gravimetric factor b. Mole ratio c. Mass ratio d. All of the choices 4. Which of the following is used to express the ppm of the solution? a. Kg analyte/liter solution b. Mg analyte/liter solution x 10^6 G analyte/ g sample x 10^6 d. Kg analyte/kg sample C.The graphic below shows the general procedure for titrating the saturated solution of magnesium hydroxide with hydrochloric acid. Select all of the true statements from the choices below. 1. Obtain a saturated solution of magnesium hydroxide. 0 2. Transfer 30.0 mL to an Erlenmeyer flask using a volumetric pipet. Add phenolphthalein. 3. Titrate to a colorless endpoint using 0.0020 M hydrochloric acid. It is important that the aliquot drawn in step 2 does not contain undissolved magnesium hydroxide solid. For titrations of the saturated solutions at elevated temperatures, the solution must be held at high temperature for the duration of the titration. Hydrochloric acid is the analyte in this titration. The volume of liquid in the buret should be read before and after the titration. At the endpoint of the titration, the solution will turn from colorless to pink.
- 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.Three drops of the phenolphthalein chemical indicator should be added to the acidic analyte sample (KHP or citric acid) before every titration. You will then carefully add the base to the analyte until the solution turns O a. from clear to a very pale pink color. O b. from a pale pink color to totally clear. O. from a dark pink color to totally clear. O d. from clear to a very dark pink color.1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/L