How does the addition of aqueous NH3 to a solution separate and identify Cut and Bi ions? Why wouldn't the addition of a strong base, such as KOH, work just as well as the addition of aqueous NH3?
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- (1) Describe how adding a solution of KOH to the original sulfide precipitate results in the separation of Sn4+ ion from the other Group II cations. (2) Why wouldn’t a weak base, such as aqueous NH3, work just as well as aqueous KOH in (1)?If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/Lwill you expect the solubility of sn-cu solution to be high? please explain why or why not?.
- Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. Number of moles of NaOH = 0.005 moles Since the reaction between acetylsalicylic acid and NaOH is a 1:1 reaction, the number of moles of acetylsalicylic acid used in the reaction is also 0.005 moles. the concentration from analysis question 5: acetylsalicylic acid in the 100.00 mL volumetric flask is 0.050 M. From your plot, what is the value of εb? From the Beer- Lambert law For the aspirin sample, calculate the concentration of acetylsalicylic acid present using the value of εb that you found The concentration from analysis question 5 represents the concentration in the 10.00 mL sample that was prepared in the volumetric flask using an aliquot of the solution in the…Use the systematic treatment to get the concentrations of all the species in a solution of: a.) saturated PbSO4 buffered at pH 7One and only one combination of cobalt salt and solvent should have turned blue, thusindicating the presence of [CoCl4]2− ion. Explain why only this combination underwent a reactionand the others did not.
- Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. RbBr (s) ->Sometimes it is not possible to indicate the end point of a titration.a) How can one proceed then and what is the name of the type of titration that can be performed? Briefly describe. An example in which this method can be used is in the determination of mercury, which forms strong complexes with EDTA, but for which there is no suitable indicator that can indicate the end point. b) You are given the task of determining the Hg2 + concentration in a sample solution? After adding an excess of EDTA, the sample solution is titrated with a magnesium solution. 20.00 ml of a 0.0452 M EDTA solution was added to 30.00 ml of sample solutionThe excess EDTA was determined by adding 0.0500 M Mg 2+ solution, consuming 4.37 ml to the end point.Explain why the addition of NH3 or HNO3 to a saturated solution of Ag2CO3 in contact with solid Ag2CO3 increases the solubility of the solid.
- What is the purpose of adding concentrated ammonia in the elimination test for cations? Select one: a. because NH3 is a stronger base than NaOH b. to provide a strongly basic solution c. to determine if the hydroxide precipitates are amphoteric d. to determine if the test ions form NH3 complexes e. to determine if the NH3 solution oxidizes the test ionsCan cadmium (II), and mercury (II) be separated quantitatively by precipitation as sulfides from a solution that is 0.15 M cadmium nitrate and 0.10 M in mercuric ions? If possible, what range of sulfide concentration is permissible? Do you expect any interference from the formation of hydroxides of both heavy metals? CdS (144.46); Ksp = 1.0 x 10 ^ -27HgS (232.66); Ksp = 2.0 x 10 ^ -53 HINT: Determine the concentration at which each of the cations start to precipitate out of solution. >Quantitative precipitation means 1/1000 remains in solution.For all metal ion - EDTA complxes, what is the relationship between the conditional formation constant Kf' and the normal formation constant, Kf ? -The conditional formation constant is always less than or equal to Kf at all pHs.. -The conditional formation constant is usually less than Kf, but can sometimes be greater than Kf for some metal ions at high pHs. -The conditional formation constant is always less than Kf at all pHs.. -There are no restrictions. Depending on the metal ion and the pH, the conditional formation constant can be less than, equal to, or greater than Kf.