Calculate the theoretical yield of silver chloride, if 5.15 g of neighborhood chloride have been added when silver nitrate is in excess. BaCl2 + 2AgNO3 --> 2AgCl + Ba(NO3)2
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- 1. How is complete precipitation assured in the Group III Cations? 2. In the confirmatory test of Magnesium ion, why is it necessary to heat the centrifugate in water bath for 5 minutes? 3. If Magnesium hydroxide is a white gelatinous precipitate, why is the confirmatory result indicated a blue precipitate?A 1.000-g sample containing bromide was dissolved in sufficient water to give 100.0 mL. A 50.00 mL aliquot was measured and after acidification, silver nitrate was introduced to precipitate AgBr, which was filtered, washed, and then dissolved in an ammoniacal solution of potassium tetracyanonickelate(II): Ni(CN)42- + 2AgBr(s) → 2Ag(CN)2- + Ni2+ + 2Br-50.00 mL remaining solution was analyzed for its Br- content by potentiometry using a metallic electrode of the second kind. a) Write the cell notation of the potentiometric set-up with SCE as the reference electrode. b) Write the Nernst equation that describes the indicator electrode set-up. Ecell recorded in running the solution using the potentiometric set-up was Ecell = 0.0286 V. (E0Ag/AgBr = 0.095 V) c) Compute for Eind. d) Compute pBr in the 50.00 mL aliquot. e) Compute for % NaBr ( in the potentiometric technique).Suppose that 0.323 g of an unknown sulfate salt is dissolved in 50 mL of water. The solution is acidified with 6 M HCl, heated, and an excess of aqueous BaCl2 is slowly added to the mixture resulting in the formation of a white precipitate. 1) Assuming that 0.433 g of precipitate is recovered calculate the percent by mass of SO42− in the unknown salt. 2) If it is assumed that the salt is an alkali sulfate determine the identity of the alkali cation.
- if we use KMnO4 and H3Po4 and MnSO4 for tritation of fecl3 and calculation of. Fe2+ what suitable ratio for tritationExplain why colour of KMnO4 disappears when oxalic acid is added to its solution in acidic medium.The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
- Complete the balanced dissociation equation for the compound below in aqueous solution. AgI ->a) Which ion, Pt(II) or Mn(II), is more likely to form a sulfide in the presence of H2S in water. b) Rationalize your answer with the trends in hard and soft character. c) Give a balance chemical equation from your reaction.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/L
- A sample weighing 0.6760 g that contains an unknown amount of BaCl₂ was completely dissolved in water and treated with an excess of sodium sulfate. Na2SO4 A precipitate of BaSO4 formed which was dried and weighed, yielding 0.4105 g. What percentage of the original sample was BaCl₂? 39.77 24.15 35.72 69.78 54.18Assuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and a value of 3.5 × 10−11 for the solubility product of FeCO3, what would you expect to be the stable iron species at pH 9.5 and pE −8.0, as shown in Figure 3.4?You are assigned an unknown solution that contains Group III cations. To -1 mL of this solution was added 6 M NH3 the solution was agitated to mix well, and a reddish-brown precipitate with a gelatinous solid clinging to the inner walls of the test tube was observed. The solution was centrifuged and the supernatant was tested for completeness of precipitation by adding an additional drop of 6 M NH3. No cloudiness was observed as the drop of reagent diffused through the solution. The supernatant was then carefully decanted into a clean test tube, labeled (1st solution), and saved for further testing later. The precipitate remaining in the test tube was washed with a small amount of water, centrifuged, and the wash decanted and discarded. To the precipitate was added about 10 drops of 6 M NAOH plus ~1 mL H20 and the test tube was vigorously agitated. The resulting suspension was centrifuged and the supernatant liquid was transferred to another clean test tube and clearly labeled (2nd…