Insoluble sulfide compounds are generally black in color. Which of the following combinations could yield a black precipitate? Check all that apply. > View Available Hint(s) O Na2S(aq)+ KCI(aq) O Li,S(aq) +Pb(NO3)2(aq) O Pb(CIO3)2 (aq) + NaNO3 (aq) OAGNO3 (aq) +KCl(aq) O K2S(aq)+ Sn(NO3)4(aq) Submit Part C Enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate. onswer as a chemical equation.
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- Observations and Interpretations 1) Balance the chromate / dichromate equilibrium equation: CrO42-(aq) + H+(aq) Cr2O72-(aq) + H2O(l) (unbalanced equation) 2) What was the original color of the K2CrO4solution? If the above equilibrium is established in the original solution, which species, CrO42-(aq), or Cr2O72-(aq) appears to be present in greatest amount? 3) What color did you observe after adding the 3M H2SO4 solution? 4) What color did you observe after adding the 1M NaOH solution? 5) Assume that the dynamic equilibrium represented in the equation in 1 is present in the original solution you placed in the test tube. Based on LeChatelier’s Principle, as stated above on page one, you will interpret the observations made in 2, above: (Notethat H2SO4 produces H+ in solution.) a) When sulfuric acid was added, which reaction (forward or reverse) was favored? What evidence supports this? Why would this reaction be…GROUP II – CATION ANALYSIS Group II consists of eight different cations : Hg+2, Pb+2, Bi+3, Cu+2, Cd+2, As+3, Sb+3 and Sn+4. They form very insoluble sulfides with characteristic colors at the 3-5 pH range. Thioacetamide, CH3CSNH2, is generally used to supply S2- to avoid the direct use of the very toxic, odoriferous H2S gas. At pH less than 3, thioacetamide hydrolyzes to furnish H2S; at a pH greater than 5, thioacetamide reacts directly with the cation to give a complex which subsequently hydrolyzes to acetamide and the insoluble sulfide. Analysis of Group II cations involves, its division into two subgroups by the action of the KOH solution. Consequently, Group IIA contains those cation sulfides which are insoluble in KOH, and Group IIB is composed of those which dissolve in KOH solution. PROCEDURE: Precipitation of Group II Ions Place 10 drops each of the test solutions in a 10-mL test tube. To this, add 2 drops of 3M HNO3 and heat in a water bath…You have a sample of approximately 100 mg/L of calcium carbonate and the standardized EDTA has a concentration of 0.00085 M. If you only want to spend approximately 15 mL of the titrant and add 25 mL of sample in the Erlenmeyer flask, can you use it or should you dilute it? the sample?, how much? Solution: No, 29 mL would be needed to titrate the sample, you must dilute it approximately 1: 2. Taking, for example, 25 mL of sample and making up to 50 mL.
- POTASSIUM PERMANGANATE AND SULFURIC ACID Place 10 drops of 0.1M potassium permanganate solution in a test tube. Add 2 drops of 6M sulfuric acid. Add drop by drop 0.1M sodium bisulfite solution until a definite color change is observed. Observations: Balanced chemical equation: H2SO4(aq) + 4KMnO4(aq) + 10NaHSO3(aq) → 6H2O(l) + 2K2SO4(aq) + 4MnSO4(aq) + 5Na2SO4(aq) What substance is responsible for the color change?Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. CuSO4From the stock solution (0.040 M), pipet 0.00, 2.00, 5.00, 10.00, 15.00 and 20.00 aliquots into 100 mL volumetric flasks. Develop the color (royal blue) by adding enough NH3 solution to form Cu(NH3)42+ complex. Add 10 mL excess to stabilize to complex. Dilute to the desired volume. Determine the concentration of each standard solution and tabulate. *I'm not sure if a Dilution Factor (DF) is still needed in here but I hope you can also explain this if DF is still needed in the computation.Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. CuSO4From the stock solution (0.040 M), pipet 0.00, 2.00, 5.00, 10.00, 15.00 and 20.00 aliquots into 100 mL volumetric flasks. Develop the color (royal blue) by adding enough NH3 solution to form Cu(NH3)42+ complex. Add 10 mL excess to stabilize to complex. Dilute to the desired volume. Determine the concentration of each standard solution and tabulate.
- xpress numerical result with an accuracy of: Х,Х 1. The substance to be analyzed – is deep-pink colored, highly soluble in water salt. Reaction with NH3 gives blue-colored precipitate, which can be dissolved in NH3 surplus accompanied by dirty-yellow colored solution formation. After precipitation of cation by “sodium carbonate drawing out” method, supernatant was independently treated by silver nitrate solution and barium chloride solution (in acid medium in both cases) – any precipitation hasn`t been observed. Addition of antipyrin in acid medium changes color to red. What kind of substance is this? Explain you answer, provide chemical equationsQualitative test of iron complex One test tube contains K3[Fe(C2O4)3].3H2O, one test tube contains ferric ammonium sulfate. To each test tubes, add a small amount of KSCN, then add more oxalic acid. For the potassium complex, the following colour changes are observed: Light green -> Yellow (With KSCN) -> Dark Yellow (Oxalic acid) For the Ferric ammonium sulfate, the following colour changes are obsserved: Light brown -> Blood red (KSCN) -> Yellow (Oxalic) Qns: Deduce the relative stabilities of the Fe(III) oxalate, aqua and thiocyanate complexes. Explain the order of stability.The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:(a) AgBr: [Ag+] = 5.7 × 10–7 M, [Br–] = 5.7 × 10–7 M(b) CaCO3: [Ca2+] = 5.3 × 10–3 M, [CO32−] = 9.0 × 10–7 M(c) PbF2: [Pb2+] = 2.1 × 10–3 M, [F–] = 4.2 × 10–3 M(d) Ag2CrO4: [Ag+] = 5.3 × 10–5 M, 3.2 × 10–3 M(e) InF3: [In3+] = 2.3 × 10–3 M, [F–] = 7.0 × 10–3 M
- Only typed explanation otherwise leave it What weight of pyrite containing 36.40% S must be obtained for analysis in order to give a precipitate of BaSO4 weighing 1.0206 g? A. 0.38 g B. 0.26 g C. 0.14 g D. 0.10 gSources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Measured mass of the precipitate 1. Filter paper was dried prior to filtration. EX _____ ET TOPIC: Standardization of Titrant 2. Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX ______ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) 3. No blank correction EX ______ ETSituation: The amount of protein in a sample of cheese is determined by a Kjeldahl analysis for nitrogen. After digesting a 0.9814-g sample of cheese, the nitrogen is oxidized to NH4+, converted to NH3 with NaOH, and distilled into a collection flask containing 50.00 mL of 0.1047 M HCl. The excess HCl is back titrated with 0.1183 M NaOH, requiring 22.84 mL to reach the bromothymol blue end point. Questions: Write the reactions involved in the above Kjeldahl analysis? Bromothymol blue is used as the indicator of titration; can you give the reason for this?