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- You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placeIn the following experiment, you will titrate 2.00 mL of 0.0100 M KMnO4 in base with 0.0200 M NaHSO3. Using your balanced redox equation in base from question 3 above, calculate the volume of titrant NaHSO3 you expect to require for a complete reaction. Balanced reaction: 2MnO4^1- + HSO3^1- +3OH^1- <=> 2MnO4^2- + SO4^2- + 2H2O2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4
- .The solubility-product constant for Ag2SO3 is 1.5x10-14. Calculate E0 for the process Ag2SO3(s) +2e → 2Ag + SO3-2In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H2O, at 20−25∘C) OH− CO2−3 SO2−4 CrO2−4 C2O2−4 Mg2+ 0.00069 0.18 35.7 54.8 0.038Ca2+ 0.16 0.00066 0.205 13.2 0.00061Sr2+ 2.25 0.00034 0.135 0.106 0.005Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate.The permanganate ion (MnO4- ) is often used in redox titrations. The strongly colored (violet)the permanganate ion forms the slightly pink Mn2+ ion upon reaction in acidic solution.Permanganate solutions are prepared by dissolving solid potassium permanganate. Atpreparation and storage of the solution, however, often forms brownstone (MnO 2 (s)) which mustfiltered before use. The concentration of the solution is therefore determined directly beforeuse by titration in sulfuric acid solution against sodium oxalate (Na2 C2 O4 ;easily soluble salt that serves as the primary standard) whereby the oxalic acid forms carbon dioxide (gas).Calculate the concentration of a potassium permanganate solution from the following data.0.6501 gram of sodium oxalate is weighed and consumes 20.00 mL of the preparedthe potassium permanganate solution.
- When all of the following are mixed together in a beaker, what is the molar concentration of the SCN- ion in the solution just after mixing but before any reaction takes place? 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 4.00 mL of 2.00 x 10-3 M KSCN 4.00 mL of 0.50 M HNO3 answer is between 0.004 and 0.005, please explain how with steps.The solubility product of Ag2SO3 is 1,5 x 10-14 Calculate E0 , for Ag2SO3 (s) + 2e- ↔ 2 Ag (s) + SO32- Ag+ + e- ↔ Ag E0 = + 0,799 VWhich of the following aqueous salts should result in a precipitate upon addition of aqueous sodium sulfate? - Ca(NO3)2 - KNO3 - Fe(NO3)2 - Al(NO3)3 - Ba(NO3)2 - Mg(NO3)2 - NH4NO3 - NaNO3 please answer fast i give upvote
- Calculations for Acetate Buffer Solutions Molarity of acetic in acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO) is 3.0 × 10-8. At equilibrium, the molarity of H3O+ in a 0.044 M solution of HClO isThe reaction of KOH with HNO2 is presented by the unbalanced chemical reaction below: ___ KOH(aq)+ ___ HNO3 (aq)---> ___ KNO3 (aq)+ ___ H2O(l)Calculate the molar concentration of Nitric acid (HNO2) when 40.5 mL of 0.674 M KOH is required to quench 101.0 mL of Nitric acid over phenolphthalein indicator.