1. Cr20aq) + CI Cr3+ (aq) + Cl2c9) in acidic solution (aq) 2. Cus) + NO3 (aq) Cu aa) + NO2) + NO29) in acidic solution 3. CN(ag) + Мп04 (аg) CNO (aq) + Mn02(s) in basic solution
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complete and balance this equation by the method of half reaction
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- A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanationC8This is for my reviewer please help me with the step by step solution and answer, thank you
- Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. In such a standardization it was found that a 0.498-g sample of sodium carbonate required 24.8 mLmL mL of a sulfuric acid solution to reach the end point for the reaction. Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq)Na2CO3(aq)+H2SO4(aq)→H2O(l)+CO2(g)+Na2SO4(aq) What is the molarity of the H2SO4H2SO4?You collected the following data from a titration experiment using a 0.129M standardized NaOH solution to titrate a 26.55 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Trial 1 0.44 19.69 ?? Trial 2 0.18 17.2 Trial 3 0.50 19.94 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units.3I- + OCl- + 2H+ ----> I3- + Cl- + H2: A 25.00 ml sample of liquid bleach was diluted to 1000 ml in a graduated flask. A 25 ml portion of the diluted sample was pipetted into an Erlenmeyer flask and treated with excess KI to oxidize OCl- to Cl- and I3- was produced at the end of the reaction. The released I3 was titrated with 0.09892 M Na2S2O3 and 8.96 ml was spent to reach the turning point besides the starch indicator. What is the percent by weight/volume of NaOCl in the bleach sample? (NaOCl:74.44 g/mol)
- 0.1724g of a mineral containing MnO₂ was dissolved and then treated with excess iodide according to the following unbalanced reaction: MnO2(s) + H+ → Mn²+ + I2 + H₂O The I₂ released was titrated with a solution of Na₂S2O3 0.07320 mol/L, requiring 14.65 mL to reach the point end of degree a) Determine the percentage of MnO₂ in the ore. b) When iodine solutions are used as titrants these are prepared by dissolving 1₂ in concentrated KI. Explain the reason for the need for KI in the preparation of these solutions?The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
- For full contact with the acid, nitrile gloves with at least 0.4 mm thickness are required. The thickness of the nitrile gloves in our labs is 6 mil (1 mil = 0.001 in). Will our gloves protect you from full contact with concentrated HCl? Show a calculation to support your conclusions.Show complete solution. Round-off your answers to four decimal places The amount of copper in a wire was determined by a redox titration using KMnO4 as the titrant. A 0.4185-g sample was dissolved in acid and the liberated Cu2+ quantitatively reduced to Cu+, using a reductor column. Titrating with 0.0250 M KMnO4 requires 41.27 mL to reach the endpoint. Determine the % w/w CuO in the sample of meteorite. Answer: % CuO = ______Make a scheme with this procedure. Write the result. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in the centrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in each centrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid in each sample. 5. To the centrifuge containing Al+3 and Cr+3, slowly add…