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3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6 H...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6H→ 5...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H202 + 2 MnO - +61 +502...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO. - + 6...
How do you calculate grams of H2O2 from the expeimental data given? (acidic medium) MnO4 +...
How
do you calculate grams of H2O2 from the expeimental data given?
(acidic medium) MnO4 + H2O2 = Mn2+ + O2 The spectator ion, K, has been left out of the equation. CH" + 2 MnO4 + Shooa 2M na +502 + 8 H2O BRAND OF HYDROGEN PEROXIDE ANALYZED: If no brand name is provide, create a name for the hydrogen peroxide brand. Be creative. AVERAGE EXPERIMENTAL MOLARITY OF THE KMnO4 SOLUTION USED: 0.0968 M KMnO4 ERLENMEYER FLASK NUMBER: #4...
2. In order to analyze a commercial H O solution using the procedure in this experiment,...
2. In order to analyze a commercial H O solution using the procedure in this experiment, it must first be diluted with distilled water. Consider 10.0 mL of a commercial peroxide solution measured with volumetric pipet diluted to 100.0 mL in a volumetric flask. If 25.00 mL of the diluted solution is titrated with 0.0202 M MnO4, calculate the percent H2O2 in the commercial peroxide solution, i.e. before dilution. The initial buret reading was 0.08 mL, and the final reading...
2 MnO4 (aq) + 5 H2O2(aq) + 6 H(aq) → 5 O2(aq) + 2 Mn2+ (aq)...
2 MnO4 (aq) + 5 H2O2(aq) + 6 H(aq) → 5 O2(aq) + 2 Mn2+ (aq) + 8 H20(1) completely oxidize 25.0 mL of a H2O2 solution, calculate the molarity of the H20, solution
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5...
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of...
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of unknown molarity starts at a buret reading for NaOH of 0.33 mL The phenolphthalein indicator turns light pink the acid solution for over 30 seconds at a buret reading of 24.19 mL 2) What was the volume of HCl you started with? 3) How many moles of HCl were in the original solution? 4) Write the balanced chemical equation for the titration reaction. 5)...
A solution of 5 x 10-3 M MnO4- is dissolved in 25.00 mL of H2O. What...
A solution of 5 x 10-3 M MnO4- is dissolved in 25.00 mL of H2O. What volume of H2O must be added to the solution to reduce the concentration of [MnO4- ] to 7.5 x 10-4 M? If possible, please show work so I can learn and understand how you approached the problem and solved it. Thanks!
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6 H...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6H→ 5...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H202 + 2 MnO - +61 +502...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO. - + 6...
How
do you calculate grams of H2O2 from the expeimental data given?
(acidic medium) MnO4 + H2O2 = Mn2+ + O2 The spectator ion, K, has been left out of the equation. CH" + 2 MnO4 + Shooa 2M na +502 + 8 H2O BRAND OF HYDROGEN PEROXIDE ANALYZED: If no brand name is provide, create a name for the hydrogen peroxide brand. Be creative. AVERAGE EXPERIMENTAL MOLARITY OF THE KMnO4 SOLUTION USED: 0.0968 M KMnO4 ERLENMEYER FLASK NUMBER: #4...
2. In order to analyze a commercial H O solution using the procedure in this experiment, it must first be diluted with distilled water. Consider 10.0 mL of a commercial peroxide solution measured with volumetric pipet diluted to 100.0 mL in a volumetric flask. If 25.00 mL of the diluted solution is titrated with 0.0202 M MnO4, calculate the percent H2O2 in the commercial peroxide solution, i.e. before dilution. The initial buret reading was 0.08 mL, and the final reading...
2 MnO4 (aq) + 5 H2O2(aq) + 6 H(aq) → 5 O2(aq) + 2 Mn2+ (aq) + 8 H20(1) completely oxidize 25.0 mL of a H2O2 solution, calculate the molarity of the H20, solution
1. (4p) In an acidic aqueous solution, Fe2+ ions are oxidized to Fe3+ ions by MnO4": 5Fe2+(aq) + MnO4 (aq) + 8H(aq) → 5Fe3+ (aq) + Mn2(aq) + 4H2O(1) In part A of the experiment, suppose that 1.067 g of Fe(NH4)2(SO4)2.6H2O(s) are placed in a 250 ml Erlenmeyer flask to which 20 mL of water and 8 mL of 3 M H2SO4(aq) are added. The solution was titrated to the end point by adding 26.89 mL of KMnO4(aq) from the...
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