Suppose that you use 38.00 mL of 0.02500 M KMnO4 in Part 2 of the lab...
Suppose that you use 38.00 mL of 0.02500 M KMnO4 in Part 2 of the lab to titrate 25.00 mL of the diluted H2O2 solution. Given that 10.00 mL of the original H2O2 solution (before dilution) had a mass of 10.849 g, calculate the %H2O2 in the original solution.
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Suppose that you use 38.00 mL of 0.02500 M KMnO4 in Part 2 of
the lab...
The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M...
The density of a 0.0122 M KMnO4 is 1.037 g/mL. Suppose 26.35 g of 0.0122 M KMnO4 are required to titrate 1.072 g of a household H2O2 solution. Except for answers to (a) and (e), use E notation. Do not include units, just enter numerical values. a) calculate the ml of MnO4- added to reach the endpoint. b) calculate the moles of MnO4- added to reach the endpoint. c) calculate the number of moles of H2O2 in the sample. d)Calculate...
suppose you have an unknown sample containing Fe^2+, and you titrate it with KMnO4 standard solution....
suppose you have an unknown sample containing Fe^2+, and you
titrate it with KMnO4 standard solution. Calculate the percent of
Fe in your sample.
equation: MnO4- + 5Fe^2+ + 8H^+ --> Mn^2+ + 5Fe^3+ +
4H2O
Suppose you have an unknown sample containing Feat, and you titrate it with a KMnO4 standard solution. Calculate the percentage of Fe in your sample. Equation: MnO(+5Fe2+ + 8H - Mn2+ + 5Fe3+ + 4H20 Data 0.08124M 2.49g Molarity of the KMnO4 standard solution:...
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...
b. A 13.8 g sample H202 dissolved in water requires 52.5 mL of 0.095 M KMnO4...
b. A 13.8 g sample H202 dissolved in water requires 52.5 mL of 0.095 M KMnO4 solution to reach the endpoint. What is the mass percent and concentration of H2O2 in the original sample? Assume that thę prügina males solution has a density of 1.00 g/mL
3. In the lab you are going to titrate a weak acid solution (25.00 mL of...
3. In the lab you are going to titrate a weak acid solution (25.00 mL of 0.100 M HCHO2, formic acid) with a strong base (0.100 M NaOH). Carry out the following calculations to determine the pH for four key points throughout the titration. Part a. Calculate the volume of 0.100 M NaOH required to reach the equivalence point for the titration. Ans. 25.00 mL Part b. Calculate the initial pH of 0.100 M HCHO2 (before adding any NaOH). Ans....
from the given data sheet, can anyone please let me know how to solve these post lab questions ? Post-Lab Questions...
from the given data sheet, can anyone please let me know how
to solve these post lab questions ?
Post-Lab Questions 1. Calculate the volume of Solution A that you would need to make 50.00 mL of NaOH solution with the same concentration as solution F. Given that one drop of a liquid is 0.05 ml, how many drops of Solution A would be needed? 2. In general, what effect would diluting a NaOH solution have on the pH of...
help please More Information on submitting your Lab Report LAB DATA Concentration (M) of starting solution...
help please
More Information on submitting your Lab Report LAB DATA Concentration (M) of starting solution Transmittance, T. (Blank) T (15 . 0.034 MOP. 7 .com NH, diluted with distilled H 0 to 100 ml. volume) T(15 ml. Unknown CT solution + 7 ml. come NH, diluted with distilled H 0 to 100 ml. total volume) LAB CALCULATIONS Absorbance (15-ml. Dilution) Ratio M/A (use 0.004 M as the given M) for the 15-ml. Dilution Absorbance of Unknown (Is Dilution) Molarity...
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 H2O2 + 2 MnO. - + 6...
suppose you have an unknown sample containing Fe^2+, and you
titrate it with KMnO4 standard solution. Calculate the percent of
Fe in your sample.
equation: MnO4- + 5Fe^2+ + 8H^+ --> Mn^2+ + 5Fe^3+ +
4H2O
Suppose you have an unknown sample containing Feat, and you titrate it with a KMnO4 standard solution. Calculate the percentage of Fe in your sample. Equation: MnO(+5Fe2+ + 8H - Mn2+ + 5Fe3+ + 4H20 Data 0.08124M 2.49g Molarity of the KMnO4 standard solution:...
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...
b. A 13.8 g sample H202 dissolved in water requires 52.5 mL of 0.095 M KMnO4 solution to reach the endpoint. What is the mass percent and concentration of H2O2 in the original sample? Assume that thę prügina males solution has a density of 1.00 g/mL
from the given data sheet, can anyone please let me know how
to solve these post lab questions ?
Post-Lab Questions 1. Calculate the volume of Solution A that you would need to make 50.00 mL of NaOH solution with the same concentration as solution F. Given that one drop of a liquid is 0.05 ml, how many drops of Solution A would be needed? 2. In general, what effect would diluting a NaOH solution have on the pH of...
help please
More Information on submitting your Lab Report LAB DATA Concentration (M) of starting solution Transmittance, T. (Blank) T (15 . 0.034 MOP. 7 .com NH, diluted with distilled H 0 to 100 ml. volume) T(15 ml. Unknown CT solution + 7 ml. come NH, diluted with distilled H 0 to 100 ml. total volume) LAB CALCULATIONS Absorbance (15-ml. Dilution) Ratio M/A (use 0.004 M as the given M) for the 15-ml. Dilution Absorbance of Unknown (Is Dilution) Molarity...
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 H2O2 + 2 MnO. - + 6...
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