Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement
A gravimetric method for the quantitative assessment of the products of electrolysis of water is presented. In this approach, the electrolysis cell was directly powered by 9 V batteries. Prior to electrolysis, a known amount of potassium hydrogen phthalate (KHP) was added to the cathode compartment,...
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| Format: | Article |
| Language: | English |
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Wiley
2018-01-01
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| Series: | Journal of Analytical Methods in Chemistry |
| Online Access: | http://dx.doi.org/10.1155/2018/2681796 |
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| author | Samuel Melaku Zewdu Gebeyehu Rajeev B. Dabke |
| author_facet | Samuel Melaku Zewdu Gebeyehu Rajeev B. Dabke |
| author_sort | Samuel Melaku |
| collection | DOAJ |
| description | A gravimetric method for the quantitative assessment of the products of electrolysis of water is presented. In this approach, the electrolysis cell was directly powered by 9 V batteries. Prior to electrolysis, a known amount of potassium hydrogen phthalate (KHP) was added to the cathode compartment, and an excess amount of KHCO3 was added to the anode compartment electrolyte. During electrolysis, cathode and anode compartments produced OH−(aq) and H+(aq) ions, respectively. Electrolytically produced OH−(aq) neutralized the KHP, and the completion of this neutralization was detected by a visual indicator color change. Electrolytically produced H+(aq) reacted with HCO3−(aq) liberating CO2(g) from the anode compartment. Concurrent liberation of H2(g) and O2(g) at the cathode and anode, respectively, resulted in a decrease in the mass of the cell. Mass of the electrolysis cell was monitored. Liberation of CO2(g) resulted in a pronounced effect of a decrease in mass. Experimentally determined decrease in mass (53.7 g/Faraday) agreed with that predicted from Faraday’s laws of electrolysis (53.0 g/Faraday). The efficacy of the cell was tested to quantify the acid content in household vinegar samples. Accurate results were obtained for vinegar analysis with a precision better than 5% in most cases. The cell offers the advantages of coulometric method and additionally simplifies the circuitry by eliminating the use of a constant current power source or a coulometer. |
| format | Article |
| id | doaj-art-c753587110834c1e914a6a97263aae6e |
| institution | Kabale University |
| issn | 2090-8865 2090-8873 |
| language | English |
| publishDate | 2018-01-01 |
| publisher | Wiley |
| record_format | Article |
| series | Journal of Analytical Methods in Chemistry |
| spelling | doaj-art-c753587110834c1e914a6a97263aae6e2025-02-03T05:43:33ZengWileyJournal of Analytical Methods in Chemistry2090-88652090-88732018-01-01201810.1155/2018/26817962681796Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric MeasurementSamuel Melaku0Zewdu Gebeyehu1Rajeev B. Dabke2Department of Chemistry, Columbus State University, Columbus, GA 31907, USADepartment of Chemistry, Columbus State University, Columbus, GA 31907, USADepartment of Chemistry, Columbus State University, Columbus, GA 31907, USAA gravimetric method for the quantitative assessment of the products of electrolysis of water is presented. In this approach, the electrolysis cell was directly powered by 9 V batteries. Prior to electrolysis, a known amount of potassium hydrogen phthalate (KHP) was added to the cathode compartment, and an excess amount of KHCO3 was added to the anode compartment electrolyte. During electrolysis, cathode and anode compartments produced OH−(aq) and H+(aq) ions, respectively. Electrolytically produced OH−(aq) neutralized the KHP, and the completion of this neutralization was detected by a visual indicator color change. Electrolytically produced H+(aq) reacted with HCO3−(aq) liberating CO2(g) from the anode compartment. Concurrent liberation of H2(g) and O2(g) at the cathode and anode, respectively, resulted in a decrease in the mass of the cell. Mass of the electrolysis cell was monitored. Liberation of CO2(g) resulted in a pronounced effect of a decrease in mass. Experimentally determined decrease in mass (53.7 g/Faraday) agreed with that predicted from Faraday’s laws of electrolysis (53.0 g/Faraday). The efficacy of the cell was tested to quantify the acid content in household vinegar samples. Accurate results were obtained for vinegar analysis with a precision better than 5% in most cases. The cell offers the advantages of coulometric method and additionally simplifies the circuitry by eliminating the use of a constant current power source or a coulometer.http://dx.doi.org/10.1155/2018/2681796 |
| spellingShingle | Samuel Melaku Zewdu Gebeyehu Rajeev B. Dabke Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement Journal of Analytical Methods in Chemistry |
| title | Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement |
| title_full | Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement |
| title_fullStr | Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement |
| title_full_unstemmed | Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement |
| title_short | Feasibility of Using an Electrolysis Cell for Quantification of the Electrolytic Products of Water from Gravimetric Measurement |
| title_sort | feasibility of using an electrolysis cell for quantification of the electrolytic products of water from gravimetric measurement |
| url | http://dx.doi.org/10.1155/2018/2681796 |
| work_keys_str_mv | AT samuelmelaku feasibilityofusinganelectrolysiscellforquantificationoftheelectrolyticproductsofwaterfromgravimetricmeasurement AT zewdugebeyehu feasibilityofusinganelectrolysiscellforquantificationoftheelectrolyticproductsofwaterfromgravimetricmeasurement AT rajeevbdabke feasibilityofusinganelectrolysiscellforquantificationoftheelectrolyticproductsofwaterfromgravimetricmeasurement |