Amperometric Methods in Control of Water Chlorination

Marks, Henry C.; Bannister, G. L.; Glass, J. R.; Herrigel, Elaine.

doi:10.1021/ac60003a022

Cited by 20 publications

(8 citation statements)

References 8 publications

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“…In an amperornetric titration apparatus (3,4,9), it is titrated to an endpoint with standard phenylarsinoxide solution to give Fraction 1. Then to the same sample is added 0.2 m1.…”

Section: Amperometric Titrationmentioning

confidence: 99%

Determination of Residual Chlorine Compounds

Marks¹,

Williams²,

Glasgow³

1951

Journal AWWA

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“…In an amperornetric titration apparatus (3,4,9), it is titrated to an endpoint with standard phenylarsinoxide solution to give Fraction 1. Then to the same sample is added 0.2 m1.…”

Section: Amperometric Titrationmentioning

confidence: 99%

Determination of Residual Chlorine Compounds

Marks¹,

Williams²,

Glasgow³

1951

Journal AWWA

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“…Residual chlorine in water can be continuously recorded by the use of a rotating copper, platinum, or gold electrode (336,534). One such method, which has been used by the Chicago Water Purification Division since 1942, is based on the depolarizing action of chlorine on a copper electrode (31).…”

Section: Diffractometrymentioning

confidence: 99%

Automatic Operations in Quantitative Analysis

Patterson¹,

Mellon²

1950

Anal. Chem.

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“…Johannesson (2), in his study of the chloramines, reported frequent interferences from other electroreducible species. Marks and Bannister (3) studied the reduction of chloramine at mercury, rotating platinum, and rotating platinum-silver microelectrodes. The "combined" chlorine is more difficult to reduce as compared to "free" chlorine, which is evidenced by a more negative shift in the half-wave potential.…”

mentioning

confidence: 99%

“…These products are pH dependent and are probably formed successively in solution. The reactions may be represented by the equations OC1" + NH3 -NH2C1 + OH" (1) OC1" + NH2C1 -* NHC12 + OH" (2) OC1" + NHC12 -NC13 + OH" (3) These reactions are extremely important when considering water and water supply disinfection with chlorine, hypochlorous acid, and/or hypochlorites (16)(17)(18)(19)(20)(21)(22)(23)(24).…”

mentioning

confidence: 99%

Voltammetric determination of the decomposition rates of combined chlorine in aqueous solution

Evans¹

1982

Anal. Chem.

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The kinetics of the aqueous reactions In free chlorine and excess ammonia were followed voltammetrlcally In the range pH 3-12. Molar ratios of ammonia to hypochlorite varied from 6.3 to 1.3. At pH 12 the pseudo-first-order constant for the formation of chloramine In a large excess of ammonia was 1.1 min"1. At lower pHs the rate was too fast to be measured. The disappearance of combined chlorine was followed over the same pH range. Typical first-order constants In buffered solutions were 2.5 X 10~2 min"1, 1.3 X 10"2 min"1, and 1.9 X 10~2 min"1 at pH 5.0, 7.5, and 11.0, respectively, depending on the dominant chloramine species. An unexpected rate minimum of 1.1 X 10~2 min"1 was observed at pH 9.8, where monochloramine should be the only reactive species. The peak potential for the reduction of chloramine at the hanging mercury drop electrode (HMDE) was an S-shaped function of pH. Essentially constant peak potentials of -0.52 V vs. saturated Ag/AgCI were observed at pH 8-12. At lower pHs the potential shifted anodlcafly Indicating composite potentials. The predominant chloramine species at each pH were confirmed by UV spectroscopy.

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Amperometric Methods in Control of Water Chlorination

Cited by 20 publications

References 8 publications

Determination of Residual Chlorine Compounds

Determination of Residual Chlorine Compounds

Automatic Operations in Quantitative Analysis

Voltammetric determination of the decomposition rates of combined chlorine in aqueous solution

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