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[0256] The amount of glycol (1,2-ethane-diol), C$_{2}$H$_{6}$O$_{2 }$ which must be added to 1.00 L ofH$_{2}$O such that the solution does not freeze above -20° C. may be calculated as follows: 

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where kf (H$_{2}$O)=1.86° C. kg mol-1; llT=i kfm where i=l. Since 1.0 Lhasa mass of 1.0 kg, 10.8 mo! of ethylene glycol is needed, so 10.8 molx62 g/mol=670 grains of ethylene glycol. The density of ethylene glycol is 1.1088. Therefore, 670 g/1.1088 g/mL=604 ml, which is dissolved in 1 L=6.04 ml in 10 ml. At this concentration, the viscosity of such a solution renders it unusable for aerosol spraying. 

[0257] The amount ofNaC!that must be added to 1.00 L of H$_{2}$O to decrease the freezing point to -20° C. can be calcu› lated: 

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where NaCl(s)-Na+(aq)+Cl-(aq) i=2 and i kf=2 (1.86° C. kg mol- 1 ). Therefore, 5.376 molx58.44 g/mot=314.17 g NaCl must be added to 1 kg (1 L) ofH$_{2}$O. 

[0258] The amount of NaO$_{2 }$ must be added to 1.00 L of H$_{2}$O to decrease the freezing point to -20° C. can also be calculated. In this example, the salts CsO$_{2}$ , RbO$_{2}$ , KO$_{2}$ , and Na$_{2}$O$_{2 }$ were prepared by the direct reaction of 0 2 with the respective alkali metal. The 0---0 bond distance in NaO$_{2 }$ is 1.33 A, vs. 1.21 AinO$_{2 }$ and 1.49 Ain o/-. The overall trend corresponds to a reduction in the bond order from 2 (0$_{2}$ ), to 1.5 (0$_{2 }$ -), to 1 (0 2 2 -). The alkali salts of sodium are orange› yellow in color and quite stable, provided they are kept dry. Upon dissolution of these salts in water, however, the dis› solved decomposes extremely rapidly: 

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In this process 0 2 - acts as a strong Bronsted base, initially forming HO$_{2}$ . The pKa ofits conjugate acid, hydrogen super› oxide (HO$_{2}$ , also known as "hydroperoxyl" or "perhydroxy radical") is 4.88, so that at neutral pH 7 the vast majority of superoxide is in the anionic form. 

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## Example 2 

## Example 3 

## Example 4 

Therefore, 5.376 molx54.98 g/mol=295.57 g NaO$_{2 }$ must be added to 1 kg (1 L) ofH$_{2}$O. 

[0259] This Example relates to the ultraviolet absorbance spectra of diphenyl phosphorochloridate (DPCP) and estab› lishing a standard curve for detecting and quantitating hydrolysis of an organophosphate ester, diphenyl chloro› phosphate, which is a stimulant for G-class Nerve Agents. For the testing of the G surrogates, certain physical properties were investigated and employed. DPCP has two six-carbon aromatic phenyl rings attached to a single phosphorous atom through an ether bond. 

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[0260] Other properties include the fact that the phenol and phenyl aromatic rings of this chemical are structurally related to benzene; the absorbance spectra of benzene like systems are characterized by E-bands and B-bands; the absorbance spectrum of benzene shows broad absorption bands in the near ultraviolet region between 230 nm and 270 nm; the fine structure arises from vibrational sublevels accompanying the electronic transitions; and the substitution of auxochromic groups on to the benzene ring produces marked changes in the benzene spectrum. 

[0261] The conversion of phenol to phenolate creates an additional unshared pair of non-bonding electrons available for interaction with then-electrons of the aromatic nucleus. The availability of these additional non-binding electrons result in a bathochromic shift of the first and second bands. One objective of this example is to establish a standard curve for the detection of diphenyl chlorophosphate. The param› eters to detect units vs. molar concentration are as follows: (i) the MW=268.33 g/M; (ii) the LD$_{50 }$is not available; (iii) the dynamic Range objective=6 logs; (iv) the lower limit of detectionobjective=4.8xl0- 6 M/L=4.8µMolar=6.192ng/ml; (v) the molar extinction coefficient 260 nm,.,459 L mole- 1 cm- 1 in one solution of the invention; and (vi) the molar extinction coefficient 220 nm""6,000 L mole-$^{1 }$cm- 1 . 

[0262] The detection technologies evaluated in this example include absorbance spectroscopy using cuvette sam› pling; reversed phase HPLC with an absorbance detector; HPLC/Mass Spectroscopy; gas chromatography with a flame ionization detector; and solid phase sampling with HPLC. 

[0263] This Example relates to the generation of a standard curve for the detection of the organophosphate ester DPPC, which structure and characteristics are given above. The fol› lowing equations are useful for the determination of hydroly› sis of a biological or chemical warfare agents. 

## Example 5 

## Example 6 

