. Hydroxylamine : its quantitative determination and some double salts . la-mine was found to be more stable in methyl alcohol than in ethylalcohol, absolute methyl alcohol was used as the solvent. The abso-lute methyl alcohol after being boiled several days with calciumoxide, and allowed to stand several hours over metallic calcium,was distilled and tightly corked. The ether used was dried overcalcium chloride. The weighed amount^about 10 grams^of hydroxylamine hydro-chloride was dissolved in 60 of absolute alcohol and then thecalculated amount of freshly prepared sodium methylate added.
. Hydroxylamine : its quantitative determination and some double salts . la-mine was found to be more stable in methyl alcohol than in ethylalcohol, absolute methyl alcohol was used as the solvent. The abso-lute methyl alcohol after being boiled several days with calciumoxide, and allowed to stand several hours over metallic calcium,was distilled and tightly corked. The ether used was dried overcalcium chloride. The weighed amount^about 10 grams^of hydroxylamine hydro-chloride was dissolved in 60 of absolute alcohol and then thecalculated amount of freshly prepared sodium methylate added. Etherwas now added to precipitate the sodium chloride and the clear solu-tion of free hydroxylamine was filtered off and used to dissolvemetallic salts, as copper sulphate, nickle sulphate, manganese chlo-ride etc. In every case the salts were arjhydrous. Using ten grains hydroxylamine hydrochloride xvould be aboutthe same as adding five grams free hydroxylamine and making up toabout one hundred and tv;enty-five , the solution would containabout .04 grams per c, -16- In trying to determine amount of hydroxylamine in colu-tion titanium solution, no concordant results were obtained,.000464, ,000234,.00053 grams respectively. No reason has yetbeen found why the titanium would not react quantitatively withthe hydroxylamine in alcohol solution. But the method of reduction of ferric sulphate worked accurately enough for strength of solution giving .0435 and .0471 grams per of the solution. of NHpOH sol. KiSnO. Wt. KHpOH used to oxidize ^sed. the FeSO^ per co. solution 10 .0433 g. 20 .0471 g. Knowing approximately the strength of the hydroxylaminesolution, and allov^ring an excess over the amount to crystallizewith anJhydrouB copper sulphate to form CuSQ^.6NHgOH, the green solu-tion (obtained by allowing the alcoholic hydroxylamine to stand overanhydrous copper sulphate) was filtered and allowed to crystallizein a quiet room at a temperature belo
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