Practical Proofs of Chemical Laws: a Course of Experiments Upon the ...
Practical Proofs of Chemical Laws: a Course of Experiments Upon the ...
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In our eReader you can find the full English version of the book. Read Practical Proofs of Chemical Laws: a Course of Experiments Upon the ... Online - link to read the book on full screen. Our eReader also allows you to upload and read Pdf, Txt, ePub and fb2 books. In the Mini eReder on the page below you can quickly view all pages of the book - Read Book Practical Proofs of Chemical Laws: a Course of Experiments Upon the ...
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To quickly assess the difficulty of the text, read a short excerpt:
— Preparation of the two chlorides of copper in a state of purity.
Cuprous chloride, — (The pupil should be ac- quainted with the mode of formation of this salt.) Take the salt as obtained from the dealers (which is not pure), dissolve it in a little strong, pure hydrochloric acid, and pour the clear solution into a large beaker of distilled water. The cuprous chloride is thrown down as a white precipitate, which quickly settles to the bottom of the beaker.
Syphon off the bluish solution as qui...ckly as pos- sible ; the loss of some of the precipitate does not matter. Fill the beaker again with distilled water, stir up, allow to settle, and syphon off again.
Repeat the operation a third time, to ensure that the washings are free from cupric salt. The pure white cuprous chloride which remains at the bottom of the beaker would readily oxidise if dried. No attempt, therefore, is made to dry and weigh the substance, it being sufficient for our purpose to determine the ratio of copper to chlorine in an unknown weight of the salt.
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You can find similar books in the "Read Also" column, or choose other free books by Vaughan Cornish to read onlineMoreLess
To quickly assess the difficulty of the text, read a short excerpt:
— Preparation of the two chlorides of copper in a state of purity.
Cuprous chloride, — (The pupil should be ac- quainted with the mode of formation of this salt.) Take the salt as obtained from the dealers (which is not pure), dissolve it in a little strong, pure hydrochloric acid, and pour the clear solution into a large beaker of distilled water. The cuprous chloride is thrown down as a white precipitate, which quickly settles to the bottom of the beaker.
Syphon off the bluish solution as qui...ckly as pos- sible ; the loss of some of the precipitate does not matter. Fill the beaker again with distilled water, stir up, allow to settle, and syphon off again.
Repeat the operation a third time, to ensure that the washings are free from cupric salt. The pure white cuprous chloride which remains at the bottom of the beaker would readily oxidise if dried. No attempt, therefore, is made to dry and weigh the substance, it being sufficient for our purpose to determine the ratio of copper to chlorine in an unknown weight of the salt.
What to read after Practical Proofs of Chemical Laws: a Course of Experiments Upon the ...?
You can find similar books in the "Read Also" column, or choose other free books by Vaughan Cornish to read onlineMoreLess
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