. Essentials of medical and clinical chemistry. With laboratory exercises . he gas, and is relightedagain as it is withdrawn. 14 Fill a side-neck test-tube one-third full of dilute (10 per cent.) sulphuricacid; add several bits of zinc; close its mouth with a cork, and attacha delivery-tube as in Fig. 7. Wait until the air is expelled, and then ignitethe gas as it issues, or collect it over water, and test it as in the previous ex-periment. 15 Attach an ordinary clay pipe to the delivery-tube of the hydrogen gen-erator and blow hydrogen soap bubbles; they rise in the air. 1HLet the demonstrato
. Essentials of medical and clinical chemistry. With laboratory exercises . he gas, and is relightedagain as it is withdrawn. 14 Fill a side-neck test-tube one-third full of dilute (10 per cent.) sulphuricacid; add several bits of zinc; close its mouth with a cork, and attacha delivery-tube as in Fig. 7. Wait until the air is expelled, and then ignitethe gas as it issues, or collect it over water, and test it as in the previous ex-periment. 15 Attach an ordinary clay pipe to the delivery-tube of the hydrogen gen-erator and blow hydrogen soap bubbles; they rise in the air. 1HLet the demonstrator fill a bladder or rubber bag with two parts of hydro-gen and one of oxygen or five of air; attach a tube and blow up soap bubblesin a basin. Touched with a flame, they explode. PART I. INORGANIC CHEMISTRY. 21 OXYGEN (O—16).—Occurrence. Most abundant of theelements, comprising one-fifth of the air, eighth-ninths of water,one-half of the crust of the earth, and three-fourths of allorganized bodies. Preparation.—Made most easily by heating potassium chlorate Fig. (Fig. 8), and decomposing it into potassium chloride and oxygen,thus : KC103 = KC1 + Physical Properties.—A colorless, odorless and tasteless gas, alittle heavier ( times) than air. Under a pressure of and at a temperature of —136 C, it condenses into 17 Grind in a mortar some potassium chlorate with half as much manganesedioxide, a black powder that facilitates the evolution of the oxygen. Heat this10 a side-neck test-tube as in Fig. 8, or in an open test-tube. Recognize theoxygen by the energetic combustion when a match, or even the glowring endof the charred stick is introduced. Note.—Experiments 18, 19 and 20 are to be performed by the instructor. 22 ESSENTIALS OF CHEMISTRY. Fig. 9.
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