GENERAL CHEMISTRY Laboratory Guide This module provides a laboratory guidelines‚ safety declaration form‚ Lab Report guidelines and Laboratory manual for subject of General Chemistry (CLD 10004). Mohd Zulkhairi Abdul Rahim Laboratory Information Before each lab session‚ you should prepare by reading the lab manual and the textbook required reading. We expect you to have a good understanding of the purpose‚ details of the procedure‚ the use of all chemicals and any significant hazards
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CHEMISTRY PRACTICAL NOTES - SALT ANALYSIS S.No. | EXPERIMENT | OBSERVATION | INFERENCE | 1(a) | Noted the colour of the salt | BluePale greenGreenPale pinkColourless | May be Cu2+May be Fe2+May be Ni2+‚ Cu2+May be Mn2+Absence of Cu2+‚ Fe2+‚ Ni2+‚ Cu2+‚ Mn2+ | (b) | Noted the physical state of the salt | (i)Amorphous(ii)crystalline | May be CO32-May be Cl-‚ Br-‚ SO42-‚ NO3- | 2 | Action of heat:The given salt is heated in a dry test tube. | (i)Reddish brown vapours(ii)Crackling sound(iii)Yellow
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Studying the pH of Strong Acid‚ Weak Acid‚ Salt‚ and Buffer Solutions The purpose of the current experiment was to determine the pH of various hydrochloric acid and acetic acid solutions‚ to determine the pH of various salt solutions‚ to prepare a buffer solution‚ and determine the effects of adding a strong acid and strong base to the buffer solution versus adding a strong acid and strong base to water. The measured pHs for the hydrochloric acid solutions were 1.6‚ 2.2‚ 2.9‚ and 3.8. The measured
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Because we synthesized the two most common kidney stones‚ calcium oxalate and calcium phosphate‚ we will focus on those two in the discussion of formation‚ treatment‚ and prevention. Calcium stones like calcium oxalate and calcium phosphate stones form when urine is “supersaturated with the constituent ions that comprise the stone” (Figge). This means‚ when urine is supersaturated with calcium and oxalate ion that type of stone is more likely to form. This supersaturation results from the ionic activity
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preparation protocol allowed ZnFe2O4 to have a smaller particle size and larger specific surface area leads to increasing of oxygen mobility. 3.2. Microcalorimetry analysis 3.2.1. Water adsorption As it is known‚ the cation as a Lewis acid (host) contributes to the stabilization of an anion as a Lewis base (base) resulting
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normally referred to as a cation. Now the chlorine atom‚ with an extra electron‚ has an overall negative charge (Cl-)‚ and is referred to as an anion. © KC Distance Learning The cation and anion with opposite electric charges are electrostatically attracted and form a neutrally charged‚ ionically bonded ion pair – in this case sodium chloride (NaCl). Na - e- → Na+ and Figure 2: This valence electron model illustrates a sodium (Na) atom losing an electron to form a sodium cation (Na+). The free electron
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hydrogenation-FALSE Endoplasmic reticulum: Endoplasmic = within the cytoplasm‚ reticulum = “little net” Atoms: Nucleus= protons (+) and neutrons ( ) Surrounding nucleus = electrons (-) Ions: unequal number of protons and electrons -Cation = more protons than electrons (+ charge) -Anion = more electrons
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flask. 4. The visual cue that allows you to determine that the first step of the reaction has gone to completion is the slowing down and eventual stopping of reflux. A substitution reaction occurs and yields Br‚ which poses a water-soluble group A anion. 5. A) The washes that are performed in part B are necessary because the RTILs are often contaminated with halide slats such as KBr‚ which would cause the RTIL to be cloudy. In order to remove the halide contamination washes must be performed until
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Environmental Chemistry and Analysis Prof. M.S.Subramanian MODULE 1.5 Advanced Waste Water Treatment Removal Of Suspended Solids Microstraining Coagulation and flocculation Filtration Removal of dissolved solids Ion exchange Reverse osmosis Electrodialysis Removal of nitrogen Phosphate removal (chemical treatment) Phosphate removal (biological treatment) Removal of dissolved organic compounds Adsorption Sludge treatment and disposal Disinfection 1 2 2 3 3 4 6 7 8 9 10 10 10 11 13 Indian
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molecule (Wikipedia). Ionic compounds are basically defined as being compounds where two or more ions are held next to each other by electrical attraction. One of the ions has a positive charge called a cation and the other has a negative charge called an anion. Cations are usually metal atoms and anions are either nonmetals or polyatomic ions. Usually‚ when we have ionic compounds‚ they form large crystals that you can see with the naked eye (4). A covalent compound is a compound in which the atoms
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