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ber Coordination Number Constitution of Solutions
Chemical Equilibria Different Types of Reactions
0xidants and Reductants Exchange of Electrons
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acetic acid acid solution add a drop Al3+ alkaline earths alkaline solution aluminium ammine ammonia ammonium anions aqueous solution arsenic As(III attacked Ba2+ Bi(III blue boiling buffer buffer solution Ca2+ cations Cd2+ cent chloride Co2+ colloidal colour colourless complexes compounds concentration cone crystals Cu2+ cyanide Detection dilute disproportionation dissolves drop of solution electrons elements Equilibrium constants excess Fe(III Fe2+ Fe3+ ferric ferrous fluoride formation formed FUNCTION OF pH g.-ion/litre gives Hg2+ hydrogen peroxide hydroxide indicators interfere Interfering iodide iodine ions large number litre low solubility mercuric metals Mg2+ mixture Mn2+ Mo(VI molecules neutral NH4+ Ni2+ nitric acid oxalate oxidation Pb2+ persulphate phosphate precipitate presence quantities reaction reagent redissolves redox indicators REDOX SYSTEMS reduced salts silver slowly Sn(IV sodium solvent Sr2+ stable strong acid sulphate sulphide sulphuric acid thiocyanate Ti(IV tion volts W(VI yellow zinc Zn2+ Zr(IV