考试中经常用到的规律（The regularity that is frequently used in examinations）.doc

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考试中经常用到的规律（The regularity that is frequently used in examinations）.doc

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考试中经常用到的规律（The regularity that is frequently used in examinations）

考试中经常用到的规律（The regularity that is frequently used in examinations） : 1, solubility law - see solubility table; 2, commonly used acid and alkali indicator color range: The color range of indicator PH Methyl orange 3.1 red 3.1 - 4.4 orange 4.4 yellow 8 8 - 10 colorless phenolphthalein red light red 10.0 5.1 5.1 - 8 litmus red purple blue 8.0 3, on inert electrode, the order of discharge of various ions: Cathode (electronic capacity): Au3+, Ag+Hg2+, Cu2+, Pb2+, Fa2+, Zn2+, H+,, Al3+Mg2+, Na+, Ca2+, K+ Anode (electron loss ability): S2-, I-, Br - Cl-, OH- oxygen radical Caution: if the metal is used as an anode, the anode itself will undergo oxidation-reduction reactions (Pt, Au, except for electrolysis) 4. Double hydrolysis ion equation writing: (1) write the hydrolysis ion on the left and write the hydrolysate on the right; (2) trim: trim the charge on the left and trim the other atoms on the right. (3) H and O are rough and add water over there. Example: when Na2CO3 and AlCl3 mixed solution: 3 CO32- + 2Al3+ + 3H2O = 2Al (OH): 3CO2 = 3 + 5. Write the equation for the total electrolysis reaction: (1) analysis: what is the reactant and the product; (2) Pei Ping. Example: KCl: 2KCl + 2H2O electrolytic solution = = = H2 + Cl2 = 2KOH + 2KCl + 2H2O = = trim: H2 = Cl2 = 2KOH + + 6, a chemical reaction method in two electrode reaction: (1) to write 2.5 electrons reaction; (2) consider the reaction of the environment (acidic or alkaline); (3) the number and the atomic charge is equal to the number of two sides. Example: the reaction in the battery is: Pb + PbO2 + 2H2SO4 = 2PbSO4 + 2H2O, write the electrode reaction as the primary battery (discharge). Write 2.5 responses: Pb - 2e- = PbSO4, PbO2, +2e-, PbSO4 Analysis: in acidic environment, fill in other atoms: negative: Pb + SO42--2e- = PbSO4 Positive: PbO2 + 4H+ + SO42- +2e- = PbSO4 + 2H2O Note: when charging, it is electrolysis, and the electrode reaction is the reverse of the above electrode reaction: For: cathode: PbSO4