Method and Tips for Inorganic Qualitative Analysis
This is a rough draft of the complete answer. A lot more will be added to the answer very soon. At present, it includes the common tests for sulfite and bisulfite ions. Please do not downvote just because it is not a complete answer yet.

Identification Of Sulfite Anion: ($\ce{SO3^{2-}}$)

All sulfites are insoluble except "group IA sulfites " and$\ce{(NH4)2SO4}$. Sulfite ppt. is always white in color.

Test With Acid:

$\ce{SO3^{2-} + H^{+} -&gt; SO2 (g)}  $ 

Sulfur dioxide gas is evolved which gives lime water test as well as baryta water test:

$\ce{SO2 + Ca(OH)2 -&gt; Ba(HSO3)2}[\text{soluble}]$ 

$\ce{SO2 + Ba(OH)2 -&gt; Ca(HSO3)2}[\text{soluble}]$

Test with $\ce{BaCl2/CaCl2}$:

$\ce{SO3^{2-} + CaCl2 -&gt; CaSO3 + 2Cl^{-}}$

$\ce{SO3^{2-} + BaCl2 -&gt; BaSO3 + 2Cl^{-}}$

Note that $\ce{BaSO3}$ is slowly oxidized by atmospheric oxygen to form heavy white ppt of $\ce{BaSO4}$. Similarly:

$\ce{BaSO3 + Br2 -&gt; BaSO4 + Br-}$

$\ce{BaSO3 + H2O2 -&gt; BaSO4 + H2O}$

$\ce{BaSO3 + HNO3 -&gt; BaSO4 + NO}$

Test With $\ce{Pb(NO3)2}$:

$\ce{Pb(NO3)2 + SO3^{2-} -&gt; PbSO3 [\text{white ppt.}]}$

On boiling $\ce{PbSO3}$ in presence of $\ce{O2}$, $\ce{PbSO4}$ is produced.

(On boiling $\ce{PbS2O3}$ we get $\ce{PbS}[\text{black ppt}]$ and $\ce{H2SO4}$. Hence, this fact can be used to distinguish sulfites from thiosulfates).

Test With $\ce{AgNO3}$:



Schiff's Test/Fuschin's Test/Magenta Reagent Test:

Both $\ce{SO3^{2-}}$ and $\ce{SO2}$ are decolorized in this test.

Distinguishing b/w $\ce{SO3^{2-}}$ and $\ce{CO3^{2-}}$ ion:





Some Important Redox Reactions:

$\ce{MnO4- + SO2/H2S -&gt; Mn^{2+} + SO4^{2-}/S}$

$\ce{Cr2O7- + SO2/H2S -&gt; Cr^{3+} + SO4^{2-}/S}$

$\ce{Br2 + H2O + SO2/H2S -&gt; Br- + SO4^{2-}/S}$

$\ce{Fe^{3+} + SO2/H2S -&gt; Fe^{2+} + SO4^{2-}/S}$

$\ce{IO3- + SO2/H2S -&gt; I2 [\text{gives deep blue color in starch}] + SO4^{2-}/S}$

$\ce{SO2}$ can either be oxidized to $\ce{SO4^{2-}}$ or reduced to $\ce{S^{2-}}$. But, $\ce{H2S}$ can only be oxidized to $\ce{S}$.

Notable Reaction (Comproportionation) : $\ce{\ce{SO4^{2-}} + \ce{H2S} -&gt; S + H2O}$

Points to remember:


$\ce{CO2/CO/CO3^{2-}/HCO3^{-}}$ do not show any change on treatment with with oxidizers like $\ce{KMnO4/K2Cr2O7/Br2\text{ water}/Fe^{3+}/IO3^{-}}$
$\ce{S^{2-},SO3^{2-}/HSO3^{-}}$ do show change on treatment with with oxidizers like $\ce{KMnO4/K2Cr2O7/Br2\text{ water}/Fe^{3+}/IO3^{-}}$.
$\ce{SO3^{2-} + H2O2 -&gt; SO4^{2-} + H2O}$ $ [\text{no visible change is observed}]$ 




Dvarda Alloy ($\ce{Zn}/\ce{Al}/\ce{Cu}$):

$\ce{Zn + NaOH -&gt; Na2ZnO2 + 2H}$

In presence of dvarda alloy the following reactions can take place:

$\ce{SO3^{2-} -&gt; S^{2-}}$

$\ce{SO2 -&gt; H2S}$

$\ce{NO2^{-} -&gt; NH3}$

$\ce{NO^{3-} -&gt; NH3}$

$\ce{Zn}$ reacts with dil. $\ce{H2SO4}$ to produce $\ce{H2}$ gas which can also reduce $\ce{SO4^{2-}}$ to $\ce{S^{2-}}$.



Test with Sodium Nitroprusside:

$\ce{Na2[Fe(CN)5NO] + ZnSO4 -&gt; Zn[Fe(CN)5NO] [\text{salmon pink ppt }]}$

$\ce{Zn[Fe(CN)5NO] + \text{moist} SO2 -&gt; \text{red color compound}}$

$\ce{S2O3^{2-}}$ and $\ce{S^{2-}}$ ions also give the test. So they can be removed on treating with $\ce{HgCl2}$ as follows:

$\ce{Hg^{2+} + S^{2-} -&gt; HgS}$ 

$\ce{Hg^{2+} + S2O3^{2-} -&gt; HgS2O3}$ 

$\ce{HgS2O3 [\text{on heating}]-&gt; HgS [\text{black ppt}] + H2SO4}$



Identification Of Bisulfite Anion ($\ce{HSO3^{-}}$):

Test With Acid:

$\ce{HSO3^{-} + H^{+} -&gt; SO2 (g)}$

Test With $\ce{H2O2}$:

$\ce{SO3^{2-} + H2O2 -&gt; SO4^{2-} + H2O} $

$\ce{HSO3^{-} + H2O2 -&gt; H^{+} + SO4^{2-} + H2O} $ (acidic)