If 20 ml of0.5M Na_(2).SO_(4) is mixed with 50ml of 0.2M H_(2)SO_(4) & 30 ml of 0.4M Al_(2)(SO_(4))_(3) solution. Calculate [Na^(+)],[H^(+)].[SO_(4^(2-))],[Al^(3+)]. [Assuming 100% dissociation]

If 20 ml of0.5M Na_(2).SO_(4) is mixed with 50ml of 0.2M H_(2)SO_(4) &

1.	If 20 ml of0.5M Na_(2).SO_(4) is mixed with 50ml of 0.2M H_(2)SO_(4) & 30 ml of 0.4M Al_(2)(SO_(4))_(3) solution. Calculate [Na^(+)],[H^(+)].[SO_(4^(2-))],[Al^(3+)]. [Assuming 100% dissociation]
Answer» Solution :Molarity`=("moles")/("VOLUME")=10M`. Moles of `Na_(2)SO_(4)` `rArr20m`. Moles of `Na^(+)` (i) `therefore[Na^(+)]=(20)/(100)=0.2M` (ii) `[H^(+)]=?` `10m`. Moles `H_(2)SO_(4)` 20M. Moles `H^(+)` `[H^(+)]=(20)/(100)=0.2M` (iii) `[SO_(4)^(2-)]=(10+10+36)/(100)=(56)/(100)=0.56M` (iv) `[Al^(3+)]=(24)/(100)=0.24M` `rarr` Derive a relationship between molarity of a solution in which `w GM` of solute of molar MASS `M g//mol` is dissolved in ` W g` solvent `&` density of resulting solution`=d' g//ml`. say `1 L` solution taken, mass of `1 lit` solution `=(1000 d) g` moles of solute `=("molarity") x m` `therefore=(("molarity")xx1000)/(1000d-"molarity"xxM.Wt)` [Where no, of moles of solute `= "molarity")`