What are the final concentrations of all the ions when following are mixed? 50 m L of 0.12 M F e N O 3 3 ,…

What are the final concentrations of all the ions when following are mixed? 50 mL of 0.12 M FeNO33, 100 mL of 0.10M FeCl3 and 100 mL of 0.26 M MgNO32?
  1. Fe3+=0.064M; NO3-=0.28 M ;  Fe3+=0.12 M;Mg2+=0.04 M
  2. Fe3+=0.064M; NO3-=0.28 M ;  Fe3+=0.12 M;Mg2+=0.104 M
  3. Fe3+=0.04M; NO3-=0.28 M ;  Fe3+=0.12 M;Mg2+=0.104 M
  4. Fe3+=0.064M; NO3-=0.8 M ;  Fe3+=0.12 M;Mg2+=0.104 M

Solution

Milli-mole of FeNO33 = 50 × 0.12 = 6  (mm=M×VmL)

∴  Milli-mole of Fe3+ = 6 ;

Milli-mole of NO3-=3 ×6= 18 

Milli-mole of FeCl3= 100 × 0.1 = 10

Milli-mole of Fe3+= 10 ;

Milli-mole of Cl- =3 × 10 = 30 

Milli-mole of MgNO32 = 100 × 0.26 = 26

Milli-mole of Mg2+ = 26 ;

Milli-mole of NO3-= 2 × 26 = 52

On mixing these three, total volume he comes 250 mL

Thus Fe3+=6+10250=0.064M

NO3-=18+52250=0.28 M

Cl-=30250=0.12 M

Mg2+=26250=0.104 M

Asked in: JEE-TOPICTESTS-CHEMISTRY

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