Question

20 mL of 0.2M Al2

(SO4

)

3

mixed with 20 mL of 0.6M BaCl2

, the concentration of highly charged cation is

(A) 0.1 (B) 0.2 (C) 0.3 (D) 0.4​

Answer 1

Given:

20 ml of 0.2 M $Al_{2} (SO_{4} )_{3}$

60 ml of 0.6 M $BaCl_{2}$

To find:

Concentration of highly charged cation

Solution:

                          $Al_{2} (SO_{4} )_{3}$     +    $BaCl_{2}$        →     $BaSO_{4}$↓ +    $AlCl_{3}$

Initial                    20*0.2*6          20*0.6*2

concentration        =24                   =24

Final                          0                       0                      24              24    

concentration

• No concentration of $Ba^{2+}$ or $SO^{-2} _{4}$  in solution since BaSO4 gets precipitated

[$M_{eq}$ = N × V in ml = M × valency × V in ml]

• The concentration of highly charged cation = [$Al^{+3}$]  = $\frac{24}{40 * 3}$ = 0.2 M