What volume (in ml) of 0.8M `AlCl_(3)` solution should be mixed with 50 ml of 0.2 M `CaCl_(2)` solution to get solution of chloride ion concentration equal to 0.6 M ?

What volume (in ml) of 0.2 M H_(2)SO_(4) solution should be mixed with the 40 mL of 0.1 M NaOH solution such that the resulting solution has the concentration of H_(2)SO_(4) as 6/55M?

20 ml of CaCl_(2) solution is mixed with 30 ml of 0.1MAlCl_(3) solution. If the resulting solution has chloride ion concentration equal is 0.34 M, the concentration of CaCl_(2) solution added is :

40 ml of 0.1 M CaCl_2 solution is mixed with 50 ml of 0.2 M AgNO_3 solution. Mole of AgCl formed in the reaction is

40 ml of 0.1 M CaCl_2 solution is mixed with 50 ml of 0.2 M AgNO_3 solution. Mole of AgCl formed in the reaction is

100 ml of 0.1 M solution A is mixed with 20ml of 0.2 M solution B. The final molarity of the solution is :

500 ml of 0.1 M AlCl_(3) is mixed with 500 ml of 0.1 M MgCl_(2) solution. Then calculation the molarity of Cl^(-) in final solution.

500 ml of 0.1 M AlCl_(3) is mixed with 500 ml of 0.1 M MgCl_(2) solution. Then calculation the molarity of Cl^(-) in final solution.

50mL of "3MHCl" solution is mixed with 150mL of 1M FeCl_(3) solution.The concentration of chloride ion in the resultant solution is (in mole/lit)

What volume of 0.2 M NaOH (in ml) solution should be mixed to 500 ml of 0.5 M NaOH solution so that 300 ml of final solution is completely neutralised by 20 ml of 2 M H_(3) PO_(4) solution [Assuming 100% dissociation]