A solution containing `0.1` mol of a metal chloride `MCl_(x)` requires 500ml of `0.8` M `AgNO_(3)` solution for complete reaction `MCl_(x)+xAgNO_(3)rarrxAgCl+M(NO_(3))_(x)`. Then the value of x is :

A solution of 0*1 M of a metal chloride MCl_(x) requires 500 mL of 0*6 M AgNO_(3) solution for complete precipitation. The value of x 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

The mass of Na_(2)CO_(3) required to prepare 500ml of 0.1M solution is

Volume (in ml) of 0.7 M NaOH required for complete reaction with 350 ml of o.3 M H_(3) PO_(3) solution is

An aqueous solution contains 0.22g of metallic chloride, 0.51g of AgNO_(3) is required for complete precipitation of chloride from that solution. If specific heat of the metal be 0.057 then what will be the correct atomic mass of of that metal? What is the formula of that metallic chloride?

Find the no. of moles of the solute present in 500ml of 0.1 M solution.