The hydrate salt `Na_2 CO_3.xH_2O` undergoes `63%`loss in mass on heating and becomes anhydrous. The value of `x` is :

The hydrated salt Na_(2)CO_(3).xH_(2)O undergoes 63% loss in mass on heating and becomes anhydrous . The value x is :

The hydrated salt Na_2 SO_4. nH_2 O undergoes 56% loss in mass on heating and becomes anhydrous. The value of 'n' will be :

Na_(2) CO_(3). 10 H_(2) O is

A 6.85g sample of the hydrated Sr(OH)_2.x H_2O is dried in an oven to given 3.13g of anhydrous sr(OH)_2. What is the value of x? (Atomic masses : Sr=87.60.O=16.0,H=1.0)

A 6.85g sample of the hydrated Sr(OH)_2.x H_2O is dried in an oven to give 3.13g of anhydrous Sr(OH)_2. What is the value of x? (Atomic masses : Sr=87.60.O=16.0,H=1.0)

Decomposition of a hydrated form of Na_(2)CO_(3) cause approximately 63% loss in its mass on strong heating. If the heating only cause removal of water of crystallization then formula of the hydrated salt is

How many molecules of water are present as water of crystallisation in Borax Na_(2)B_(4)O_(7).nH_(2)O if it loses 47.117% of mass on heating till it becomes anhydrous?

13.4 g of a sample of unstable hydrated salt Na_(2)SO_(4).XH_(2)O was found to contains 6.3 g of H_(2) O . The number of molecular of water of crystalistion is

A 3.0 g sample of Na_(2)CO_(3).H_(2)O is heated to a constant mass. How much anhydrous salt remains ?