" A hydrate of "Na_(2)SO_(3)" has "50%" water by mass.It is: "

A hydrate of Na_(2)SO_(3) completely loses 22.2% of water by mass on strong heatin. The hydrate is-

The compound Na_(2)CO_(3).xH_(2)O has 50% H_(2)O by mass. The value of 'x' is

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

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

Sodium sulphate is soluble in water whereas barium sulphate is sparingly soluble because (a) the hydration energy of Na_(2)SO_(4) is less than its lattice energy (b) the hydration energy of Na_(2)SO_(4) is more than its lattice energy (c) the lattice energy of BaSO_(4) is more than its hydration energy (d) the lattice energy has no role to play in solubility

The hydrated salt Na_(2)SO_(4).xH_(2)O undergoes 55% loss in weight on heating and becomes anhydrous. The value of x will be

The hydrated salt, Na_(2)SO_(4)*nH_(2)O undergoes 55.9% loss in weight on heating and becomes anhydrous. The value of n will be:

A 7.66 g sample of hydrated sodium sulphate, Na_(2)SO_(4). xH_(2)O , forms 4.06g of anhydrous Na_(2)SO_(4) . What is the value of x? {:("Molar mass", (gmol^(-1))), (Na_(2)SO_(4), 142):}

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