How many moles of magnesium phosphate $M{g}_3(P{O}_4{)}_{2}Mg\_3(PO\_4)\_2$ will contain 0.25 mole of oxygen atoms?

Which among the following is the heaviest?

The molality of 1L solution of 93% $H_{2}S{O}_{4}H\_2SO\_4$ (w/v) having density of 1.84 g/mL is :

0.7g of $N{a}_{2}C{O}_3\mathrm{.}x{H}_{2}ONa\_2CO\_3.xH\_2O$ is dissolved in 100 mL water, 20 mL of which required 19.8 mL of 0.1N HCl. The value of x is :

The normality of 20 volume hydrogen peroxide solution is

Vapour density of a volatile substance is 4. Its molecular weight would be :

3g of an oxide of a metal is converted to chloride completely and it yielded 5g of chloride. The equivalent weight of the metal is :

If 0.50 mole of $BaC{l}_{2}BaCl\_2$ is mixed with 0.20 mole of $N{a}_{3}P{O}_4,Na\_3PO\_4,$ the maximum number of moles of $B{a}_3(P{O}_4{)}_{2}Ba\_3(PO\_4)\_2$ that can be formed is :

A molar solution is one that contains one mole of solute in :

In which mode of expression, the concentration of a solution remains independent of temperature?