2 millimolar solution of sodium ferrocyanide is 60% dissociated at 27°C. osmotic pressure of the slotution is .

Given that 2 millimolar solution of sodium ferrocyanide (Na4[Fe(CAN)6] ) is 60% dissociated at 27°C.

First find van't Hoff facter's (i) than Calculate osmotic pressure (π)= icRT as follow:

Decimolar solution of K4[Fe(CN)6] dissociate by 60% at 27°C. Determine osmotlc pressure in Nature/M2.

We know that osmotlc pressure is equal to the (π) = iCRT then  first Calculate the value of(i) then osmotlc pressure.

A complex is represented as CoCl3.xNH3.Freezing point of its 0.1 molar solution is - 0.558° C (Kf = 18.6) Assuming 100 % dissociation and coordination number of Co(iii) is six , the what is the complex formula ?

We can find the formula of Complex by :

A complex is wrltten as M(en)y.xBr. lts 0.05 molar solution shows 2.46 atm osmotlc pressure at 27°C. Assuming 100 % ionisaton and coordination number of metal (iii) is six, complex may be:

The Complex is M(en)y.xBr. and given c= 0.05 M, osmotlc pressure = 2.46 atm and The= 300K.

We know that osmotlc pressure (π)= icRT

Where To is universal gas constant = 0.0821j/mole per K

Then I = π/ cRT = 2.46/0.05×0.0821×300

                           =2 

  The vant Hoff facter's is (2) means their is two ions furnish after dissociation of Complex since  coordination number is (6) and van't hoff facter is (2) then formula of Complex is :

[M(en)2Br2]Br --> [M(en)2Br2]+  +Br- 

A non Stoichiometric oxide of iron represented as Fe_x O_1.0 , contains one Fe+3 for every three Fe+2 ions , then find the value of x is...

Given that one Fe+3 for every Fe+2 and total ions of Fe+3 and Fe+2 is equal to "x"  then number of Fe+3 is x/4 and Fe+2 is equal to 3x/4.

Finally we can calculate the value of x by balancing Oxidation state of Compound, given as :