Class 11th
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New answer posted
8 months agoContributor-Level 10
It is product of molar concentration of ion raised to the power of number of ions produced per compound in saturated solution.
Solubility of electrolyte decreases due to common ion effect.
New answer posted
8 months agoContributor-Level 10
Equilibrium is a state at which rate of forwarding reaction is equal to the rate of backward reaction. The equilibrium between ions and unionised molecules is called ionic equilibrium.
New answer posted
8 months agoContributor-Level 10
A catalyst does not affect the equilibrium composition of a reaction mixture. Catalysts influence the rate of both forward and backward reactions equally.
New answer posted
8 months agoContributor-Level 10
Equilibrium constant depends upon the way in which the reaction is written.
New question posted
8 months agoNew answer posted
8 months agoContributor-Level 10
5.10. We know,
PV=nRT
n = PV/RT
n= (0.1 x34.05 x 10-3)/ (0.083 x 819)
&n
New answer posted
8 months agoContributor-Level 10
(a) In case of a non-polar (covalent) solvent, solvation enthalpy is small and hence, not sufficient to overcome lattice enthalpy of the salt. Consequently, the salt does not dissolve in non-polar solvent. As a general rule, for a salt to be able to dissolve in a particular solvent its solvation enthalpy must be greater than its lattice enthalpy so that the latter may be overcome by former. Each salt has its characteristic solubility which depends on temperature.
New answer posted
8 months agoContributor-Level 10
(d) Higher order ionization constants (Ka2, Ka3) are smaller than the lower order ionization constant (Ka1) of a polyprotic acid. The reason for this is that it is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces. This can be seen in the case of removing a proton from the uncharged H2CO3 as compared from a negatively charged HCO3–.Similarly, it is more difficult to remove a proton from a doubly charged HPO42– anion as compared to H2PO4–.
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