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Hydrolysis (/ h aɪ ˈ d r ɒ l ɪ s ɪ s /; from Ancient Greek hydro- 'water' and lysis 'to unbind') is any chemical reaction in which a molecule of water breaks one or more chemical bonds. The term is used broadly for substitution , elimination , and solvation reactions in which water is the nucleophile .
Solvation or dissolution is a kinetic process and is quantified by its rate. Solubility quantifies the dynamic equilibrium state achieved when the rate of dissolution equals the rate of precipitation. The consideration of the units makes the distinction clearer. The typical unit for dissolution rate is mol/s.
Aqua ions are subject to hydrolysis. The logarithm of the first hydrolysis constant is proportional to z 2 /r for most aqua ions. The aqua ion is associated, through hydrogen bonding with other water molecules in a secondary solvation shell. Water molecules in the first hydration shell exchange with molecules in the second solvation shell and ...
No significant dissolution takes place. For example, iron oxides are converted to iron hydroxides and the hydration of anhydrite forms gypsum. [38] Bulk hydration of minerals is secondary in importance to dissolution, hydrolysis, and oxidation, [37] but hydration of the crystal surface is the crucial first step in hydrolysis. A fresh surface of ...
Dissolution of weak acids in alkaline media is similarly important. + () + The uncharged molecule usually has lower solubility than the ionic form, so solubility depends on pH and the acid dissociation constant of the solute. The term "intrinsic solubility" is used to describe the solubility of the un-ionized form in the absence of acid or alkali.
A broader definition of acid dissociation includes hydrolysis, in which protons are produced by the splitting of water molecules. For example, boric acid (B(OH) 3) produces H 3 O + as if it were a proton donor, [11] but it has been confirmed by Raman spectroscopy that this is due to the hydrolysis equilibrium: [12]
If the hydration energy is greater than the lattice energy, then the enthalpy of solution is negative (heat is released), otherwise it is positive (heat is absorbed). [3]The hydration energy should not be confused with solvation energy, which is the change in Gibb's free energy (not enthalpy) as solute in the gaseous state is dissolved. [4]
The rate of dissolution will decrease substantially once it needs to penetrate through the pores of substance A in order to continue targeting substance B. [1] This penetration can often lead to dissolution of substance A, [1] or the product of more than one solute, [10] both unsatisfactory if specific leaching is desired.