Solvation is the process of dissolving.
Dissociation is the separation of a substance into charged components during dissolution.
<h3>What is the difference between dissolving and dissociating?</h3>
Dissolution (dissolving), which simply refers to becoming solvated by the solvent, is a subset of dissociation, which is particularly the separation of two charged ions in solution. When the solvent completely envelops each individual solute molecule, solvation takes place. By definition, something that is dissociated in a solvent must be dissolved in it. For instance, the salt dissociates in water, which is how it dissolves in water. In water, ethanol dissolves but does not dissociate; it remains ethanol.
<h3>How does Van't Hoff's factor work?</h3>
The Van't Hoff factor is a tool used to compare the real number of moles of solute injected to create a solution to the apparent amount produced by colloidal characteristics.
<h3>What is the Van't Hoff factor's value?</h3>
Van't Hoff factor's value is:-
- No association or dissociation i=1
- Dissociation i<1
- Association i>1
Learn more about Van't Hoff's factor here:-
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Which of the following statements is generally true about change in the workplace ? a ) Most people accept change easily . b) Smart companies can avoid change altogether. c) Change in the workplace fairly infrequently d) Individuals can learn to manage the change in their lives.
What basically your question is can you tell
Answer:
Mg^2+ and OH- are the chemical species present at the equilibrium. Mg(OH)2 will not affect the equilibrium.
Explanation:
Step 1: data given
Reactants are Solid Mg(OH)2 and H2O(l)
Kc1 = 1.8 * 10^-11
Step 2: The balanced equation
Mg(OH)2(s) ⇄ Mg2+(aq) + 2OH-(aq)
Step 3: Define the equilibrium constant Kc
Kc = [OH-]²[Mg^2+]
Pure solids and liquids do not have any effect or influence on the equilibrium in the reaction. So they are not included in the equilibrium constant expression.
This means Mg^2+ and OH- are the chemical species present at the equilibrium. Mg(OH)2 will not affect the equilibrium.
