Which represents the ionization of a strong electrolyte?
CH3OH(l) mc015-1.jpg CH3OH(aq)
K3PO4(s) mc015-2.jpg 3K+(aq) + PO43–(aq)
H2CO3(aq) mc015-3.jpg H+(aq) + HCO3–(aq)
CH3COOH(aq) + H2O(l) mc015-4.jpg H3O+(aq) + CH3COO–(aq)
Electrolyte ionizations fall into 2 categories ( 3 if you include non-electrolytes )...
Strong Electrolytes => Ionize 100%
Weak Electrolytes => Ionize < 100%
Non-Electrolytes => Ionize 0%
Strong Electrolytes include:
Strong Acids (HCl, HBr, HI, HNO3, HClO4 & H2SO4 (1st ionization step only).
All salts (metal + nonmetal) ionize 100%, but not all salts have the same solubility in water. However, whatever does dissolve, ionizes 100%.
So, for the above question, choices a, b, & d are weak acids... Only K3PO4 qualifies a salt. Salts ionize 100%... Now the degree of ionization does govern it's strength as a conducting electrolyte. Typically, group 1A salts have high solubilities in water and proceed to provide strong charge flow because of hi concentration of ions in solution. Salts with very low solubilities give very low levels of solubility delivering few conductive ions into solution and there fore have poor conductivity properties.
Find the slope of the line passing through the points 2003-13-02-00-00_vl_files/i0020000.jpg and 2003-13-02-00-00_vl_files/i0020001.jpg.
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The correct representation of the ionization of a strong electrolyte is:
K3PO4(s) -> 3K+(aq) + PO43-(aq)
The ionization of a strong electrolyte is represented by the second equation:
K3PO4(s) → 3K+(aq) + PO43–(aq)
To determine which equation represents the ionization of a strong electrolyte, we need to understand the characteristics of a strong electrolyte.
A strong electrolyte is a substance that completely dissociates into ions when dissolved in water, resulting in a high concentration of ions in the solution. This complete dissociation is often indicated by the presence of strong acids, strong bases, and salts in their ionic forms.
Let's examine each equation to see which one meets these criteria:
1. CH3OH(l) → CH3OH(aq)
This equation represents the process of dissolving methanol (CH3OH) in water. However, pure methanol is a covalent compound and does not dissociate into ions when dissolved in water. Therefore, this equation does not represent the ionization of a strong electrolyte.
2. K3PO4(s) → 3K+(aq) + PO43–(aq)
This equation shows the complete dissociation of potassium phosphate (K3PO4) into potassium ions (K+) and phosphate ions (PO43–). As a salt, potassium phosphate represents a strong electrolyte that readily dissociates into ions when dissolved in water.
3. H2CO3(aq) → H+(aq) + HCO3–(aq)
This equation represents the dissociation of carbonic acid (H2CO3) into hydrogen ions (H+) and bicarbonate ions (HCO3–). However, carbonic acid is a weak acid that only partially ionizes in water. Hence, this equation does not represent the ionization of a strong electrolyte.
4. CH3COOH(aq) + H2O(l) → H3O+(aq) + CH3COO–(aq)
This equation represents the ionization of acetic acid (CH3COOH) into hydronium ions (H3O+) and acetate ions (CH3COO–), forming a weak electrolyte. Acetic acid, a weak acid, only partially dissociates into ions in water.
Therefore, the equation that represents the ionization of a strong electrolyte is:
K3PO4(s) → 3K+(aq) + PO43–(aq)