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.
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)
2 answers
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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6 answers