Chemistry 122 d

Question

Briefly explain why an aqueous solution of calcium chloride would be considered an electrolyte but and aqueous solution of glucose (C6H12O6) would not. How would they behave differently in an electrical circuit as described in class?

Answer 1

Hi Bailey,

the question asks why CaCl2 (calcium chloride) in an aqueous solution is considered an electrolyte but C6H12O6 (glucose) in an aqueous solution is not an electrolyte? In an electrical circuit how would they behave differently?

A electrolyte is a compound that ionizes, breaks up into its respective ions in water and thus will conduct electricity through water when connected to an electric circuit.

When calcium chloride dissolves in water it breaks up into its respective ions, ( charged particles) one mole of CaCl2 breaks up into one mole of a Ca+2 ion and 2 moles of Cl-1 ions thus it is a strong electrolyte and will conduct electricity when dissolved in water.

CaCl2(aq) >>>> Ca+2 +. 2Cl-1

Glucose will not ionize that is break apart into ions (charged particles) thus it is not an electrolyte and will not conduct an electric current in water, but will dissolve in water because of the -OH group incorporated in the molecule meaning it has a strong hydrogen bond just like the hydrogen bonds in water (H2O)

Note: hydrogen bonds form when hydrogen combines with oxygen as seen above in glucose and water, as well as when hydrogen combines with nitrogen and fluorine. These hydrogen bonds have very

strong intermolecular forces permitting intermolecular bonding to develop between water and glucose making it water soluble.

The second part of the question asks how CaCl2 and glucose will behave differently in an electric circuit?

CaCl2 being a strong electrolyte as mentioned above will easily conduct an electric current when dissolved in water and connected to an electric circuit, while glucose not being an electrolyte will not conduct an electric current when dissolved in water and when connected to an electric circuit.