Final answer:
A 1 M solution of CaCl2 is a stronger electrolyte than 1 M NaCl because it produces a higher total ion concentration, with CaCl2 dissociating into three ions (one Ca2+ and two Cl-) and NaCl into two ions (one Na+ and one Cl-). Doubly charged ions like Ca2+ also conduct more current than singly charged ions, contributing to the higher electrolytic strength of CaCl2.
Step-by-step explanation:
A 1 M solution of CaCl2 is considered a stronger electrolyte than 1 M NaCl because when CaCl2 dissolves in water, it dissociates into three ions (one Ca2+ and two Cl−), thereby leading to a higher total ion concentration in the solution. In contrast, NaCl dissociates into two ions (one Na+ and one Cl−).
The strength of an electrolyte is often associated with both the number of ions it provides in solution and the charge of these ions. Therefore, CaCl2, which produces more ions with higher charges, results in a higher concentration of ions and is thus a stronger electrolyte.
In addition, ions that are doubly charged, like Ca2+, carry twice as much current through the solution compared to singly charged ions such as Na+. This difference in charge contributes to the stronger electrolytic behavior of CaCl2. The concentration of individual ions in a solution is also significant; for a 1 M solution of NaCl, the concentration of Na+ and Cl− ions is 1 M each, but in a 1 M solution of CaCl2, the concentration of Cl− ions is 2 M, further highlighting why CaCl2 is a stronger electrolyte.