What is the difference between a strong electrolyte and a weak electrolyte? Explain what makes an electrolytic solution strong or weak.
Do you look at the pH to determine between a strong electrolyte and a weak one?
No. A strong electrolyte, by definition, is one that ionizes 100%; i.e., AB becomes A ions and B ions and there are NO AB molecules floating around in the solution.
A weak electrolyte, by definition, is one that ionizes less than 100%; i.e., AB becomes some A ions, some B ions (the number depends upon the percent ionization) and there are still some AB molecules floating around in the solution along with the ions.
Students often get confused by this terminology. They often equate a strong acid, for example, as one that eats a hole in the flesh or in clothes but that isn't true. We can have a dilute solution of a strong acid or a concentrated solution of a weak acid. Strong and weak acids, bases, and electrolytes, all follow this same terminology.
To understand the difference between a strong electrolyte and a weak electrolyte, let's first discuss what an electrolyte is. An electrolyte is a substance that, when dissolved in water or melted, produces ions that can conduct electricity. These ions are formed when the substance dissociates into positive and negative ions.
A strong electrolyte is a substance that completely dissociates into ions when dissolved in water. This means that nearly all of the molecules of the substance break apart into positive and negative ions. As a result, a strong electrolytic solution conducts electricity efficiently because it has a high concentration of ions that are free to move and carry electric charge.
On the other hand, a weak electrolyte is a substance that only partially dissociates into ions when dissolved in water. In this case, only a small fraction of the molecules break apart into ions while the majority remains in the molecular form. Consequently, a weak electrolytic solution conducts electricity less efficiently since it has a lower concentration of ions available for conducting electricity.
The strength of an electrolyte can be influenced by factors such as temperature and concentration. Generally, compounds that are ionic (composed of positive and negative ions) tend to be strong electrolytes, while compounds that are covalent (composed of molecules held together by shared electrons) tend to be weak electrolytes. However, this is not always the case, as certain covalent compounds can also exhibit some degree of ionization.
To determine whether a substance is a strong electrolyte or a weak electrolyte, it is not necessary to look at the pH. pH is a measure of the hydrogen ion concentration in a solution, which is specifically related to the acidity or alkalinity of the solution. Electrolytic strength, on the other hand, refers to the degree of ionization of a substance and is unrelated to pH.
The strength of an electrolyte can be experimentally determined by observing its conductivity or measuring its ability to carry electric current. A substance that conducts electricity effectively is likely to be a strong electrolyte, whereas a substance with poor conductivity is more likely to be a weak electrolyte or a non-electrolyte that does not dissociate into ions.
In summary, the difference between a strong electrolyte and a weak electrolyte lies in their degree of ionization when dissolved in water. Strong electrolytes fully dissociate into ions, while weak electrolytes only partially dissociate. The pH of a solution is not directly indicative of its electrolytic strength.