Electrolytes are easier for the body to absorb for nutritional value than salts. Essentially, salts are just salts, while electrolytes are salts plus more, such as potassium.
A solution of salt (NaCl) is an electrolyte.
no, a calcium salt is an electrolyte
Table salt is an electrolyte due to its ionic bonding. It will completely dissolve in aqueous solutions and is capable of conducting electricity.
The electrolyte of a commercial galvanic cell normally extends from anode to cathode without interruption by a salt bridge. A salt bridge is normally a teaching tool to help show that: 1. Galvanic half-cells do not produce voltage 2. Conductors and insulators are not necessarily salt bridges. An electrolyte must extend from anode to cathode before the galvanic cell can produce voltage. 3. The chemical composition of the salt bridge can differ from the electrolytes in the half cells. 4. Ions travel through the salt bridge between the cell's anode and cathode. Salt bridges raise more questions than answers. For example: 1. Can the difference between an electrolyte and a conductor be defined? 2. How do ions quickly move through a solid or a long electrolyte? 3. When salt bridge composition differs from the galvanic cell electrolyte(s), must the salt bridge chemically react with the galvanic cell electrolyte(s)? 4. Why does galvanic cell voltage remain nearly constant while anode to cathode distance doubles.
An electrolyte.
molecules
A solution of salt (NaCl) is an electrolyte.
Since salt is an electrolyte, yes, it does cook faster, but it's not that much of a difference.
electrolyte
no, a calcium salt is an electrolyte
A salt solution is an electrolyte.
Table salt is an electrolyte due to its ionic bonding. It will completely dissolve in aqueous solutions and is capable of conducting electricity.
Salt (sodium chloride) is an electrolyte in water solutions or when is melted. Glucose is not an electrolyte.
The salt would be an electrolyte.
Electrolyte. sulphuric acid
The electrolyte of a commercial galvanic cell normally extends from anode to cathode without interruption by a salt bridge. A salt bridge is normally a teaching tool to help show that: 1. Galvanic half-cells do not produce voltage 2. Conductors and insulators are not necessarily salt bridges. An electrolyte must extend from anode to cathode before the galvanic cell can produce voltage. 3. The chemical composition of the salt bridge can differ from the electrolytes in the half cells. 4. Ions travel through the salt bridge between the cell's anode and cathode. Salt bridges raise more questions than answers. For example: 1. Can the difference between an electrolyte and a conductor be defined? 2. How do ions quickly move through a solid or a long electrolyte? 3. When salt bridge composition differs from the galvanic cell electrolyte(s), must the salt bridge chemically react with the galvanic cell electrolyte(s)? 4. Why does galvanic cell voltage remain nearly constant while anode to cathode distance doubles.
Dissolved or (melted) sodium chloride is an electrolyte.