What to eat to replenish electrolytes

If you want to replenish electrolytes, there are actually many foods that can achieve this goal, but most people still choose to inject glucose. This is indeed the most intuitive method of supplementation at present. However, consuming some fresh vegetables and fruits in daily life can also achieve the same effect. There is no need to deliberately eat some foods that are very nutritious.

In the acute phase, it can generally be calculated according to the basal metabolic requirements, that is, 50-60 ml/kg·d of 5%-10% glucose, 1-2 mmol/kg·d of sodium and potassium each (10 ml of normal saline contains 1.5 mmol of sodium, and 10 ml of 10% potassium chloride solution contains 13 mmol of potassium), or 60-75 g/m2 of sugar and 50-70 mmol/m2 of sodium and potassium each given at 1500 mL/m2 of body surface area. Physiological needs can also be supplemented with a 3:1 solution. During hypertonic dehydration, the posterior pituitary gland secretes antidiuretic hormone, which promotes water absorption in the distal renal tubules. Therefore, some people believe that during hypertonic dehydration, the physiological requirements should be reduced by 1/4.

Electrolytes are compounds that can conduct electricity when dissolved in aqueous solution or in a molten state. According to their degree of ionization, they can be divided into strong electrolytes and weak electrolytes. Strong electrolytes are almost completely ionized, while weak electrolytes are only partially ionized.

Electrolytes are substances that are bound together by ionic bonds or polar covalent bonds. Compounds can dissociate into freely mobile ions when dissolved in water or heated. Ionic compounds can conduct electricity in aqueous solution or in the melt; some covalent compounds can also conduct electricity in aqueous solution, but there are also solid electrolytes whose conductivity comes from the migration of ions in the crystal lattice.

Electrolysis of water: the cathode in the electrolytic cell is an iron plate, the anode is a nickel plate, and the electrolyte is a sodium hydroxide solution. When power is applied, under the action of the external electric field, the positive and negative ions in the electrolyte migrate to the cathode and anode respectively, and the ions undergo electrochemical reactions at the electrode-solution interface. An oxidation reaction takes place at the anode, and a reduction reaction takes place at the cathode.

The electrolysis of water is the decomposition of water into H2(g) and O2(g) under the action of an external electric field. Electrolysis is a very powerful means of promoting redox reactions. Many redox reactions that are difficult to carry out can be achieved through electrolysis. For example, molten fluoride can be oxidized to elemental fluorine at the anode, and molten lithium salt can be reduced to metallic lithium at the cathode.