what reaction do you get when adding 3 tespoons of Na2S2O3 to 50
ml of boiling water
To determine the reaction that occurs when adding 3 teaspoons of Na2S2O3 (sodium thiosulfate) to 50 ml of boiling water, you first need to understand the properties of these substances.
Na2S2O3 is a white crystalline solid that is commonly used as a reducing agent and is soluble in water. When it dissolves in water, it dissociates into sodium ions (Na+) and thiosulfate ions (S2O3²-).
Water, on the other hand, is a polar molecule. When it is heated to its boiling point, it undergoes a phase change from a liquid to a gas. Boiling water molecules have increased kinetic energy and move more rapidly than at lower temperatures.
When you add 3 teaspoons of Na2S2O3 to 50 ml of boiling water, the following reaction occurs:
Na2S2O3 (s) + H2O (l) -> Na+ (aq) + S2O3²- (aq)
In this reaction, the solid Na2S2O3 dissolves in the liquid water, forming sodium ions (Na+) and thiosulfate ions (S2O3²-) in the aqueous solution.
It is worth noting that the reaction might be exothermic, meaning that it releases heat due to the dissolution process. However, the reaction itself does not involve any observable physical changes or production of gases or precipitates, as the ions formed simply remain dissolved in the water.
If you are conducting an experiment or investigating the effects of adding Na2S2O3 to boiling water, it would be helpful to clarify the purpose or desired outcome, as it is unclear from the provided information.