Problems with the preparation of sodium barbital buffer
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I saw a method for preparing a buffer using sodium barbital and hydrochloric acid. I would like to ask: if I replace hydrochloric acid with nitric acid of the same concentration, and use sodium barbital and nitric acid to prepare a buffer, will the properties of the resulting solution be the same as those of the solution prepared using hydrochloric acid? That is, pH value, buffering capacity, etc. If one wants to minimize the degree of impurities introduced by acids, which is better, hydrochloric acid or nitric acid (assuming both are of analytical grade)?
When preparing this buffer, hydrochloric acid cannot be replaced with nitric acid, as nitric acid is a strong oxidizing acid that will rapidly oxidize the organic substances present in the solution, thereby causing the sodium barbiturate to be oxidized and become ineffective. This buffer can only be prepared using hydrochloric acid; if a substitute is needed, phosphoric acid or dilute sulfuric acid might work.
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Hmm, I see. Thank you for your answer. As for hydrochloric acid, if it is of high purity, analytical grade, is the amount of metal impurities in such a hydrochloric acid solution high? Are there any methods to further improve the purity of hydrochloric acid?
The packaging of hydrochloric acid products always indicates the impurity content, so you can refer to that. As for further increasing the purity of hydrochloric acid, it is necessary to determine which purification method is most suitable based on the characteristics of the raw materials and the desired product. There are methods available, but it’s impossible to determine which one is suitable for you. If you have the money, you can simply purchase electronic-grade products.