Effect of distilled water pH on the pH of the solution being measured
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For the convenience of companies, our company produces and sells *AO acid AN solutions. However, the customers have strict requirements regarding the pH value of these solutions, which generally needs to be kept between 5 and 6. I would like to ask: when measuring the pH value of a 10% *AO acid AN aqueous solution, what impact does the pH value of distilled water have on the pH value of the *AO acid AN solution? If the solution is acidic, distilled water is alkaline, and if the solution is alkaline, distilled water is acidic – are the results of these two measurements accurate? Is there any error, and how can it be avoided? Looking forward to your reply! ! !
The impact must be minimal! Even if distilled water is alkaline, the degree of alkalinity is very low, unless the distilled water has gone bad! You can test one group with distilled water and another without it to see the difference! The results should be quite close, right! Personal opinion! This post was last edited by zjs0536 on 2009-3-11 21:12.]
I’m not quite sure – are you using distilled water for comparison, or to prepare nitric acid solutions, or to prepare pH standard solutions? Can an *ao acid solution also be basic?
If the distilled water has not deteriorated, its pH value is essentially neutral. It will not affect the pH value of *ao acid an. It is difficult to accurately measure the pH value of distilled water; in experiments, conductivity is commonly used to determine the purity of distilled water. *AO acid AN is a salt of a strong acid and a weak base; it exhibits acidity after hydrolysis. If the solution is alkaline, consider whether there is an issue with the purity of the drug.
Distilled water prepared normally has a pH close to neutral, and it does not affect pH measurements. It is recommended that you first measure the pH value of your distilled water. And then draw a conclusion.