What is the acidity value that turns sodium carbonate into a carbon dioxide tower?
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This post was last edited by Yinuo Zhang on 2012-5-29 10:07 The existing sodium carbonate solution has a sodium carbonate concentration of about 0.5g/L. Add hydrochloric acid dropwise to it. Please tell me.: How long does it take to adjust the content of hydrochloric acid to turn sodium carbonate into a dioxide tower, and the solution no longer contains sodium carbonate? Adjust the pH value of the solution to 3, 2, 1, or adjust the hydrogen ion concentration to 1mol/L, 2mol/L, 3mol/L... At what time is it feasible? Please give me your advice.
This post was last edited by qugd on 2012-5-31 22:33 The acidity of sodium carbonate solution acidified and decomposed is not a fixed value, but a range, and it is relatively wide. In addition, the range of acidolysis is also affected by temperature and the concentration of sodium carbonate. Through the secondary ionization process of carbonic acid, the approximate acidolysis concentration can be calculated, but it is also more complicated to calculate the concentration of acid when carbon dioxide escapes, or the pH value. The poster can refer to the figure below to see the relationship between different forms of carbonic acid and pH. From the figure, it can be roughly seen that when the pH value is less than 8, free carbon dioxide may exist, but whether it can escape is related to the temperature and the total concentration of the system. One thing that is certain is that when the free acid (hydrogen ions) added to the system reaches half the number of moles of sodium carbonate, if there is an excess of one drop of acid, carbon dioxide may be generated. The pH value at this time is about 8.3 ~ 8.4. http://jpkc.ncwu.edu.cn/sfxhx/shouke/yemian/tansuan.jpg