Why use nahco3 instead of naoh

In this way, they can be extracted from an organic layer into an aqueous layer. As previously discussed, carboxylic acids can be extracted from an organic layer into an aqueous layer by shaking them with basic solutions, which converts them into their more water-soluble salts. Therefore, a solution of bicarbonate can be used to separate mixtures of phenols and carboxylic acids Figure 4. The acid-base properties previously discussed allow for a mixture containing acidic e.

It is assumed that readers conducting this type of experiment are familiar with performing single and multiple extractions. In this section are described differences between general extraction procedures and the process as summarized in Figure 4. Lisa Nichols Butte Community College. Complete text is available online. How They Work A modification of the extractions previously discussed in this chapter is to perform a chemical reaction in the separatory funnel in order to change the polarity and therefore partitioning of a compound in the aqueous and organic layers.

Figure 4. Sodium Bicarbonate Washes An acid-base extraction can be used to extract carboxylic acids from the organic layer into the aqueous layer.

The ester is then isolated in the organic layer. Mixtures of Acids and Bases As has been discussed previously, the acid-base properties of compounds can be utilized to selectively extract certain compounds from mixtures. This strategy can be extended to other examples Extracting Bases Basic compounds such as amines can be extracted from organic solutions by shaking them with acidic solutions to convert them into more water-soluble salts.

Extracting Carboxylic Acids vs. Phenols As previously discussed, carboxylic acids can be extracted from an organic layer into an aqueous layer by shaking them with basic solutions, which converts them into their more water-soluble salts. Extracting Acid, Base, and Neutral Compounds The acid-base properties previously discussed allow for a mixture containing acidic e. After acidification, two routs may be taken, depending on if the acidic component is solid or liquid.

If a solid forms upon acidification of the ionic salt, it can be collected through suction filtration. This method should only be used if large quantities of large-sized crystals are seen. If fine crystals form which are quite common , they will clog the filter paper and interfere with adequate drainage. If only a small amount of solid is seen compared to the theoretical quantity, it is likely the compound is quite water-soluble, and filtration would lead to low recovery.

Sodium hydroxide and sodium carbonate are derivatives of the alkali metal sodium, atomic number 11 on the Periodic Table of Elements. Both sodium hydroxide and sodium carbonate have commercial importance. The two are unique and have different classifications; however, sometimes they are used interchangeably.

Sodium hydroxide is considered to be a simple base, whereas sodium carbonate is considered to be a salt of the weak acid, carbonic acid. If sodium hydroxide and sodium carbonate can used interchangeably, it may be advisable to use the carbonate because it is less hazardous.

Reacted with acids stronger than carbonic acid, both produce the same salt. Washing soda refers to its laundry use. Sodium hydroxide is too alkaline for such an application.

Sodium carbonate is also used in water treatment and in the manufacture of glass. He furthered his education through the University of Virginia's Citizen Scholar Program program, taking many courses in organic and quantum chemistry. He has written technical articles since Sodium Carbonate.