Sodium Bisulfate - NaHSO₄

Sodium Bisulfate, with the molecular formula \[(NaHSO_{4})\], is the sodium salt of the bisulfate anion. It is an acid kind of salt that is formed by partial neutralization of sulfuric acid by an equivalent of sodium base. It is typically in the form of either sodium hydroxide (lye) or sodium chloride. Sodium bisulfate is produced as a median in the Mannheim process. Mannheim is an industrial process involving the reaction of sodium chloride and sulfuric acid: \[NaCl + H_{2}SO_{4} \rightarrow  HCl + NaHSO_{4}\]. It is highly toxic to certain echinoderms but impartially harmless to most other life forms; so it is used in controlling outbreaks of crown-of-thorns starfish.

Properties of Sodium Bisulfate \[(NaHSO_{4})\]

There are two different properties of sodium bisulphate \[(NaHSO_{4})\] 

Physical Properties of Sodium Bisulfate \[(NaHSO_{4})\]

Sodium bisulfate \[(NaHSO_{4})\] is commonly available in both anhydrous (dry) and monohydrate \[(NaHSO_{4}.H_{2}O)\] forms. Anhydrous \[(NaHSO_{4})\] is a shapeless and hygroscopic white powder, having a density of 2.74 g/mL and a melting point of 315 °C. The monohydrate is a white sandy solid having a density of 1.8 g/mL and a melting point of 59 °C. It is considered a dry acid that is suitable for safe shipping and storage as well.

Chemical Properties of Sodium Bisulfate \[(NaHSO_{4})\]

Sodium bisulfate \[(NaHSO_{4})\] is highly water-soluble. It is not a typical neutral salt but chemically an acidic salt, due to the substitution of only one acidic proton of the diprotic sulfuric acid. Aqueous solutions of \[(NaHSO_{4})\] are highly acidic. It reacts powerfully with strong bases and potent oxidizing agents. It is perfectly steady under normal conditions but decomposes upon exposure to water.

Uses of \[(NaHSO_{4})\]

We have listed a few uses of \[(NaHSO_{4})\] sodium bisulfate below:

Sodium bisulfate is often used as a preservative, in meat processing, food additives, drugs, and dietary supplements. Uses of sodium bisulfate are also extended in pH control, household cleaning products, leather tanning, disinfecting, swimming pools, metal cleaning, and many other applications. Sodium bisulfate was once an essential active ingredient in the toilet bowl cleaners Vanish and Sani-Flush, but now both are discontinued.

1. Sodium bisulfate is used in lowering the pH of water in swimming pools.

2. Used in metal finishing.

3. Used in the chicken house to reduce the concentration of Salmonella.

4. Used as a bleaching agent.

5. Used as a catalyst.

6. Used in the manufacturing of paper products.

7. Used in water treatment products.

8. Used in paints.

9. Used in agricultural chemicals.

10. Used in velvet cloths.

Chemical Reactions of Sodium Bisulfate

The hydrated sodium bisulfate first dehydrates and then separates from the water molecule which is attached to it at 60°C temperature. It is allowed to cool. Heating it to 290 °C produces sodium pyrosulfate which is nothing but an absolute colorless salt:

\[ 2 NaHSO_{4} \rightarrow  Na_{2}S_{2}O_{7} + H_{2}O \]

What is Bisulfate?

Bisulfate is a liquid solution consisting of a white crystalline solid dissolved in water. It is corrosive to metals and tissue. Bisulfate is an ester or salt of sulphuric acid which contains – \[ HSO_{4} \] or the ion \[ HSO_{4} \] –, the monovalent group (which is a modifier) consisting of, containing, or concerned with the group:

– \[ HSO_{4} \] or the ion \[ HSO_{4} \]

Solved Problem

Question: How is Sodium Bisulfate Made?

Solution: Sodium bisulfate is formed or made as a median in the Mannheim process. It is an industrial process involving the reaction of sodium chloride and sulfuric acid:

\[ NaCl + H_{2}SO_{4} \rightarrow  HCl + NaHSO_{4} \]

The liquid sodium bisulfate is sprayed and cooled to help it form a solid bead. The hydrogen chloride gas is dissolved in H_{2}O (water) to form hydrochloric acid. Sodium bisulfate if not for economical interest but can be given rise as an outgrowth of the production of many different mineral acids through the reaction of their sodium salts with more sulfuric acid:

\[ NaX + H_{2}SO_{4} \rightarrow  NaHSO_{4} + HX  \]

Question: How do you neutralize Sodium Bisulphate?

Solution: Sodium bisulfate is not very toxic to the environment if in small quantities, though it should be neutralized first before disposal. We can use a base like sodium carbonate or bicarbonate in an aqueous solution.

Studying the Sodium Bisulfate \[(NaHSO_{4})\] – Properties, Uses, Chemical Reactions, and Solved Problem

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Importance of learning the Sodium Bisulfate \[(NaHSO_{4})\] – Properties, Uses, Chemical Reactions, and Solved Problem 

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