Chemistry
Making Salts
Making salts involves a chemical reaction between an acid and a base, resulting in the formation of a salt and water. This process is known as neutralization. The salt produced depends on the specific acid and base used. Salts have various practical applications, including as flavor enhancers, preservatives, and in chemical processes.
Written by Perlego with AI-assistance
Related key terms
1 of 5
6 Key excerpts on "Making Salts"
eBook - PDF- Rose Marie O. Mendoza(Author)
- 2023(Publication Date)
- Arcler Press(Publisher)
CHEMISTRY OF SALTS AND AQUEOUS SOLUTIONS 5 CONTENTS 5.1. Introduction .................................................................................... 116 5.2. History of Salt ................................................................................. 117 5.3. Properties of Salt ............................................................................. 118 5.4. Identification of Salts ...................................................................... 119 5.5. Differentiation Between Acidic and Basic Salt................................. 119 5.6. Salts In Aqueous Solutions .............................................................. 119 5.7. Salt–Water Systems in Modern Applications ................................... 122 5.8. Solution Models and Thermodynamic Databases ............................ 125 5.9. Data Sources and Experiments ........................................................ 127 5.10. Formation of Salt Hydrates and Double Salts ................................ 130 5.11. At Enhanced Temperatures the Properties of Salt Solutions ............ 134 5.12. Summary ...................................................................................... 139 References ............................................................................................. 140 CHAPTER The Study of Ions and Salts in Chemistry 116 5.1. INTRODUCTION In chemistry, a salt is defined as a chemical substance that is made up of an ionic assembly of cations and anions, which is defined as follows: As a rule, salts are constituted of a similar number of cations and anions, resulting in a product that is characterized as electrically neutral by the scientific community (without any net charge) (Ladd, 1994). They can be organic, such as acetate (CH 3 CO 2 ), or inorganic, such as chloride (Cl); they can be monatomic, like fluoride or polyatomic, like sulfate (SO 2− 4 ), or a combination of the two types.
- J. A. Beran(Author)
- 2013(Publication Date)
- Wiley(Publisher)
Salts are ionic compounds. If the salt is soluble, then it exists as ions in solution; if the salt is insoluble, then it exists as a solid precipitate. For example, consider two beakers, one containing silver nitrate and the second sodium chloride (Figure 6.4). Both silver nitrate and sodium chloride are soluble and therefore exist in solution as Ag + (aq), and Na + (aq), Cl – (aq) in their respec- tive beakers; no AgNO 3 or NaCl molecules are present! When the two solutions are mixed, a white precipitate of AgCl(s) forms, leaving the Na + (aq) and ions in solution. Therefore, AgCl is considered an insoluble salt and NaNO 3 is a soluble salt in water. A proper equation expressing the two separate solutions, combined solutions, and the observation would then be: (6.9) AgCl(s, white) + Na + (aq) + NO 3 – (aq) —› Ag + (aq) + NO 3 – (aq) + Na + (aq) + Cl – (aq) NO 3 – (aq) NO 3 – (aq) H 2 SO 4 (aq) + 2 NaOH(aq) —› 2 H 2 O(l) + Na 2 SO 4 (aq) CO 3 2– (aq) + H 2 O(l) HCO 3 – (aq) + OH – (aq) NaOH(aq) —› Na + (aq) + OH – (aq) NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH – (aq) Fe(H 2 O) 3+ (aq) + H 2 O(l) FeOH 2+ (aq) + H 3 O + (aq) NH 4 + (aq) + H 2 O(l ) NH 3 (aq) + H 3 O + (aq) 104 Acids, Bases, and Salts Figure 6.1 Phosphoric acid is the additive that delivers the tart taste in many soft drinks. 1 Also called oil of vitriol, sulfuric acid production (number one produced chemical worldwide) exceeds the number two produced chemical (ammonia) by a margin of ~3:1 in the United States annually. For that reason, sulfuric acid is often called the “old horse of chemistry.” Bases Salts Neutralization reaction: a chemical reaction between an acid and a base Hydrated: ions having bonded water molecules are hydrated. Ionic Compounds, Reactions, and Equations Soluble salts are, for this discussion, considered 100% ionized; insoluble salts are 0% ionized. Vincent LaRussa/John Wiley and Sons
eBook - PDF- Stanley E. Manahan(Author)
- 2009(Publication Date)
- CRC Press(Publisher)
212 Fundamentals of Sustainable Chemical Science 212 Fundamentals of Sustainable Chemical Science Sodium chloride dissolved in water is a solution of a Sodium chloride dissolved in water is a solution of a salt salt . A salt is made up of . A salt is made up of a positively charged ion called a a positively charged ion called a cation cation and a negatively charged ion called an and a negatively charged ion called an anion anion . If the water were evaporated, the solid salt made up of cations and anions . If the water were evaporated, the solid salt made up of cations and anions would remain as crystals. A salt is a chemical compound made up of a cation (other would remain as crystals. A salt is a chemical compound made up of a cation (other than H than H ) and an anion (other than OH ) and an anion (other than OH ). ). Amphoteric Substances Amphoteric Substances Some substances, called Some substances, called amphoteric substances amphoteric substances , can act both as an acid and , can act both as an acid and a base. The simplest example is water. Water can split apart to form a hydrogen ion a base. The simplest example is water. Water can split apart to form a hydrogen ion and a hydroxide ion: and a hydroxide ion: H 2 O O Æ H H OH OH (6.2.7) (6.2.7) Since it produces a hydrogen ion, water is an acid. However, the fact that it Since it produces a hydrogen ion, water is an acid. However, the fact that it produces a hydroxide ion also makes it a base. This reaction occurs only to a produces a hydroxide ion also makes it a base. This reaction occurs only to a very small extent. In pure water, only one out of 10 million molecules of water very small extent. In pure water, only one out of 10 million molecules of water is in the form of H is in the form of H and OH and OH .
- Heewon Lee(Author)
- 2014(Publication Date)
- CRC Press(Publisher)
415 Salt Formation of Pharmaceutical Compounds process with sufficient productivity and throughput The acid or base counterion should be miscible with the free base or free acid solution to form a homogeneous solution to allow uniform acid–base reaction to generate the ionic pair species The process must be amenable to the generated salt crystallizing from the solu-tion If the generated salt has a low solubility in the original solvent system in which the free base/acid is dissolved, the salt would naturally crystallize out of the solution promptly as it forms Otherwise, the salt would remain dissolved in the solution Subsequently, the dissolved salt can be crystallized by means of lowering the solubil-ity, such as changing the temperature or solvent composition via antisolvent addition In developing a salt crystallization process, several things must be considered First is the accurate control of the stoichiometric ratio of the acid and base species This is especially important for the salt formation of APIs for which the crystal phase purity and the product pH are critical for ensuring consistent API properties and thus the performance of the drug products The stoichiometry of the salt product may be affected by the accuracy of quantitation of the free acid/base amount in solution and calculation of the proper amount of the counterion to be added Overcharging or undercharging counterions often results in the precipitation of one of the com-ponents and causes an undesired mixture of solid phases The addition mode of the counterion can also have an impact on the purity and quality of the product Too fast an addition or inadequate mixing during the addition of the counterion may easily lead to poor crystallinity or polymorph control of the salt or even new impurities being generated from extreme local pH Other considerations include proper choice of the solvent or
eBook - ePubUnderstanding Basic Chemistry Through Problem Solving
The Learner's Approach
- Kim Seng Chan, Jeanne Tan(Authors)
- 2014(Publication Date)
- WSPC(Publisher)
CHAPTER 8ACIDS, BASES, AND SALTS1.Write the ionic equations, with state symbols, for the following reactions: (a)Barium nitrate solution reacts with sodium sulfate solution to form an insoluble salt and sodium nitrate solution.Explanation:Q Why are some ionic compounds soluble in water while others are not? A:For ionic compounds that are soluble in water, we can say that in general, it is because the attractive forces that are formed between the ions and water molecules are able to provide a sufficient amount of energy to break up the ionic lattice. For those that are insoluble, it is probably due to the insufficient amount of energy supplied to overcome the large strength of ionic bonds. Thus, we can classify salts into soluble salts and insoluble salts:Soluble salts Insoluble salts •Salts containing Na+ , K+ , and NH4 + as cation are soluble. •Salts containing NO3 – as the anion are soluble. •PbCl2 , PbBr2 , PbI2 •Salts containing Cl– , Br– , and I– as the anion are soluble EXCEPT •AgCl, AgBr, AgI •Salts containing SO4 2– as the anion are soluble EXCEPT •PbSO4 , BaSO4 and CaSO4 (sparingly soluble) •Na2 CO3 , K2 CO3 , (NH4 )2 CO3 . •Salts containing CO3 2– as the anion are insoluble EXCEPT Do you know?—To prepare an insoluble salt: Step 1: Mix two solutions together. Step 2: Filter the mixture and collect the residue. Step 3: Wash the residue with deionized water. Step 4: Dry it and you get the salt crystals!(b)Magnesium reacts with dilute hydrochloric acid to form a soluble salt and hydrogen.Explanation:Do you know?—There are three important characteristics that an acid may display: •An acid reacts with a metal to give off hydrogen gas. •An acid reacts with a carbonate/hydrogencarbonate to give off carbon dioxide gas. •An acid reacts with base to give a salt and water.—But not all acids would display all the above three characteristics simultaneously. Some acids may just display one out of the three. For example, water reacts with sodium metal to give off hydrogen gas but does not react with carbonates or with a base.
- Morris Hein, Scott Pattison, Susan Arena, Leo R. Best(Authors)
- 2014(Publication Date)
- Wiley(Publisher)
• They have a slippery feeling. • They change litmus from red to blue. • They interact with acids to form water and a salt. • Arrhenius definition of acids and bases: • Acids contain excess H + ions in aqueous solutions. • Bases contain excess OH - ions in aqueous solutions. • Brønsted–Lowry definition of acids and bases: • Acids are proton donors. • Bases are proton acceptors. • Lewis definition of acids and bases: • Acids are electron pair acceptors. • Bases are electron pair donors. C H A P T E R 1 5 R E V I E W This ancient stone carving on the Burgos Cathedral in northern Spain shows the destructive power of acid rain over time. Mark Boulton/Photo Researchers, Inc. KEY TERM hydronium ion 358 CHAPTER 15 • Acids, Bases, and Salts KEY TERM amphoteric KEY TERMS electrolyte nonelectrolyte dissociation ionization strong electrolyte weak electrolyte 15.2 REACTIONS OF ACIDS AND BASES • Acids react with metals above hydrogen in the activity series to form hydrogen gas and a salt. • Acids react with bases to form water and a salt (neutralization reaction). • Acids react with metal oxides to form water and a salt. • Acids react with carbonates to form water, a salt, and carbon dioxide. • Bases react with acids to form water and a salt (neutralization reaction). • Some amphoteric metals react with NaOH or KOH to form hydrogen and a salt. 15.3 SALTS • Salts can be considered to be derived from the reaction of an acid and a base. • Salts are crystalline and have high melting and boiling points. 15.4 ELECTROLYTES AND NONELECTROLYTES • A substance whose aqueous solution conducts electricity is called an electrolyte: • Aqueous solution contains ions. • A substance whose aqueous solution does not conduct electricity is called a nonelectrolyte: • Aqueous solution contains molecules, not ions. • Dissociation is the process by which the ions of a salt separate as the salt dissolves. • Ionization is the formation of ions that occurs as a result of a chemical reaction with water.
Index pages curate the most relevant extracts from our library of academic textbooks. They’ve been created using an in-house natural language model (NLM), each adding context and meaning to key research topics.
