Examples of acid salt in the following topics:
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- When dissolved in water, acidic salts form solutions with pH less than 7.0.
- When dissolved in water, acidic salts will yield solutions with pH less than 7.0.
- Acid salts can also contain an acidic proton in the anion.
- Anilinium chloride is an example of an acid salt.
- Explain the formation of acid salts and their effects on a solution's pH.
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- Basic salts form from the neutralization of a strong base and a weak acid; for instance, the reaction of sodium hydroxide (a strong base) with acetic acid (a weak acid) will yield water and sodium acetate.
- Acid salts are the converse of basic salts; they are formed in the neutralization reaction between a strong acid and a weak base.
- The conjugate acid of the weak base makes the salt acidic.
- The ammonium ion contains a hydrolyzable proton, which makes it an acid salt.
- This video examines the hydrolysis of an acid salt, a basic salt, and a salt in which both ions hydrolyze.
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- Because of their enhanced acidity, carboxylic acids react with bases to form ionic salts, as shown in the following equations.
- In the case of alkali metal hydroxides and simple amines (or ammonia) the resulting salts have pronounced ionic character and are usually soluble in water.
- Heavy metals such as silver, mercury and lead form salts having more covalent character (3rd example), and the water solubility is reduced, especially for acids composed of four or more carbon atoms.
- Carboxylic acids and salts having alkyl chains longer than six carbons exhibit unusual behavior in water due to the presence of both hydrophilic (CO2) and hydrophobic (alkyl) regions in the same molecule.
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- In acid-base chemistry, a salt is defined as the ionic compound that results from a neutralization reaction between an acid and a base.
- There are several varieties of salts, and in this section we will consider basic salts.
- What makes a basic salt basic?
- It is due to the fact that the anion in the salt is the conjugate base of a weak acid.
- Keep in mind that a salt will only be basic if it contains the conjugate base of a weak acid.
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- A common method of resolving racemates is by diastereomeric salt formation with a pure chiral acid or base.
- In the initial display, the carboxylic acid function contributes to diastereomeric salt formation.
- Next, an ammonium salt is formed by combining the carboxylic acid with an optically pure amine, such as brucine (a relative of strychnine).
- Since the amino acid moiety is racemic and the base is a single enantiomer (levorotatory in this example), an equimolar mixture of diastereomeric salts is formed (drawn in the green shaded box).
- Finally the salt is broken by acid treatment, giving the resolved (+)-amino acid derivative together with the recovered resolving agent (the optically active amine).
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- Acids and bases will neutralize one another to form liquid water and a salt.
- Common examples of acids include acetic acid (in vinegar), sulfuric acid (used in car batteries), and tartaric acid (used in baking).
- sulfuric acid (H2SO4; only the first proton is considered strongly acidic)
- Stronger acids have a larger Ka and a more negative pKa than weaker acids.
- Acids and bases react with one another to yield water and a salt.
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- Carboxylic acids are organic acids that contain a carbon atom that participates in both a hydroxyl and a carbonyl functional group.
- As proton donors, carboxylic acids are characterized as Brønsted-Lowry acids.
- Salts and esters of carboxylic acids are called carboxylates.
- Generally, in IUPAC nomenclature, carboxylic acids have an "-oic acid" suffix, although "-ic acid" is the suffix most commonly used.
- Upon exposure to a base, the carboxylic acid is deprotonated and forms a carboxylate salt.
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- Most base reagents are alkoxide salts, amines or amide salts.
- Since alcohols are much stronger acids than amines, their conjugate bases are weaker than amide bases, and fill the gap in base strength between amines and amide salts.
- In the following table, pKa again refers to the conjugate acid of the base drawn above it.
- Pyridine is commonly used as an acid scavenger in reactions that produce mineral acid co-products.
- Finally, the two amide bases see widespread use in generating enolate bases from carbonyl compounds and other weak carbon acids.
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- Natural fatty acids may be saturated or unsaturated, and as the following data indicate, the saturated acids have higher melting points than unsaturated acids of corresponding size.
- The trans-double bond isomer of oleic acid, known as elaidic acid, has a linear shape and a melting point of 45 ºC (32 ºC higher than its cis isomer).
- Because of their enhanced acidity, carboxylic acids react with bases to form ionic salts, as shown in the following equations.
- In the case of alkali metal hydroxides and simple amines (or ammonia) the resulting salts have pronounced ionic character and are usually soluble in water.
- Heavy metals such as silver, mercury and lead form salts having more covalent character (3rd example), and the water solubility is reduced, especially for acids composed of four or more carbon atoms.
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- Lewis bases are electron-pair donors, whereas Lewis acids are electron-pair acceptors.
- A Lewis base, therefore, is any species that donates a pair of electrons to a Lewis acid.
- We have previously described this as an acid-base neutralization reaction in which water and a salt are formed.
- Thus, in this version of the neutralization reaction, what interests us is not the salt that forms, but the covalent bond that forms between OH- and H+ to form water.
- This lesson continues to describe acids and bases according to their definition.