Topics in ChemistrySalts and Types of Salt in Chemistry Mixtures and Separation of Mixtures Separation of Mixtures part 2 Separation of Mixtures part 3 Physical Change, Chemical Change, Element, Compound and Mixture Electrolysis, Electrolyte, Electrode, Anode and Cathode Grahams law of diffusion Physical Properties of Metals Daltons Atomic Theory and its Modifications Periodic table and Classification of Elements
Academic Questions in Chemistry
The reaction involving an acid and a base is termed _____.
Which of the following is NOT a type of salt?
The only metal that exist as liquid at room temperature is _____.
Almost everyone would have used the word “salt” when it comes to cooking. This ‘cooking’ salt or better still table salt or common salt is just one of the many salts we have in chemistry.
Chemically, this table salt or common salt is referred to as Sodium Chloride
Sodium chloride has the chemical symbol "NaCl"
Note: NaCl is naturally present in sea water; and they often give rise to the salt water habitat which happens to be home to some organisms.
Generally, a salt can be defined as a compound/substance composed of a positive metallic ion and a negative non metallic ion.
For instance, Na ion (Na+) is a positive metallic ion while chlorine ion (Cl-) is a negative non metallic ion. NaCl is therefore a salt based on our definition.
In the laboratory, salts can be prepared in a variety of ways and as a result, salts are of different types.
Note: The ideal definition of a salt will be based on how the salt was formed. This implies that we will have different definition for salts (based on how they are produced).
A normal salt is formed from an acid and a base. It is electrically neutral.
By definition, a normal salt is the product formed when an acid react with a base.
The acid and the base must be of equal strength; for instance, a strong acid reacting with a strong base.
Note: This reaction involving an acid and a base is known as neutralization reaction. The other product formed from neutralization reaction is water (H2O).
Recall that an acid will always have hydrogen ion as its only positive ion; so for a normal salt to be formed, all the hydrogen ions must be replaced by the metal from the base.
Note: A base will always have hydroxide ion (OH-) as its only negative ion.
The equation below shows the formation of a normal salt.
Notice that the hydrogen ion (H+) from the acid reacts with the hydroxide ion (OH-) from the base to form water (H2O) while the metallic ion (Na+) replaced the hydrogen in (HCl acid) to form NaCl. For this reason, the normal salt is electrically neutral.
For an acid salt to be formed, only a part of the hydrogen ions in the acid is replaced; and as a result, hydrogen ion is always present in an acid salt. In fact, it is presence of hydrogen ion (H+) in the salt that makes it an acid salt.
Note: The acid required to form an acid salt must have a basicity greater than one.
The basicity of an acid is the number of replaceable hydrogen ion(s) in one molecule of the acid.
For instance, Hydrochloric acid (HCl) is monobasic since it only one replaceable hydrogen within it.
Hydrogen tetraoxosulphate(VI) acid (H2SO4) is dibasic since it has two replaceable hydrogen ions within its molecule.
From our explanation above; it is quite clear that HCl will not be able to form an acidic salt since it’s monobasic. H2SO4 on the other hand will form an acid salt since it is dibasic.
H2SO4(aq) + NaOH(aq) -> NaHSO4(s) + H2O(l)
Note: One of the hydrogen ions from the acid H2SO4 had been replaced by Sodium (Na).
Unlike an acid salt which contains hydrogen ion (H+) within it, a basic salt contains hydroxide ion (OH-) within it.
A basic salt will always contain the positive metal ion from the base, hydroxide ion from the base and the negative ion from the acid.
Note: When a strong base reacts with a weak acid, a basic salt is formed. Also, when the concentration of a base is much higher than the acid, a basic salt will also be formed.
Examples of basic salts are ZnOHCl and MgOHCl
A double salt is one that ionizes to produce three different types of ions is solution, out of which two are positively charged while one is negatively charged.
Examples of double salts are [Aluminium Potassium tetraoxosulphate(VI) dodecahydrate] or KAl(SO4)2.12H2O and [Ammonium Iron(II) tetraoxosulphate(VI) hexahydrate] or (NH4)2 Fe(SO4)2.6H2O.
Notice that if KAl(SO4)2.12H2O was dissolved in water, The ions produced will be: Potassium ion (K+) which is positively charged, Aluminium ion (Al3+) which is positively charged and sulphate ion (SO42-) which is negatively charged.
Similarly, (NH4)2 Fe(SO4)2.6H2O will ionize to produce Ammonium ion (NH4+), Iron (II) ion (Fe2+) and sulphate ion (SO42-) respectively.
Any salt that contains complex ions within it is regarded as a complex salt.
For now, just imagine complex ions to consist of a charged group of atoms.
An example of a complex salt is Sodium tetrahydroxozincate(II) or Na2Zn(OH)4. If this complex salt is dissolved in water, sodium ions (Na+) and Zinc hydroxide ions Zn(OH)2- will be produced respectively. It is the presence of Zn(OH)2- that makes this salt a complex salt.
Another example of a complex salt is Potassium hexacyanoferrate(II) or K4Fe(CN)6 which ionizes to produce potassium ion (K+) and [Fe(CN)6]4- respectively. It is the presence of [Fe(CN)6]4- that makes K4Fe(CN)6 a complex salt.
Mg(s) + 2HNO3(aq) -> Mg(NO3)2(s) + H2(g)
Mg(NO3)2 is the salt formed from the above reaction. This salt qualifies as a normal salt.
2HCl(aq) + Na2CO3(s) -> 2NaCl(s) + H2O(l) + CO2(g)
Alfred Ajibola is a Medical Biochemist, a passionate Academician with over 7 years of experience, a Versatile Writer, a Web Developer, a Cisco Certified Network Associate and a Cisco CyberOps Associate.
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