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Strong Acid and Base Solutions

Acid-Base: An Introduction

Last updated date: 23rd Mar 2023
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Acids are compounds that give out hydrogen ions or a proton when mixed in an aqueous solution and have a pH below 7. These acids generally contain dissociable protons or hydrogen groups, also called acidic hydrogen that readily dissociates in solution or in presence of bases.

Bases are compounds that produce hydroxyl ions when mixed in an aqueous solution. They have a pH above 7. A base, therefore, bears a dissociable hydroxyl group or a basic group that dissociates in an aqueous medium. Bases are also compounds that can steal or accept hydrogen ions, thus, bases can also be defined as compounds which are hydrogen acceptors.

The strength of an acid or base is measured by the pH scale, which indicates its degree of dissociation. A strong acid or a strong base is one which dissociates completely in the aqueous medium furnishing hydrogen or hydroxyl ions in large amounts. The dissociation of acid or base is measured by a dissociation constant. A strong acid or strong base will have a high dissociation constant.

Strong Acid

Strong acids HA have high dissociation due to the presence of highly acidic hydrogens. These hydrogens are usually connected to highly electronegative groups (often halogens like chlorine, fluorine, and iodine). In the solution, the resulting anion after losing a proton is called the Conjugate base of the acid; they are extremely weak bases and therefore, can sustain longer in the solution.

The conjugate base of an acid, the anion, can usually carry a negative charge comfortably due to the high electronegativity of the group or charge stabilisation mechanism.

HA + H2O → H3O+ + A-

Strong acids have low pH. The pH is associated with the concentration of hydrogen ions in a solution. Mathematically, pH is represented as the negative algorithm of the concentration of hydrogen ions.

pH= -log [H+]

Therefore, large hydrogen ion concentration corresponds to low pH value. The concentration of hydrogen ions in a solution is related to what extent the acid dissociates and releases the protons.

The degree of dissociation is accounted for by a parameter Ka called the dissociation constant of acids. A large Ka value indicates higher dissociation and therefore, higher acidity. In chemistry, for convenience pKa value is considered, which is the logarithmic acid dissociation constant, mathematically, represented as the negative logarithm of Ka. So, the high value of acid dissociation constant Ka will correspond to a low pKa and thus, stronger acids will have a small pKa value.

pKa = -log Ka

Some strong acids can be remembered with help of a mnemonic device:

“Chemistry needs preparation sometimes, help!”

Table: Few Examples of Strong Acids

Strong Acids

Hydrochloric Acid, HCl

Sulphuric Acid, H2SO4

Nitric Acid, HNO3

Perchloric Acid, HClO4

Strong Base

Strong bases BOH are compounds that dissociate completely in solution producing large concentrations of hydroxyl ion. Moreover, the bases can be powerful proton acceptors, so in an aqueous solution, they can steal a proton from a water molecule H2O producing an OH- ion.

BOH(aq) → B+ (aq) + OH- (aq)

The conjugate acid of a strong base, i.e., the cation is a weak acid. In an aqueous solution, these cations are solvated by the water molecules surrounding them and the charge is stabilised.

Similar to pH, pOH is associated with hydroxyl ion concentration. Being a negative logarithm of hydroxyl ion concentration, a strong base furnishing large amounts of hydroxyl ion would have low pOH.

pOH= -log [OH-]

The degree of dissociation in the case of bases is captured by the base dissociation constant Kb. The logarithmic base dissociation constant, pKb is similar to pKa and low pKb relates to stronger bases.

pKb = -log Kb

In an aqueous solution pH and pOH is related by the equation:

pH + pOH = 14

Either pH or pOH can be calculated if the other is known. In chemistry, both the strength of acid and base is indicated by the pH scale, where the pH for bases is calculated from the above equation.

Strong acids usually correspond to a pH range 1-2, while strong bases have a pH 13-14. Strong acids and bases both are extremely dangerous and harmful. They are corrosive and cause serious burns on contact.

Table: Few Examples of Strong Bases

Strong Bases

Barium Hydroxide, Ba(OH)2

Calcium Hydroxide, Ca(OH)2

Sodium Hydroxide, NaOH

Potassium Hydroxide, KOH

Lithium Hydroxide, LiOH

Caesium Hydroxide, CsOH

Strontium Hydroxide, Sr(OH)2

Interesting Facts

  • Fluoroantimonic acid is the world’s strongest acid, it is a superacid

  • o-diethynylbenzene dianion is the strongest proton acceptor in the gas phase and can be considered the strongest base in the world, right now.

Key Features

  • Strong acids and Strong Bases dissociate completely in aqueous solution

  • Strong acids produce large concentrations of hydrogen ions in solutions

  • Strong acids have low pH (1-2)

  • Strong bases produce large concentrations of hydroxyl ions in solutions

  • Strong bases high pH (13-14)

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FAQs on Strong Acid and Base Solutions

1. What is the pH in the body?

Human blood has a pH of 7.35 - 7.45, which makes it very slightly alkaline. The human stomach is the most acidic part of the body with a pH of 1.5 - 3.5. The low pH in the stomach is maintained for degrading food items for digestion purposes and killing any unwanted germs.

2. What are superacids?

Superacids are basically classified as those acids which have acidity higher than 100% sulphuric acid. Some commercially available superacids are trifluoromethanesulphonic acid (CF3SO3H) and fluorosulphuric acid (HSO3F).

3. What are superbases?

According to IUPAC, superbases are defined as a “compound having a very high basicity, such as lithium diisopropylamide.”