Acid and Alkali Game Quiz Online
Acids are a group of chemicals that contain a H= ion examples of which are vinegar, Hydrochloric acid, and Sulphuric acid. Alkalis are a group of chemicals that contain the OH= ion an example is Sodium Hydroxide. To understand how acid and alkali are different, you must know what water is made up of. Water molecules have the chemical formula H2O, which splits into two different ions. In a neutral solution, the concentration of hydrogen ions and hydroxide ions is equal. When acid and alkali are added, the concentration of hydrogen ions is increased while hydroxide ions are reduced. This is the process of a reaction known as acidification.
Arrhenius
The difference between acid and base is a matter of definition. Arrhenius theory defines an acid as a substance that donates a proton to a water molecule. However, this theory cannot explain acidity and basic behavior of compounds. The Bronsted-Lowry theory expands this theory to explain acid and base behavior in insoluble solutions. Hence, the Arrhenius theory does not apply to all kinds of compounds.
A weak acid, on the other hand, does not release hydrogen ions. Instead, it exists as an equilibrium mixture of hydrogen and oxygen-containing molecules. Such acid has a high pH value, but the dissociation constant is lower. This makes Arrhenius' acid-base theory the most limited. It requires a compound to have a hydrogen ion or a hydroxyl group in addition to being soluble in water. As a result, acid and base compounds cannot be classified as acids or bases unless they contain a hydrogen ion.
Bronsted-Lowry
The Bronsted-Lowry acid and base theory states that an acid donates a proton to a base and the latter accepts it. The result is a conjugate acid and base. Both acids and bases are composed of hydrogen and act as proton donors and acceptors. The Bronsted-Lowry theory was independently developed in 1923 by Johannes Nicolaus Bronsted and Thomas Martin Lowry.
To differentiate between acids and bases, we can first look at the chemical structure of the two substances. The acid is the strongest, while the base is the weakest. The bronsted-Lowry acid and base can be recognized by their ability to react with water. However, the base may have stronger effects on water. This reaction occurs when an acid or base reacts with an alkali substance.
Lewis
A brief definition of what Lewis means by "acid" and "alkali" is the process by which an acid or an alkali accepts or donates a pair of electrons. A proton, for example, is a Lewis acid because it accepts a pair of electrons. Borane, on the other hand, is a Lewis base because it donates an electron pair to a proton.
To understand the differences between an acid and an alkali, the definitions of the two are important. An acid is a substance that lacks an octet. An acid has six valence electrons and needs one more pair to be a Lewis acid. A Lewis alkali, on the other hand, contains an octet. Those acids, or alkalis, lack one octet.
Hydronium ion
The Hydronium ion in an acid and alkali solution is usually abbreviated H+(aq). The H+ ion is a proton in an isolated form that cannot exist in aqueous solution. It is transferred to a water molecule to form H3O+, which is the most representative acidic species in water. In contrast, hydrochloric acid is written HCl (aq) and is a strong electrolyte.
In chemistry, the concentrations of hydronium and hydroxide ions are inversely proportional and determine the properties and chemical behavior of a solution. In many cases, the proportion of one ion to the other is equal and can be referred to as autoionization. When this is true, water has a lower concentration of hydronium than it does of hydroxide ions.
Ammonia
Ammonia and acid and alkali are essentially the same thing, but in different ways. Ammonia is a weak base, and alkali is a strong acid. Acids have a pH level below neutral. Ammonia, on the other hand, has a pH level above neutral. As a result, it is a weak base. It is soluble in water, and it can be used to clean windows.
A mixture of ammonia and acid produces an ammonium salt. In both cases, ammonia reacts with a hydrogen ion, and it forms a co-ordinate bond with the acid. This process is called neutralisation, and the water produced during neutralisation cancels out the water used during ionisation. This chemical reaction is also responsible for producing carbon monoxide, which is classified as an acid.