What is Ka2 for H2SO4?
What is Ka2 for H2SO4?
In the lecture sulfuric acid, H2SO4, was mentioned explicitly, because it is an exception to the rule. The Ka1 value on its own is large, and the Ka2 value is 10^-2 which by itself is also significant in the equilibrium.
Why is Ka2 Ka1 for H2SO4?
H2SO4 ionises in two stages and hence has two dissociation constants. Ka2 << Ka1. This is because the negatively charged HSO4- ion has much less tendency to donate a proton to H2O as compared to neutral H2SO4.
What does Ka2 mean in chemistry?
Ka2 represents the dissociation of the 2nd H+.
What is the pKa of H2SO4?
Sulfuric acid (H2SO4): pKa1 ≈ -3 (first dissociation only) p-Toluenesulfonic acid: pKa = -2.8.
What acid eats through steel?
Hydrochloric acid
Which acid is stronger HCl or h2so4?
Generally, both Hydrochloric acid (HCl) and Sulfuric acid (H2SO4) are really strong acids compared to any other acids. However, HCl is stronger than H2SO4. This is mainly due to the difference in the basicity of both acids. Additionally, if we look at the pKa value HCl has a pKa of -6.3 and sulfuric acid has a pKa ~-3.
Why is Sulphuric acid called King of chemicals?
Sulphuric acid (H2SO4) is called the “King of Chemicals” because it is used in the preparation of a very large number of other useful chemicals such as hydrochloric acid, nitric acid, dyes, drugs etc. Sulfuric acid is prepared industrially by the reaction of water with sulfur trioxide.
Which Oxoacid of Sulphur is called King of chemicals?
Sulphuric acid
Where does Sulphuric acid come from?
Sulfuric acid is formed naturally by the oxidation of sulfide minerals, such as iron sulfide. The resulting water can be highly acidic and is called Acid Rock Drainage (ARD). The acidic water so formed can dissolve metals present in sulfide ores, resulting in brightly colored and toxic streams.
Is sulfuric acid used in bleach?
Chlorine bleach is a solution of sodium hypochlorite and water. Chlorine gas is produced when sulfuric acid is mixed with chlorine bleach. This reaction is a function of the change in pH of the solution from alkaline to acidic combined with the strong oxidant properties of hypochlorous acid.