Why is sulfuric acid a Diprotic acid?

Asked By: Adriaan Marchis | Last Updated: 21st March, 2020
Category: science chemistry
3.9/5 (359 Views . 25 Votes)
The most important chemical feature for a diprotic acid molecule is its ability to deprotonate two protons in two sequential steps during dissociation. Sulphuric acid follow this properties, that's why it is called diprotic acid.

Click to see full answer


Furthermore, is sulfuric acid a Diprotic acid?

Diprotic acids, such as sulfuric acid (H2SO4), carbonic acid (H2CO3), hydrogen sulfide (H2S), chromic acid (H2CrO4), and oxalic acid (H2C2O4) have two acidic hydrogen atoms. When sulfuric acid is classified as a strong acid, students often assume that it loses both of its protons when it reacts with water.

One may also ask, what is the PH of sulfuric acid? pH of Common Acids and Bases

Acid Name 1 mM
H2SO4 sulfuric acid 2.75
HI hydroiodic acid 3.01
HBr hydrobromic acid 3.01
HCl hydrochloric acid 3.01

Keeping this in consideration, what does it mean when an acid is Diprotic?

Definition: A diprotic acid is an acid that can donate two proton or hydrogen atom per molecule to an aqueous solution. Examples: Sulfuric acid (H2SO4) is a diprotic acid.

Is sulfuric acid a Monoprotic acid?

There is no monoprotic acid. The starting acid, sulfuric acid (H2SO4), has two acidic protons. In other words, these acidic protons were attached to the sulfate molecule. Always remember that monoprotic acids can only donate one acidic proton, not two as in the case of this acid.

39 Related Question Answers Found

Is nitric acid a Diprotic acid?

Hydrochloric acid (HCl) and nitric acid (HNO3) are common monoprotic acids. Although it contains more than one hydrogen atom, acetic acid (CH3COOH) is also a monoprotic acid as it dissociates to release only a single proton.

Why is Sulphuric acid called vitriol?

Originally Answered: Why sulfuric acid is known as oil of vitriol? To elaborate on Jeff Barber's answer, “green [and other colors] vitriol” are so called because crystals of these minerals resemble glass (vitrum), and it's oil of vitriol because concentrated sulfuric acid has an oily consistency.

What are Triprotic acids?

A triprotic acid is an acid that has three dissociable protons that undergo stepwise ionization: Phosphoric acid is a typical example: The first ionization is.

What are Diprotic and Triprotic acids?

diprotic acid: one that contains within its molecular structure two hydrogen atoms per molecule capable of dissociating. triprotic acid: one that can donate three hydrogen ions per molecule during dissociation.

Does sulfuric acid donate both protons?


Clearly, both the protons are not lost at the same time; it does happen step-wise. In fact, there are TWO equilibria that are set up for a STRONG dibasic acid (capable of donating two protons) like H2SO4. Clearly, both the protons are not lost at the same time; it does happen step-wise.

What is a weak Diprotic acid?

When we make a solution of a weak diprotic acid, we get a solution that contains a mixture of acids. Carbonic acid, H2CO3, is an example of a weak diprotic acid. The bicarbonate ion can also act as an acid. It ionizes and forms hydronium ions and carbonate ions in even smaller quantities.

Is HClO a strong acid?

Strong Acid: dissolves and dissociates 100% to produce protons (H+) 1. seven strong acids: HCl, HBr, HI, HNO3, H2SO4, HClO4, & HClO3 2. any acid that is not one of the seven strong is a weak acid (e.g. H3PO4, HNO2, H2SO3, HClO, HClO2, HF, H2S, HC2H3O2 etc.)

Are Diprotic acids stronger than Monoprotic?

Monoprotic acids, like HCl and HBr, contain just one hydrogen ion. Polyprotic acids, like H2 SO4 and H3 PO4, contain two or three hydrogen ions. It's tempting to think that polyprotic acid are stronger than monoprotic acids because they contain multiple hydrogen ions, but that's actually not true.

Is h3po4 a Diprotic acid?

Phosphoric acid (H3PO4) is a triprotic acid, phosphorous acid (H3PO3) is a diprotic acid, and hypophosphorous acid (H3PO2) is a monoprotic acid.

How do you know if an acid is Polyprotic?


Re: How to identify a polyprotic acid/base
As for the second part of your quesion, you can simply look at the anion. In order to be a polyprotic acid, the acid must be able to donate more than one H+ protons. Thus, thinking logically, you can look at the anion of the acid to see whether it is polyprotic or not.

Is h3po4 a strong acid?

While phosphoric acid is quite acidic, it is evident that it is, indeed, a weak acid because of the lack of full dissociation in water; a 1 M solution of strong acid would be around 0 (0 for monoprotic species, possibly less for diprotic due to an additional hydrogen ion).

What is the difference between Monoprotic Diprotic and Triprotic acids?

Polyprotic acid are able to donate more than one proton per acid molecule, in contrast to monoprotic acids that only donate one proton per molecule. Certain types of polyprotic acids have more specific names, such as diprotic acid (two potential protons to donate) and triprotic acid (three potential protons to donate).

How does Diprotic acid affect titration?

A diprotic acid is titrated with NaOH solution of known concentration. Molecular weight (or molar mass) is found in g/mole of the diprotic acid. Weighing the original sample of acid will tell you its mass in grams. Moles can be determined from the volume of NaOH titrant needed to reach the first equivalence point.

What is a Polyprotic acid?

A polyprotic acid is an acid that can donate more than one proton or hydrogen atom per molecule to an aqueous solution.

Is ch3cooh a Polyprotic acid?


Examples of weak acids include acetic acid (CH3COOH), which is found in vinegar, and oxalic acid (H2C2O4), which is found in some vegetables. Acids with a Ka less than 1.8×10−16 are weaker acids than water. If acids are polyprotic, each proton will have a unique Ka.

What is the pH of NaCl?

The pH of a sodium chloride solution remains ≈7 due to the extremely weak basicity of the Cl ion, which is the conjugate base of the strong acid HCl. In other words, NaCl has no effect on system pH in diluted solutions where the effects of ionic strength and activity coefficients are negligible.