it can donate a maximum of 2, but may only donate 1 due to the amount of dissociation that occurs. if the acid is added to water, the first hydrogen will be lost in the reaction:
H2PO4 <===> HPO4- + H+
The next reaction may or may not occur due to the dissociation of the first H+. if the first hydrogen has remained, then the second will not dissociate as the concentration of hydrogens is too high, and the backwards reaction may take place, where the negative, single hydrogen ion will accept the hydrogen as it is a conjugate base, creates the original reactant.
The molecular formula tells you this H2PO4:
2 Hydrogen atoms
1 Phosphorous atom
4 Oxygen atoms
= 7 atoms in total in one molecule of the dihydrogen phosphate anion
This depends on the concentration and to a smaller extend to temperature.
For normal dilute solutions of ethanoic acid it can be calculated by this formula:
[H+] = SQRT(1.8*10-5 * Ca) in which Ca is the ethanoic acid concentration and [H+] is the H ions concentration, both in mol/L.
Examples: pH = -log[H+] , so:
and
1 H+ Ion.
H3PO4 ===> H(+) + H2PO4(- )
Acid donates on singular H ion. This is evidenced by there only being one molecule of H within the equation.
U can use RMM to solve this question
The acid H2SO4 can donate up to 2 H+ ions.
An acid is a substance that releases hydrogen ions in water or will donate a hydrogen ion to another molecule. A monoacid, or monoprotic acid, is an acid that can only donate one hydrogen atom per molecule. You can also have diprotic acids, such as sulfuric acid, which can donate two hydrogen ions, and triprotic acids such as phosphoric acid, which can donate three.
Acid: A substance that can donate H+ ions. Alkali: A substance that can donate OH- ions. Neutral: A substance that cannot donate H+ or OH- ions.
Diprotic or dibasic acids are those which may produce two protons (H+ ions) per molecule in aqueous solutions as H2SO4.
A Diprotic Acid is not a single compound with a molecular formula. It is a type of acid that must have two hydrogens cable of turning into ions during dissolution. A good example is sulfuric acid, H2SO4. First, it separates into ions when dissolved in a solvent: H2SO4 → H+(aq) + HSO4−(aq) Then, the negative ion separates again, fulfilling the definition of having two H+ ions dissolved per molecule: HSO4−(aq) → H+(aq) + SO42−(aq)
That lad's sulphuric acid, H2SO4. It's a funky little molecule in which a sulphate ion (SO42-) is stabilised by a pair of hydrogen ions (2H+). It works quite well as a reducing agent, as it has twice as much hydrogen to donate as (for instance) hydrochloric acid.
An acid is a substance that releases hydrogen ions in water or will donate a hydrogen ion to another molecule. A monoacid, or monoprotic acid, is an acid that can only donate one hydrogen atom per molecule. You can also have diprotic acids, such as sulfuric acid, which can donate two hydrogen ions, and triprotic acids such as phosphoric acid, which can donate three.
H+ ions cause the acidity. The anion will simply be what's left of the molecule after dissociation. A molecule of sulphuric acid (H2SO4) for instance forms two H+ ions and one SO42- ion when dissolved in water
Acid: A substance that can donate H+ ions. Alkali: A substance that can donate OH- ions.
Acid: A substance that can donate H+ ions. Alkali: A substance that can donate OH- ions.
Acid: A substance that can donate H+ ions. Alkali: A substance that can donate OH- ions. Neutral: A substance that cannot donate H+ or OH- ions.
Any reasonably strong acid produces hydronium ions when dissolved in water. Sulfuric acid, with formula H2SO4, is a common example.
Diprotic or dibasic acids are those which may produce two protons (H+ ions) per molecule in aqueous solutions as H2SO4.
Yes and no. One definition of an acid is a molecule that can donate a H+ ion. So for example if you have an acid such as hydrochloric acid (HCl) in water, HCl will donate it's H+ to the H2O molecule, forming Cl- and H3O+. In contrast, a base is a molecule that accepts H+ ions. This means a base such as NH3 reacts with H2O to form OH- and NH4. So when pH is measured, it is the ratio of H3O+ ions to OH- ions. If there are more H3O+ ions, you then know that there are more acidic molecules in the solution, since they must be giving away their H+ ions. So a solution with an acid in it will have more H3O+ ions (which can be described as H+ ions) in it. However, an acid by itself will have nothing to donate H+ ions to. P.S The number of H's in a molecule often don't help to identify it as a base or an acid.
A Diprotic Acid is not a single compound with a molecular formula. It is a type of acid that must have two hydrogens cable of turning into ions during dissolution. A good example is sulfuric acid, H2SO4. First, it separates into ions when dissolved in a solvent: H2SO4 → H+(aq) + HSO4−(aq) Then, the negative ion separates again, fulfilling the definition of having two H+ ions dissolved per molecule: HSO4−(aq) → H+(aq) + SO42−(aq)
That lad's sulphuric acid, H2SO4. It's a funky little molecule in which a sulphate ion (SO42-) is stabilised by a pair of hydrogen ions (2H+). It works quite well as a reducing agent, as it has twice as much hydrogen to donate as (for instance) hydrochloric acid.
No, H2SO4 is an electrolyte, as it produces hydronium ions in aqueous solution.
You just know it does.... Only possible explanation is that sulfuric acid is H2SO4. H2SO4 --> H2 + (SO4)-2.