Calculate the concentration of h+ ions in a 0.010m aqueous solution of sulphuric acid and it can be find the concentration with the strong acid, such as h2so4.

Hello, reders, today we will discuss about hydrogen ions concentration.

We will try to show valuable information regarding this.

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Hydrogen ion concentration

Hydrogen ions concentration are related with pH or it is represent and expressed as pH. hydrogen ions concentration units are gram moles per liter. and hydrogen ions concentration show how solution is acidic or basic. if you know about value of pH then you can easily calculate properly the hydrogen ions concentration. and you know that the pH mean or ph full form is potential of hydrogen.


the hydrogen ions concentration equation is,

pH = [-log10H+]

You can find the value of pH with the help of this equation.

But if you want to find the value of H+ in mole -1 then you can calculate using this equation,

H+ = 10-ph

In same way, a solution with a pH of 7 contains 10-7 mol/l of hydrogen ions.

and similarly, a solution with a pH of 6 contains 10-6 mol/l of hydrogen ions.

the over all, hydrogen ion concentration related to it’s ph, it is properly find out on the pH scale.


the lower hydrogen ion – less ph

Less hydrogen ion – higher ph.

So, in this way you can find out the value of pH as well as h+ ions.

Calculate the concentration of h+ ions in a 0.010m aqueous solution of sulphuric acid.

Aqueous solution of sulphuric acid is,

H2SO4 – 2 H+ + so4-

Where, h2SO4 – sulphuric acid

This equation indicate,

one mole of sulphuric acid (h2so4) gives 2 H+ ions, (2 mole of hydrogen ions)

So, according to question,

0.010 mol of h2SO4 will give 2 × 0.010 moles of H+ ion.

Concentration of H+ ion = .020 M

therefore, the concentration of hydrogen ions is 020 M.

Classify each of substance as a strong acid, strong base, weak acid, weak base?

Here, first we will discuss about strong acid and strong base. after this we will discuss about weak acid and weak base?

Lets started,

Strong Acid

  1. H2SO4 – sulphuric acid
  2. HCl – hydrochloric Acid
  3. HNO3 – Nitric Acid
  4. HBr – hydrobromic Acid

Strong Base

  1. NaOH – sodium hydroxide
  2. KOH – potassium hydroxide
  3. LiOH – lithium hydroxide
  4. Ca(OH)2 – calsium hydroxide

Weak Acid

  1. H2SO3 – Carbonic Acid
  2. H3PO4 – Phosphoric Acid
  3. H2SO3 – Sulphurous Acid
  4. CH3COOH – Acetic acid

Weak Base

  1. Mg(OH)2 – magnesium hydroxide
  2. NH4 OH – Ammonium hydroxide

Note:- strong acid ionise fully in water to produce large amount of H+ ions. Where as strong base also ionised fully in water to produce large amount of H+ ions. But if i am talking about, weak acid and other weak base, they are not ionised fully in water, so they are produce small amount of H+ ions.