How do you find the pH of H3PO4?

1. pH = -log{H+} = 5.00 given.
2. So {H+} = 1 x 10^-5M.
3. H3PO4(aq) = H2PO4- + H+ = HPO4- – + H+ = PO4- – – + H+
4. Ka1,Ka2 and Ka3 values for H3PO4 are 10^-3, 10^-8 and 10^-12 respectively.
5. Ka1 = 10^-3 = {H+}x{H2PO4-}/[H3PO4}
6. So {H+} = {H2PO4-} = x.
7. Then x^2 /[H3PO4} = 10^-3 and [H3PO4} = x^2/10^-3.

How do you calculate the pH of dibasic acid?

(a) Calculate the hydrogen ion concentration and pH of a 1.5 mol dm–3 solution of sulfuric acid.

1. H2SO4 is dibasic/diprotic acid, so [H+(aq)] = 2 x 1.5 = 3.0 mol dm–3
2. pH = –log(3.0) = –0.477.

What is the pH value of sulfuric acid?

What Is The pH Value Of Sulphuric Acid?

Why are Polyprotic acids weak?

Defining Polyprotic Weak Acids HA is a weak acid because it does not completely dissociate (ionise), that is, the molecular form of the acid is in equilibrium with the ions produced by its partial dissociation.

Are all Polyprotic acids weak?

Polyprotic acids are specific acids that are capable of losing more than a single proton per molecule in acid-base reactions….Introduction.

What is the pH of 0.1% phosphoric acid?

approximately 1.5
2 The pH of a 0.1 N aqueous solution is approximately 1.5.

Can you have a negative pH?

Summary of Negative pH Negative pH is possible and simple to calculated, but not something you can easily measure. Special electrodes are used to assess extremely low pH values. In addition to negative pH, it’s also possible for pH to have a value of 0.

Does sulfuric acid have a high or low pH?

Since sulfuric acid is a strong acid, a 0.50 M solution of sulfuric acid has a pH close to zero.

How do you find the pH of polyprotic acid?

A polyprotic acid is an acid that can donate more than one hydrogen atom (proton) in an aqueous solution. To find the pH of this type of acid, it’s necessary to know the dissociation constants for each hydrogen atom. This is an example of how to work a polyprotic acid chemistry problem.

What is an example of a polyprotic acid chemistry problem?

This is an example of how to work a polyprotic acid chemistry problem. Determine the pH of a 0.10 M solution of H 2 SO 4 . H 2 SO 4 has two H + (protons), so it is a diprotic acid that undergoes two sequential ionizations in water:

Which is more difficult to remove h+ from a polyprotic acid?

Note:(i) K a1> K a2> K a3Always true for polyprotic acids, i.e., each ionization step is more difficult because it is more difficult to remove H+from a molecule as its negative charge increases. BUT this does not apply for ionic salts of these acids, e.g., Na

Why is it more difficult to ionize polyprotic acids?

a1> K a2> K a3Always true for polyprotic acids, i.e., each ionization step is more difficult because it is more difficult to remove H+from a molecule as its negative charge increases. BUT this does not apply for ionic salts of these acids, e.g., Na