What is the pH of 10 3 m H2SO4?

Therefore the pH of the given solution is 2.69.

What is the pH of the solution of Sulphuric acid having a concentration of 0.01 m?

The pH of 0.01 M sulphuric acid is 1.699.

What is the pH of 10 2m H2SO4?

Thus pH of the solution is 1.7.

What is the pH of H2SO4?

1.01
pH of Common Acids and Bases

Acid	Name	100 mM
H2SO4	sulfuric acid	1.01
HI	hydroiodic acid	1.08
HBr	hydrobromic acid	1.08
HCl	hydrochloric acid	1.08

What is the pH of 0.0005 m H2SO4 solution?

Therefore the pH value of a 0.005 molar aqueous solution of sulphuric acid is approximately 2.0.

What is the pH for H2SO4?

What is the pH of 10\% sulfuric acid?

1
Pricing & Availability

Physicochemical Information
Boiling point	101 °C (1013 hPa)
Density	1.066 g/cm3 (20 °C)
pH value	1 (H₂O, 20 °C)

What is the pH of H2SO4 10^-3(m)?

Since the concentration of H2SO4 is 10^-3 (M), the concentration of H+ in the solution will be 2*10^-3(M) (because each molecule of H2SO4 releases 2 H+ ions). pH of a solution is -log([H+]). So, the pH of the given solution is, -log(0.002)=2.69. Therefore the pH of the given solution is 2.69.

How do you find the concentration of sulfuric acid at pH 1?

When you know pH, you can calculate concentration of H 3 O + ions from pH equation. Due to pH = 1, H 3 O + concentration is 0.1 mol dm -3. Due to dibasic acid, when sulfuric acid molecule dissociate, two H 3 O + ions are given. Therefore, concentration of sulfuric acid should be a half of concentration of H 3 O +.

Is H2SO4 a strong diprotic acid?

> The pH of a 0.005 M H2SO4 s… is a strong diprotic acid. The equation for ionization is Each molecule of acid gives 2 molecules of H + . The concentration of H + ion is 2 x 0.005 = 0.010M pH = −log[H +]= −log[0.01]= 2.

What is the formula for dissociation of H2SO4?

[H+] = C+x, C is due to the first dissociation and x due to the second. H2SO4is a diprotic acid, dissociating in aqueous solution in two steps. The first dissociation is complete because pK1 = – 3.