Table of Contents
What is the pH of 0.1 m H2SO4 solution?
Further, H+ concentration = 10/100 = 0.1 M ( as the volume of the solution is 100 ml). So, we get pH = 1, which is the answer.
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 pH of 0.05 m H2SO4?
1
∴pH of 0.05M of H2SO4 is 1 The pH of 0.05M aqueous solution of diethyl amine is 12.0.
What is the pH of 10 3 m H2SO4?
Therefore the pH of the given solution is 2.69.
What is the pH of 1/10 2 molar aqueous solution of H2SO4?
pH is nothing but negative base 10 logarithm of hydrogen ion concentration in a solution. pH of the solution is calculated by formula. pH = -log(conc.) Hence, pH of given H2SO4 soln is 2.
What is the pH of 10 Sulphuric acid?
What Is The pH Value Of Sulphuric Acid?
Sulphuric acid | 1 mM | 10 mM |
---|---|---|
2.75 | 1.87 |
What is the normality of 0.05 m H2SO4?
Since 2 protons are available to react on each molecule of H2SO4, the normality is 2 N.
What is the pH of 10-8 M HCl solution?
The pH of 10-8 M of HCl is less than 7.
How do you calculate pH from H2SO4 molarity?
So, the pH of the sulfuric acid solution can then be calculated: pH = -log10[H+(aq)] pH = -log10[c + x]…Example: Calculating pH of Sulfuric Acid using R.I.C.E. Table and Quadratic Equation.
Ka2 | = | [H+(aq)][SO42-(aq)] [HSO4-(aq)] |
---|---|---|
x2 + 0.5x + 1.2 × 10-2x – 6.0 × 10-3 | = | 0 |
x2 + 0.512x – 6.0 × 10-3 | = | 0 |