H20SO4(aq)-> 2H+(aq) + SO4 2- (a)

Calculate the hydrogen ion concentration (in mol 1-1) in this solution.

Show steps and explain your reasoning

Also what is the pH of the sulfuric acid solution nearet whole number

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Sulfuric Acid (H2SO4) is a strong acid, which dissociates when dissolved in water according to the following equation:

H20SO4(aq)-> 2H+(aq) + SO4 2- (a)

A 0.21g sample of sulfuric acid is dissolved completely in sufficiebt water to make 0.25litre of the final solution.
Calculate the hydrogen ion concentration (in mol 1-1) in this solution.
Answer to scientific notation to an appropriate number of sig fig.

Show steps and explain your reasoning

b)Also what is the pH of the sulfuric acid solution nearet whole number

To calculate the hydrogen ion concentration (in mol 1-1) in the sulfuric acid solution, we need to use the given information:

- A 0.21g sample of sulfuric acid is dissolved completely in sufficient water to make 0.25 litre of the final solution.

Step 1: Calculate the molar mass of sulfuric acid (H2SO4).
The molar mass of H2SO4 = (2 * 1.01 g/mol) + (32.07 g/mol) + (4 *16.00 g/mol) = 98.09 g/mol

Step 2: Convert the mass of sulfuric acid to moles.
0.21 g / 98.09 g/mol = 0.00214 mol

Step 3: Calculate the concentration (in mol 1-1) of hydrogen ions (H+).
Since 1 mole of sulfuric acid yields 2 moles of H+, the concentration of H+ is twice the initial concentration of sulfuric acid:
0.00214 mol * 2 = 0.00428 mol

So, the hydrogen ion concentration in the sulfuric acid solution is 0.00428 mol 1-1.

To calculate the pH of the sulfuric acid solution, we need to use the concept that pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration.

Step 4: Calculate the pH.
pH = -log10(0.00428) = 2.37

Therefore, the pH of the sulfuric acid solution is approximately 2.