Question

Calculate the pH of a 2.0 M H2SO4 solution.

Answer 1

 H2SO4 gives 2 moles oh H+ per mole of acid 

[H2SO4] = 2M so [H+] = 4M 

pH = -log(4) = -.6 

Therefore, the pH of a 2.0 M H2SO4 solution is -0.6


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Answer 2

Answer:The pH of the solution -0.60 .The pH scales ranges value from 1 to 14.So, the given pH of the solution is coming out to negative which means that in a lab preparation of solution with this pH is not feasible.

Explanation:

The pH of the solution defined as negative logarithm of $[H^+]$ ion concentration.

$H_2SO_4(aq)\rightarrow 2H^+(aq)+SO_4^{2-}(aq)$

According to reaction 1 moles of sulfuric acid gives 2 moles of $H^+$

Then 2 mol /L solution of sulfuric acid will give = 4 mol/L of $H^+$ ions.

$pH=-\log[H^+]=-\log[4.0]=-0.60$

The pH scales ranges value from 1 to 14.So, the given pH of the solution is coming out to negative which means that in a lab preparation of solution with this pH is not feasible.