Question

calculate the pH of resulting mixture 10ml of 0.1M H2SO4 + 10ml of 0.1M KOH. Best answer would be given brainliest answer

Answer 1

the pH for 0.1M of H2SO4 and KOH is 2.60
* you first need to write the balanced equation: 

H2SO4(aq) + 2KOH(aq) → 2H2O(l) + K2SO4(aq) 

* mole ratio for acid and base from the equation is 1 : 2 

* 0.01 mole of H2SO4 will react with 0.02 moles of KOH. but because you only have 0.01 moles of KOH, it will limit your reaction. 

therefore, only 0.005 moles H2SO4 reacts with 0.01 moles of KOH. 

number of moles of excess acid is 0.01 - 0.005 = 0.005 moles of H2SO4 

concentration of the excess acid in solution C = n/v ---> =0.005 / 2 ---> = 0.0025 mol/L 

pH= -log [H] 
= -log[0.0025] 
= 2.60