Problem
Problem
In a neutralisation experiment, 25 cm3 of dilute sulfuric acid was required to react completely with 40 cm3 of a solution of 0.25 mol dm-3 potassium hydroxide. a. a Write a balanced chemical equation for the reaction between dilute sulfuric acid and potassium hydroxide. b. b Calculate the number of moles of potassium hydroxide solution used in the reaction. c. c How many moles of dilute sulfuric acid would this number of moles of potassium hydroxide react with? d. d Calculate the concentration of the dilute sulfuric acid. e. e Which indicator could have been used to determine when neutralisation had just occurred?Intuitive explanation
This is about using stoichiometry and concentration relationships to find an unknown acid strength. The key insight is that at the neutralisation point, the moles of ions from the acid must exactly equal the moles of ions from the base—so you can calculate the base's moles first, then use the acid–base ratio from the balanced equation to work backwards to the acid's concentration.
Intuitive explanation
This is about using stoichiometry and concentration relationships to find an unknown acid strength. The key insight is that at the neutralisation point, the moles of ions from the acid must exactly equal the moles of ions from the base—so you can calculate the base's moles first, then use the acid–base ratio from the balanced equation to work backwards to the acid's concentration.