A 1.025 g sample containing a weak acid HX (mol. Mass=82) is dissolved in 60 mL. water and titrated with 0.25 M NaOH. When half of the acid was neutralised the pH was found to be 5.0 and at the equivalence point the pH is 9.0. Calculate mass precentage of HX in sample :

0.45 g of an acid ( mol. Mass = 90 ) is neutralised by 20 mol of 0.5 N NaOH solution. The basicity of the acid is :

A 0.252g sample of unknown organic base is dissolved in water and titrated with a 0.14 M HCl solution .After then addition of 20mL of acid ,a pH of 10.7 is recorded. The equivalence point is reached when a total of 40mL of HCl is added . What is the molar mass of the base?

A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid H_(2)A is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is:

A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid H_(2)A is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is:

A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid H_(2)A is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is: