Question

The neutralization of an acid with a base yields a salt and usually water in aqueous solution. Calculate the pH when 55.0 mL of 0.273 M perchloric acid is mixed with 55.0 mL of 0.273 M sodium hydroxide solution at 25 °C. pH = Calculate the pH when 55.0 mL of 0.273 M of a monoprotic weak acid, HA, is mixed with 55.0 mL of 0.273 M sodium hydroxide solution at 25 °C. The Ką for HA is 4.9 x 10-5. pH =

Answer 1

& acid = moles of bease aced & base so 2 Solution ID Here moles of & both are the strong at equivalence point PH=7 I br. In - but so PH this the at also moles of acid = moles al base aced is weak acid. equivalence Point. PH = - I log (kwka) CHA / CHA concentration of CHA - moles - Total volume. acid MINI x, the 027 3855 Sstss - 0.137 M 0.137 PH = I log (10-14 x 4.9x10-s) Pt-Llog ( 4.9x10-19) Pra 8.72 139 Answer,