A chemist titrates 130.0mL of a 0.7797M sodium hydroxide NaOH solution with 0.52

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A chemist titrates 130.0mL of a 0.7797M sodium hydroxide NaOH solution with 0.5269M HCl solution at 25°C . Calculate the pH at equivalence. Round your answer to 2 decimal places. ome Flle Edit View History Bookmarks People Window Help xf Facebook A ALEKS-Learn-Albert Yeboa x( hstagram CSecure https:/www.-awh.aleks.com/alekscgi/x/lsl.exe/1o.u-igNslkr 7j8P3jH-lis1SBdKFh4JYC7viz6 juOtYisau7L4e3 O ACOS, BASES AND AQUEOUS EQUILIBRIA -Calculating the pH at equivalence of a titration A chemist titrates 130.0 ml of a 0.7797 M sodium hydroxide (NaOH) solution with 0.5269 M HCI solution at 25 °C Calculate the pH at equivalence. Round your answer to 2 decimal places Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH - Check

Explanation / Answer

equivalence point is the point in titration where equal mol of acid and base are added

Here acid is HCl which is strong acid

Here base is NaOH which is strong base

when we add equal amount of HCl and NaOH, all HCl and NaOH will react completely to form salt and water which is neutral

Since final solution is neutral, pH will be 7

Answer: pH = 7.0

Feel free to comment below if you have any doubts or if this answer do not work

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