A chemist titrates 30.0 mL of 0.840 M hydroxylamine, HONH2 Kb = 1.1 x 10–8 ,...

A chemist titrates 30.0 mL of 0.840 M hydroxylamine, HONH2 Kb = 1.1 x 10–8 , with 0.900 M HNO3. Calculate the pH at each of the following volumes of added titrant.

12.0 mL HNO3

14.0 mL HNO3

28.0 mL HNO3

35.0 mL HNO3

Expert Solution

NOW PH= 14 - POH

= 14 - 7.83

= 6.17

Please check the calculations and pay attention to the unit analysis.

queen_honey_blossom answered 1 year ago

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