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Chemistry
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11 Dec 2019

Suppose 20.0 mL of a 0.100 M NH3 solution is titrated with 0.100 M HI. Determine the pH of the solution after the addition of the following volumes of titrant.

a. 5.00 mL

b. 10.00 mL

c. 15.00 mL

d. 20.00 mL

e. 25.00 mL

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Tod Thiel
Tod ThielLv2
13 Dec 2019

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Related questions

A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution.

During the titration of 25.00 mL of 0.130 M weak base NH3 (Kb = 1.8 x 10^-5) with 0.100 M HCl, calculate the pH of the solution at the following volumes of acid added:

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25.00 mL of a solution of 0.100 M uric acid(Ka = 1.3 x10-4), andthen adds 5.00 mL of 0.15 M HCl, what is the pH?


25.00 mL of a solution of 0.100 M uric acid(Ka = 1.3 x10-4), andthen adds 15.00 mL of 0.15 M NaOH, what is the pH?


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Please show step by step explanation.thanks.

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