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13 Dec 2019

consider the titration of 25.0 ml of 0.100 m nh3 with 0.100 M HCl. If 8.00 mL of HCl was added, what is the pH solution?

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Casey Durgan
Casey DurganLv2
17 Dec 2019

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Related questions

25.0 mL of a 0.100 M NH3 is titrated with a strong acid. 0.100 M HCl. Calculate the pH of the NH3 solution at the following points during the titration: (Kb= 1.8 x 10^-5) A. Prior to the addition of any HCl. B: After the addition of 10.5 mL of a 0.100 M HCl. C: At the equivilance point. D: After the addition of 3 mL of 0.100 M HCl. Show your work.

Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). A list of ionization constants can be found here.alculate the change in pH when 8.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.

Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq)

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