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What is the pH of a buffer solution prepared by dissolving 0.075 moles of the weak base, aniline (C6H5NH2), and 0.045 moles of a salt of its conjugate acid, anilinium chloride (C6H5NH3Cl), in a total buffer volume of 1.00 liters?  

Initial pH of buffer solution is:

What will the pH be after 0.012 moles of HNO3 are added?  This addition does not change the total volume of the solution. 

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Related questions

A buffer solution contains 0.312 M C6H5NH3Cl and 0.324 M C6H5NH2 (aniline). Determine the pH change when 0.075 mol NaOH is added to 1.00 L of the buffer.

pH after addition − pH before addition = pH change =

1.A buffer solution contains 0.314 M KH2PO4 and 0.368 M K2HPO4. Determine the pH change when 0.110 mol HCl is added to 1.00 L of the buffer.


pH change = _________

2.A buffer solution contains 0.272 M C6H5NH3Cl and 0.399 M C6H5NH2 (aniline). Determine the pH change when 0.115 mol HNO3is added to 1.00 L of the buffer.


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1. A buffer is made by mixing 1.250 mol formic acid, HCOOH, with 0.750 mol sodium formate, HCOONa in enough water for a total volume of 1.00L. The Ka of formic acid is 1.87 x 10-4

a. What is the pH of this buffer?

b. If 0.075 mol HCl is added to this buffer, what is the pH of the resulting buffer? (assume no volume changes)

c. If 0.055 mol NaOH is added to this buffer, what is the pH of the resulting buffer? (Assume no volume changes)

2. A buffer solution contains 0.120 moles of propionic acid, HC3H5O2, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer?

b. What is the pH of this buffer after the addition of 0.010 mol of NaOH?

c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?

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