Buffer with Acid and Base Chem Question? Help Please?

A buffer contains significant amounts of ammonia and ammonium chloride.

a. Write an equation showing how this buffer neutralizes added acid (HI).

Here's what I have; where am I going wrong??

NH3+HI---->NH4+ + I-.

b.Write an equation showing how this buffer neutralizes added base (Ba(OH)2)

Again, apparently, I am going wrong; how?



Thank you for any help!!!

Chemteam: Thanks but apparently they wanted HI NH3---- NH4I. I am STILL not sure why.

2 Answers

  • Since HI is a strong acid, you could do this:

    NH3+H+ ---->NH4+

    Neutralizing the base is this reaction:

    NH4+ + OH- ---> NH3 + H2O

    The reaction you wrote:


    is that of a strong base (the Ba(OH)2) reacting with a strong acid (the HCl).

    Source(s): ChemTeam
  • The solution contains NH4+ (ammonium chloride) and NH3 (ammonia). Adding the strong acid HI is adding H+ ions. The H+ ions will react with NH3 to produce more NH4+:

    HI + NH3 ----> NH4+ + I-

    this reduces the concentration of NH3 and increases the concentration of NH4+ The equation for a basic buffer is pOH = pKb + log[NH4+]/[NH3]. the log term increases, so the pOH increases and the pH decreases.

    OH- from Ba(OH)2 reacts with the NH4+ ions in the buffer.

    OH- + NH4+ ----> NH3 + H2O

    [NH3] increases and [NH4+] decreases, the reverse of above

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