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    Hi everyone...

    I seriously do not get buffers!!! They are so complicated. I just had an equilibria test and had no idea how to go about the following three questions...

    Please help me out?

    (1) State and explain whether a 1.0 dm^3 solution of 0.10 mol NH3 and 0.20 mol HCl will form a buffer solution?

    (2) State and explain whether a 1.0 dm^3 solution containing 0.20 mol NH3 and 0.10 mol HCl will form a buffer solution?

    (3) Explain how you would prepare a buffer solution of pH 3.75 starting with methanoic acid?
    For this question, a previous part asked me to calculate the Ka value, [H^+] and pH which were: Ka = 1.78 x 10^-4, [H^+] = 1.33 x 10^-3 and pH = 2.87

    Thank you everyone :yep:
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    (Original post by MHMQ786)
    Hi everyone...

    I seriously do not get buffers!!! They are so complicated. I just had an equilibria test and had no idea how to go about the following three questions...

    Please help me out?

    (1) State and explain whether a 1.0 dm^3 solution of 0.10 mol NH3 and 0.20 mol HCl will form a buffer solution?

    (2) State and explain whether a 1.0 dm^3 solution containing 0.20 mol NH3 and 0.10 mol HCl will form a buffer solution?

    (3) Explain how you would prepare a buffer solution of pH 3.75 starting with methanoic acid?
    For this question, a previous part asked me to calculate the Ka value, [H^+] and pH which were: Ka = 1.78 x 10^-4, [H^+] = 1.33 x 10^-3 and pH = 2.87

    Thank you everyone :yep:
    Just remember that buffers are composed of a weak acid/base and its constituent salt =) that should help you through! Which part of the question do you not understand?
 
 
 
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