Topic: How much of a buffer needed to achieve a given pH? (Read 11866 times)

Borek · « **Reply #15 on:** April 05, 2009, 04:24:45 PM »

Quote from: yankeekd25 on April 05, 2009, 10:26:41 AM

NH3 + H+ --> NH4 + H2O

Perhaps its nitpicking, but charges are not balanced.

This way I will never know if what you write is wrong because you are making typos, or because you don't understand what you are doing. Hard to help in such situation.

yankeekd25 · « **Reply #16 on:** April 05, 2009, 11:41:04 PM »

Quote from: yankeekd25 on April 05, 2009, 10:26:41 AM

NH3 + H2O --> NH4+ + OH-

NH3 + H+ --> NH4 + H2O

Just made a typo on the last rxn. It's NH4+ + H2O right?

Borek · « **Reply #17 on:** April 06, 2009, 03:24:21 AM »

Yes, and that's almost the same as the necessary reaction of amine.

How many moles of conjugated acid do you need in the final solution?

yankeekd25 · « **Reply #18 on:** April 06, 2009, 08:39:36 AM »

Quote from: Borek on April 06, 2009, 03:24:21 AM

Yes, and that's almost the same as the necessary reaction of amine.

How many moles of conjugated acid do you need in the final solution?

Would it be .328 M x .225 L= 0.0738 ?

Topic: How much of a buffer needed to achieve a given pH? (Read 11866 times)

Borek

Re: How much of a buffer needed to achieve a given pH?

yankeekd25

Re: How much of a buffer needed to achieve a given pH?

Borek

Re: How much of a buffer needed to achieve a given pH?

yankeekd25

Re: How much of a buffer needed to achieve a given pH?

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