Chemistry
For the reaction 2 N2O <===>O2 + 2 N2 what happens to the equilibrium position if the pressure is increased
Chemistry
Second thought I just don't understand what to do. pH= pKa + log [NH3]/[NH4NO3] pH= -l log ? + log (0.005/?) pH= ? pH= ?
Chemistry
Don't think I know how to calculate the M of NH4NO3
Chemistry
So is it a problem if the conch of NH4NO3 was not given to me. Or do I just assume it's the same as the NH3
Chemistry
Calculate the pH buffer made by combing 50.0 mL of 1.00M ammonia and 50.0mL of ammonium nitrate. Can I use the same formula? If so do I do anything with the mL
chemistry
DrBob I want to thank you SOOOOO much for all the help you give. I had never heard of the H H equation. And I also appreciate you patience
chemistry
This what I did log(1.76 x 10-5) +log(0.150/0.200) = 4.879
chemistry
No I'm sorry I just used this as the example of the H H equation
chemistry
pH = pKa + log ([A-]/[HA]) pH = pKa + log ([C2H3O2-] / [HC2H3O2]) pH = -log (1.8 x 10-5) + log (0.50 M / 0.20 M) pH = -log (1.8 x 10-5) + log (2.5) pH = 4.7 + 0.40 pH = 5.1 I used this example And I still got it wrong it should have been 4.75 + 0.12 = 4.87 or do I use just 4.7...
chemistry
Ok DrBob I think I got it after all the plugging in my final answer is 5.45 I hope
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