daydayup

Thanks for your kind help! You are correct- I am studying biochemistry, and some biomedical science right now:) (and seems I am not getting so well with the chemistry foundations) I could check out the useful textbook later today and hope it can help figure out what happening on this topic:) Just now I am reading the book General Chemistry-Principles and Modern Applications and seems I have to know more on the topic, maybe I will come back later today to see if I have any idea on this question (so far I still don't what going on and didn't get what kind of calculation has been done...) I could try to reach the moderator to move it to the chemistry forum (but I needed some time to figure out how to reach the moderator...), hope you have a nice day anyway:)

Hi! I am a new user of this forum. Recently I have been studying the general Chemistry class and I have been struggling with the calculation of equilibrium. In this slide, it has declared that 10 mmol H+ is added to 1L of solution, with the buffer 0.1M HCO3 existing. My thinking would be like that : pH = pKa + log (conjugate base/acid), where pH=pKa=6.1 Thus, log (conjugate base/acid) =0 conjugate base [HCO3-] / acid [H+] = 1 When there is 0.1M HCO3, there would be 0.1M H+, however, I cannot drive to the same conclusion as my lecturer. I would like to ask how the lecturer could conclude that log (conjugate base/acid) =1 and why [buffer] = [acid] + [conjugate base]. I know that my questions seem stupid but I really struggle with the equilibrium calculation and would be much appreciated by anyone who wants to give a helping hand. If there is any textbook/ online resource that could help me learn this course (or biochemistry), I would also go and read it 😉 Thanks!