Hi guys. Imagine how dumb I feel for never having heard of this

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The discussion centers on the Henderson-Hasselbalch equation, which is crucial for understanding buffer solutions and ionic equilibria. Users emphasize the importance of grasping the equation's applications, particularly in calculating pH using the formula pH = pKa + log[salt]/[acid] or its variations. A key point made is the necessity of learning to calculate logarithms manually, as calculators are not permitted during the exam. Practicing logarithmic evaluations is recommended to build confidence and proficiency. The equation is described as a rearranged form of the dissociation constant, reinforcing its validity when equilibrium concentrations are used. Overall, mastering this equation and logarithmic calculations is essential for success in the upcoming exam.
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Hi guys. Imagine how dumb I feel for never having heard of this equation before today. I have a serious exam coming up and the only thing I know is that this will definitely be coming up.


I know it's applications, but I have no clue how to apply it proper. There are no calculators allowed and I don't know how to get a log.


Help? I'm pretty desperate here.
 
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this eqn. can be used not only in acidic and basic buffers but also in any equation involving ionic equilibrium.instead of the concentration of the salt you might also put the conc. of the ion of the electrolyte , still the eqn. holds good.
ph=pKa + log[salt]/[acid] or ph = pKa + log[anion]/[aci]d and so on.
learn to calculate simple logarithms.this will do the trick for the exam.practise 6 to 7 evaluations of log and u will be on.
all the best for your exam.
 


HH equation is just a rearranged dissociation constant, it HAS to hold, as long as you put equilibrium concentrations in it.
 

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