Acids and Bases
What is the formula for calculating pH if the concentration of hydrogen ions ([H+]) in a solution is known?
Which component do you need to calculate using the Henderson-Hasselbalch equation for a buffer solution?
In the Henderson-Hasselbalch equation, what is the relationship between the pH of a solution and the pKa when the concentrations of an acid and its conjugate base are equal?
Given equal molecular masses, what is the primary reason that polar substances generally have higher boiling points than nonpolar substances?
In an efficient buffer system composed predominantly of NH₄Cl (NH₄⁺), if the nitrous acid (HNO₂) is present as a weak acid with a pKa of 3.35 and pH is adjusted to an optimal buffering range, how would the pH compare to the aforementioned pKa?
What is the primary role of buffer systems as related to the Henderson-Hasselbalch equation?
If you have a buffer solution containing a weak base with pKb = 3.70 and its salt at concentrations [B] = [HB+], what will be its approximate pH?
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A solution of acetic acid has a pH of 6.75. The ratio of acid to conjugate base is _______________. (pKa = 4.75)
Why does ethylene glycol have a higher boiling point than ethanol despite having a lower molecular weight?
Which change would NOT affect the validity of using the Henderson-Hasselbalch equation for a buffered solution?