Acids and Bases
Given equal molecular masses, what is the primary reason that polar substances generally have higher boiling points than nonpolar substances?
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?
Which change would NOT affect the validity of using the Henderson-Hasselbalch equation for a buffered solution?
What happens to the pH of a buffered solution when the concentration of its conjugate base is increased while the concentration of the weak acid stays the same?
A researcher prepares two buffer solutions with equal volumes of 0.050 M HCOOH (formic acid) but varies formate (HCOO-) ion amounts creating 0.025 M for first solution & 0.075 M for second; which buffer resists increase in pH better upon adding same moles of NaOH?
What is the formula for calculating pH if the concentration of hydrogen ions ([H+]) in a solution is known?
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?
How are we doing?
Give us your feedback and let us know how we can improve
If a student wrongly uses half as much conjugate base required when preparing a buffered solution using Henderson-Hasselbalch equation, what effect does this error have on pH?
Why does ethylene glycol have a higher boiling point than ethanol despite having a lower molecular weight?
How would you prepare a buffer solution with a desired pH using the Henderson-Hasselbalch equation?