Can I ask you to explain your rationale for your statement that fronting peaks may be caused by inadequate buffering?
I agree with this, but I am not sure if you are making a general claim or describing a specific case.
It's a general claim, but occurs infrequently and under specific circumstances.
First of all, the most common result of insufficient buffer is tailing of basic compounds (assuming silica-based packings and a low enough pH to suppress silanol ionization).
However, if "active-silanol" tailing is not an issue (non-silica column, or very pure, fully covered silica, etc.) and the analyte is basic, you can get fronting as illustrated in the sketch below (as above, I apologize for the poor artwork, but it's easier to sketch than to try and explain entirely in words).
The upper graph shows the k' vs. pH curve for a basic compound. Below its pKa the molecule is ionized and relatively hydrophilic. Above its pKa, it is unionized and relatively hydrophobic. Imagine that you are using a low-pH buffer, with a pH at point "A" on that curve. Now visualize what happens if you inject your basic sample at a higher concentration than the buffer can handle (lower drawings). The low-concentration parts of the peak (leading and trailing edge) is still within the effective range of the buffer, and "see" a pH value of "A". If the high-concentration part of the peak (apex) exceeds the buffer capacity, it will "see" a higher pH of "B", because the analyte will in effect act as a buffer and pull the pH toward its pKa.
Per the upper graph, the "A" parts of the peak will have a low k' (move fast) while the "B" parts of the peak will have a high k; (move slowly) so that the apex of the peak lags behind the leading and trailing edges, resulting in a "fronting" shape.