The natural variables of the internal energy $U$ are ${S,V}$. Sometimes it is helpful to get rid of the entropy here, and replace it by its conjugate variable. However, it is said in the literature (https://link.springer.com/content/pdf/bbm%3A978-1-4419-7344-3%2F1.pdf) :
One may replace the independent variable, X, by P. Simply replacing the coordinate X by the function’s slope at that point to yield a new function, Y(P), however, doesn’t quite work, because, as will be shown, some information is lost by this direct substitution. Notice that for a single variable, Eq. (A.2) becomes an ordinary differential equation, which, when integrated, yields the solution, Y(X). Indeed, this result occurs, but the solution so obtained is established only to within an as yet unknown constant of integration! See Fig. A.1. Thus, by using direct substitution some information is lost.
that we cannot simply write $U$ as a function of the partial derivative $\left.\frac{\partial U}{\partial S}\right|_V=T$, because this would lead to information loss (Basically because $U$ can be shifted up or down and the slope does not encode all information). This actually leads to the introduction of the Legendre transform which gives a new thermodynamic potential (the Helmholtz free energy) which has the natural variables ${T,V}$. However, I do not understand this reasoning, as we can always express the internal energy in any 2 thermodynamic variables, e.g. as a function of ${T,V}$ as:
$dU=\left.\frac{\partial U}{\partial T}\right|_V dT+\left.\frac{\partial U}{\partial V}\right|_T dV$
So is the latter formulation not exact or leads to a loss of information?
Edit:
Is this because we can actually exactly predict $dU$ but not the absolute value of the internal energy $U$ by using the slope? How does this go together with the definition of the internal energy as $U=TS-pV$?