Temperature is a measure proportional to the average translational energy (bouncing around) of molecules in a substance, but not energy itself. It is an important measure because energy always transfers from high temperature to low temperature bodies. Heat is the energy change during the transfer.
For Example: When we heat a fluid at a constant pressure.
$ Q $ is our heat added
$ \Delta t $ is our temperature change, $m$ is our mass, $ C_p $ is our constant pressure specific heat capacity.
$$ Q = mC_p\Delta t $$
Note that a body with a higher $m$ and $C_p$ can be heated by the same amount, but with a lower temperature increase.
Between the saturated liquid and saturated gas points, adding or losing heat does affect the temperature at all, but changes the relative proportions of liquid and gas in the mixture.