lnk = -Ea/RT + lnA
y = mx + c
(The Arrhenius equation).
As you can see, concentration doesn't appear in this equation.
lnk = natural log of rate constant (k)
Ea= activation energy
R= relative gas constant (8.314)
T= Temperature, kelvin.
lnA= natural log of preexponential factor A (don't worry about what this is).
You use this equation in A2 to find the activation energy (and sometimes A) from graphs.
Another way you can tell that concentration doesn't affect the rate constant is the "simpler" rate equation:
Rate =k [M]m[N]n where m and n are the orders of the reactants (basically the effect that increasing concentration of these reactants has on the overall reaction). The square brackets represent concentrations of the reactants.
As you can see, rate is affected by concentration- if [M] were to increase, so would the rate because k and [N] are being multiplied by a larger number.
But, k in itself isn't affected by concentration. It is the rate constant for a reaction at a given temperature.
Think about the kinetics of a reaction. Increasing concentration means there are more molecules/atoms in a certain volume, increasing the likelihood of molecules colliding, but not affecting the number of molecules above activation energy.
However, increasing temperature means that more molecules are above activation energy (look at Boltzmann distributions).
This links back to the Arrhenius equation, which talks about activation energy but not concentration- hence catalysts and temperature does change the rate constant.
Sorry this is badly explained, it's been a while since I did this rate constant nonsense XD