How would an increase in the concentration of a sucrose solution affect the rate of its acidic hydrolysis? Regarding the acidic hydrolysis of sucrose 

$$\ce{\underset{sucrose}{C12H22O11} + H2O + \underset{catalyst}{H+} -&gt; \underset{glucose}{C6H12O6} + \underset{fructose}{C6H12O6} + H+},$$ 

I think that its mechanism can be described as a 2-step reaction consisting of a step which involves the H+, and then the step which involves the $\ce{H2O}$, and I believe the latter step to be a rate limiting step. 

My question in detail is: 


  Would an increase in the concentration of a sucrose solution, with a constant $\ce{H+}$ concentration, have a 1-to-1 influence on reaction rate (for example, if doubling the concentration of the sucrose solution would result in a hydrolysis reaction twice as fast), or would the addition of $\ce{H2O}$ in the second step significantly limit the change in reaction rate?
Looking at the reaction mechanism (of which I understand you are aware)
is good to keep in mind that the reaction rate really depends on the amount of intermediate here, provided the second step is rate limiting.

In the first step, $H^+$ is consumed. Since it is not rate limiting, I can assume the intermediate $[sucrose.H^+]$ to be in pseudo-equilibrium with $[H^+]$&amp;$[sucrose]$, on the timescale of the second reaction step.

$$r_2 = k_2[sucrose.H^+]$$

This means adding more sucrose (provided you have enough acid to protonate it) will indead result in the formation of more [sucrose.H^+] intermediate, and thus, higher kinetics.

Btw, I'm simpifying stuff here by not taking into account the reaction backwards for the second step.