I have done an experiment on the hydrolysis of aspirin, which is pseudo-first order. I need to find the rate constant, but I only have the final ($0.0278\mathrm{~M}$) and initial ($0\mathrm{~M}$) concentrations of the product (salicylic acid), the volume of the solution ($0.06\mathrm{~L}$), the change in time ($24$ hours), and the temperature ($25\mathrm{~^\circ C}$). Is there a way to find the rate constant of this reaction? My main problem is that I do not know the initial or the final reactant concentrations; I cannot simply subtract the concentration of product formed from initial reactant concentration to find the final reactant concentration, as I do not have either reactant concentration.

  • $\begingroup$ What's the relationship between the concentration of your product and the concentration of your reactant? I won't tell you any more. Figure it out yourself. It's important. $\endgroup$ – orthocresol Oct 24 '15 at 18:37
  • $\begingroup$ The reaction is Acetylsalicylic Acid + Water to Salicylic Acid + Acetic Acid $\endgroup$ – Zaleron Oct 24 '15 at 18:38
  • $\begingroup$ pseudo first order $\endgroup$ – Zaleron Oct 24 '15 at 18:38
  • $\begingroup$ You're not answering the question $\endgroup$ – orthocresol Oct 24 '15 at 18:39
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    $\begingroup$ Try and figure it out yourself first. If you're really stuck look at this previous question chemistry.stackexchange.com/questions/32346 I have to go off and won't be around to answer comments. $\endgroup$ – orthocresol Oct 24 '15 at 18:45