How many grams of water are required to completely hydrolyze 0.54 grams of lidocaine?
What type of be equation should be used?
To determine the grams of water required to completely hydrolyze lidocaine, you need to know the chemical equation for the hydrolysis reaction involving lidocaine. Without this equation, it is not possible to determine a specific answer.
However, I can provide you with a general approach to solving this type of problem:
1. Write the balanced chemical equation for the hydrolysis of lidocaine. This equation should include lidocaine and water as reactants and the corresponding hydrolyzed products.
2. Calculate the molar mass of lidocaine. Determine the number of moles of lidocaine in 0.54 grams using the formula:
Moles = Mass / Molar mass
3. Use the stoichiometry of the balanced equation to determine the mole ratio between lidocaine and water. This ratio will tell you how many moles of water are required per mole of lidocaine.
4. Convert moles of water to grams by multiplying the number of moles by the molar mass of water.
It is important to remember that the specific hydrolysis reaction and its stoichiometry are necessary to provide an accurate answer.
http://en.wikipedia.org/wiki/Lidocaine
The above is lidocaine. The hydrolysis is shown here. The bond between the NH-C=O is split to leave the ring amine on the left and the carboxylic acid on the right as shown here.
http://www2.courses.vcu.edu/ptxed/m2/powerpoint/download/Lamb%20Drug%20Metabolism.pdf