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Can someone please explain the chemistry of lidocaine synthesis to me. We made lidocaine in the lab and used 2,6 dimethylaniline, glacial acetic acid, chloracetyl chloride, sodium acetate, toluene, diethtylamine, hexane, HCL, potassium hydroxide and magnesium sulfate. I think this is pretty much a standard experiment in organic chemistry lab but I do not know the chemistry behind it. Can someone shed some light on this for me?
Before investigating the scene, the technician must dilute the luminol solution to a concentration of 2.00×10-2 it M. The diluted solution is then placed in a spray bottle for application on the desired surfaces.
An aqueous solution containing 34.1 g of an unknown molecular (nonelectrolyte) compound in 141.3 g of water was found to have a freezing point of -1.5 degrees C. Calculate the molar mass of the unknown compound.
At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.00. What is the Ksp of the salt at 22 °C
which of the following combinations of hybridization and molecular geometry is possible?1. sp3 trapezoidal2. sp3
Which statement is true for a reaction with Kc equal to 2.43 × 10-12? A) Increasing the temperature will not change the value of Kc. B) There are appreciable concentrations of both reactants and products.
Octane has a density of 0.692 g/mL at 20°C. How many grams of O2 are required to burn 1.00 gal of C8H18?
Calculation of Hydrogen Ion Concentration from pH What is the H concentration of a solution with pH of
supposed the theoritical yield in a reaction is 68.8g, and the percent yield is 66.0%. What is the actual yield of product obtained?
At 2000 degrees Celsius the equilibrium constant for the reaction 2NO (g) N2 (g) + O2 (g) is Kc=2.4x10^3 The initial concentration of NO is 0.174 M
The solution was then titrated to a blue-black endpoint with 26.0mL of a 0.0163 M KIO3 solution. How many mg of Vitamin C were in the tablet ?? and what % of the powder was Vitamin C?? Please solve this out for me
Calculate the heat energy released when 10.3 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for Mercury at 1 atm: Heat capacity: 28.0 J/(mol*K) Melting Point: 234.32 K Enthalpy of fusion
Write net Bronsted equations and determine the equilibrium constants for the acid-base reactions that occur when aqueous solutions of the following are mixed.
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