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A setup similar to experiment 2.1 has been conducted to find the heat of neutralization for an acid-base reaction.
A monoprotic acid, CH3COOH was used to mix with NaOH (sodium hydroxide). The initial temperature of the acid and base is 250C.
Around 35 mL of the base and 50 mL of the acid was mixed in a calorimeter.
Both solutions have a molar concentration of 0.25 M.
After the mixing and the reaction is finished, a final temperature of 26.402 0C was recorded.
Calculate the heat of neutralization and round answers to 2 decimal places (2% tolerance).
Assume calorimeter insulates and does not absorb any heat, and specific heat of the solution is 4.184 J/g-0C. Take note of the sign of the final answer.
Show all the steps in the mechanism for the following reaction, When benzene is mixed with deuterated sulfuric acid, deuterium is slowly incorporated onto the ring. Show the mechanism for this reaction and explain how this relates the sulfonation of ..
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