The initially red color has faded in the course of the reaction. Briefly explain why did the color disappear.

Draw the content of the final reaction mixture. Explain your reasoning.

Which of the following statements best describes the end point of the reaction and when you should stop the timer? Group of answer choices Once the purple color of the initial mixture, caused by the KMnO4, fades After 5 minutes have passed Once the KMnO4 has reacted completely with the malonic acid, turning the solution yellow Once the mixture turns colorless

PLEASE HELP ME ANSWER QUESTION 5) A student starts a titration without phenolphthalein in the Erlenmeyer flask. The student realizes the mistake and adds the phenolphthalein during the titration. Once the phenolphthalein is added, the solution in the Erlenmeyer flask remains colorlessCan the results of this titration be used? Concisely explain.

what is the purpose of addition of acid during the reaction

Provide a plausible arrow pushing mechanism for the reaction belaw. 1. nBuLi 2. NMe MgCI HO,C 3. CO2 4. acidic workup NMez

%N in sample can be obtained by converting all N containing compounds to NH3.  The generated NH3 is then reacted with excess HCl and excess HCl  is backtitrated with NaOH. Why is back titration done for this analysis?   a.Titration with strong acid and strong base will produce sharper endpoint than titration with strong acid and weak base. b.Nitrogen compounds will only react with excess acids. c.Backtitration will be faster than doing direct titration. d.NH3 is a weak base and large amount of titrant is needed to reach equivalence point.

Write a balanced net ionic equation to show why the solubility of CaCO3 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.   Here is the problem:

There is something wrong with the following reaction scheme. Identify what is incorrect and explain why. Feel free to use chemical drawings to aid in your answer .

What reaction occurs as a hydrochloric acid solution is added to a solution containing equal concentrations of acetic acid and sodium acetate Group of answer choices CH3COOH + H+ → CH3COOH2+ CH3COOH + H+ → CH3CO+ + H2O 2CH3COO– + 2H+ → CH3COO + H2 CH3COO– + H+ → CH3COOH