Use the concentration and rate data presented in the table below to answer the following questions about the hypothetical reaction:
A + 2B + 4C→ 2D + E
<span><span>Line[A] (mol/L)[B] (mol/L)[C] (mol/L)Rate (mol/L.s)</span><span>10.1000.1000.1003.6 x 10-2</span><span>20.2000.1000.1003.6 x 10-2</span><span>30.1000.2000.1007.2 x 10-2</span><span>40.2000.2000.2002.9 x 10-1</span><span>50.3000.2000.300?</span></span><span>Why would you expect this reaction to be a multi-step reaction, based on the overall reaction?What is the order of the reaction, with respect to each reactant?What is the overall order of the reaction?Write the rate law equation.How does the rate law equation confirm that this is a multi-step reaction?Predict the rate indicated by the “?”Propose a reaction mechanism using the criteria presented in the lesson, with the third step as the rate-determining step.<span>Draw a potential energy diagram to illustrate this reaction mechanism, assuming that the overall reaction is endothermic. Label reaction intermediates with the “RI”, and activated complexes with “AC”</span></span>
Answer:
b. The weak base of an alkaline buffer will accept hydrogen protons when a strong acid is added to the solution
d.The conjugate acid of an alkaline buffer will donate hydrogen protons when a strong base is added to the solution.
Explanation:
A buffer is a solution that resist pH change, it shows minimal change upon addition of small amount of strong acid or strong base. An alkaline buffer will have a basic pH, above 7. It is made by mixing a weak base and its salt with a strong acid. An example of an alkaline buffer is carbonate-bicarbonate buffer that is prepared using varying amount of anhydrous sodium carbonate and volume of solution of sodium bicarbonate to get pH range between 9.2 to 10.7
Within the buffer,the salt is completely ionized while the weak base is partly ionized. on addition of acid, the released protons will be removed by the bicarbonate ion to form sodium carbonate; on addition of base, the hydroxide ion released by the base will be removed by the hydrogen ions to form water and the pH remains relatively the same