# dear sir i want the pre lab done after 10 hours and for the rest i'll send the information tomorrow night and i want everything done in 04/ 05 Document Preview: Experiment #5 - pH Buffers Required...

dear sir i want the pre lab done after 10 hours

and for the rest i'll send the information tomorrow night and i want everything done in 04/ 05

Document Preview:

Experiment #5 - pH Buffers Required Skills To perform this experiment you need to have mastered the entire laboratory skills required for Experiment #3. Most importantly, you need to have developed a solid theoretical understanding of pH buffers. A short summary follows, but each student should read and understand the sections in their CHM 158 textbook regarding buffers. If the background material is mastered prior coming to lab, this lab is very easy. Background A buffer is a solution that has an appreciable concentration of a weak acid and its conjugate base. Such solutions are called "buffers" because they resist change in pH when the volume of the solution is changed (through either dilution or concentration) and when small amounts of strong acid or strong base are added. Most naturally occurring aqueous solutions (e.g., blood and lakes) are buffered. In the laboratory, buffers can be created in numerous ways, but the three most common ways are: i. Adding comparable amounts of the weak acid and its conjugate base to water. ii. Adding a limited amount of strong acid to a solution of a weak base. iii. Adding a limited amount of strong base to a solution of a weak acid. Predicting the pH of a Buffer The pH of a buffer solution can be easily derived from the equilibrium expression associated with the dissociation of the weak acid: - +HA + H O ? A + H O (Rxn 1) 2 3- +[A ][H O ]3K = (Eq 1) a[HA]Equation 1 can be rearranged to yield [HA]+[ ] (Eq 2) H O =K3 a-[A ]1 Rev 1/2013CHM 158: Experiment #5 If we take the negative logarithm of each side of equation 2 we obtain -[A ]pH= pK +log (Eq 3) a[HA]+where pH = -log[H O ] and pK = -log K . Eq. 3 is known as the Henderson-Hasselbalch 3 a aequation, and it is the fundamental relationship used to predict buffer pH from the relative concentrations of the acid and its conjugate base. The Henderson-Hasselbalch...

## Solution

David answered on Dec 31 2021
Question 1
Vol of buffer taken V2= 25 mL
Vol of HCl required to neuterlise buffer V1= 25 mL (from graph)
Conc of HCl M1= 0.126 M
Conc of base in buffer = M2
By volumetric formula
V1 M1 = V2 M2
M1= 25 mL x 0.126M/25 mL= 0.126 M
So conc of in base in buffer = 0.126 M
Question 2
Vol of buffer taken V2= 25 mL
Vol of NaOH required to neuterlise buffer V1= 10 mL (from graph)
Conc of...
SOLUTION.PDF