Explain why the solution prepared in part a is a buffer splution. Hint: re read the first page of this experiment: Answer the following questions (la-d and 2a-c). Make sure you place the prelab pages on theinstructor's bench.These calculations relate to the lab. You will not be able to do the lab without havingthese calculations done first!Given:-CH,COOH= 25.0mL-ICHCO0H]= 0.10MKa=1.8x/0-5"- NACH, C00= 20.0 mL-INACH3CO0]= 10.0M= [CH3C00]1. a. What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka= 1.8 x 105) and 20.0, mL of 0.10 M sodium acetate?Dissociation Rxn:CH3CO0H + H20= CHg C 0O+Hg0+Base Conugate Con usateAcidBase6Using Equation:pH=pKqt log Ilonj. BroelAcid]Henderson-Hasselkach[Conj. BaselF(20.0mL)(0.10mol)(25.0+20.0) mLpH = -log(1.8x10-9) + log T 25.0 umL (onO kap(25.0+20.0) mLpH=4.4478 Prelab: Before coming to lab, outline the procedures and neatly prepare the followingdata tables in your lab notebook.Data Table 1: Testing of Buffer Solution and WaterInitial pHSolutionAfter 5.0 mL HCIAfter 5.0 mL NAOHHC2H3O2/ C2H;O2H2OData Table 2: Ammonia Buffers# Drops of 1.0 MHCIto reach pH =8.00# Drops of 1.0 M NAOH toreach pH = 10.00BufferNote to students:This is how you'll count1) NH3 NH4 ag solutionsyour drops:Make thase boxes plenty lrgeyou will record many deopsHITIl etc...Some solution may équireuprds of I00 ops or moreMake these boxes plentylarge, you will recorddropsmany2) NH3/solid NHẠC1Some solution may requireupwards of 100 drops ormore3) NH: titrated with HCI

Answered: 1. a. What is the pH of a solution…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Concept explainers

Question

Explain why the solution prepared in part a is a buffer splution. Hint: re read the first page of this experiment:

Prelab: Before coming to lab, outline the procedures and neatly prepare the following
data tables in your lab notebook.
Data Table 1: Testing of Buffer Solution and Water
Initial pH
Solution
After 5.0 mL HCI
After 5.0 mL NAOH
HC2H3O2/ C2H;O2
H2O
Data Table 2: Ammonia Buffers
# Drops of 1.0 MHCI
to reach pH =8.00
# Drops of 1.0 M NAOH to
reach pH = 10.00
Buffer
Note to students:
This is how you'll count
1) NH3 NH4 ag solutions
your drops:
Make thase boxes plenty lrge
you will record many deops
HITI
l etc...
Some solution may équire
uprds of I00 ops or more
Make these boxes plenty
large, you will record
drops
many
2) NH3/solid NHẠC1
Some solution may require
upwards of 100 drops or
more
3) NH: titrated with HCI

Expert Solution

Step 1

25.0 mL of 0.1 M acetic acid and 20 ml of 0.1 M sodium acetate are mixed.

Acetic acid is a weak acid and acetate is a salt obtained by the neutralization of weak acetic acid and a strong base. A mixture of weak acid and its salt with strong base act as acidic buffer.

pH of a buffer can be calculated using the expression:

$p H = p K_{a} + \log \frac{[C o n j u g a t e b a s e]}{[A c i d]}$

K_a = 1.8 * 10^-5

pKa = -log(1.8 * 10^-5)

= 5 - log 1.8

= 5 - 0.2553

= 4.7447

= 4.74

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions