SATHEE: Equilibrium Question 307

Equilibrium Question 307

Question: What is the pH of 0.01 M glycine solution’ For glycine, $K a_{1} = 4.5 \times 10^{- 3}$ and $K a_{2} = 1.7 \times 10^{- 10}$ at 298 K [AIIMS 2004]

Options:

A) 3.0

B) 10.0

C) 6.1

D) 7.2

Show Answer

Answer:

Correct Answer: C

Solution:

$K = K a_{1} \times K a_{2}$

$= 4.5 \times 10^{- 3} \times 1.7 \times 10^{10}$

$H^{+} = \sqrt{K c}$

$= \sqrt{4.5 \times 10^{- 3} \times 1.7 \times 10^{- 10} \times .01}$

$= .87 \times 10^{- 7}$

$p H = - \log 0.87 \times 10^{- 7}$

$= 7 - 0.93 = 6.07$ .

पिछला

अगला

गोपनीयता नीति

द्वारा संचालित Prutor@IITK

sathee@iitk.ac.in

SATHEE का मीडिया कवरेज

खेल स्टोर

ऐप स्टोर

Ask SATHEE

Welcome to SATHEE !
Select from 'Menu' to explore our services, or ask SATHEE to get started. Let's embark on this journey of growth together! 🌐📚🚀🎓

I'm relatively new and can sometimes make mistakes.
If you notice any error, such as an incorrect solution, please use the thumbs down icon to aid my learning.
To begin your journey now, click on "I understand".

Equilibrium Question 307

Question: What is the pH of 0.01 M glycine solution’ For glycine, Ka1=4.5×10−3 and Ka2=1.7×10−10 at 298 K [AIIMS 2004]

Options:

Answer:

Solution:

इंजीनियरिंग की तैयारी

चिकित्सा तैयारी

एनसीईआरटी पुस्तकें और समाधान

महत्वपूर्ण संसाधन

अन्य संसाधन

पाठ्यक्रम

परीक्षा मंच

नमूना मॉक टेस्ट

सदस्यता

एनसीईआरटी व्यायाम वीडियो समाधान

Menu

Question: What is the pH of 0.01 M glycine solution’ For glycine, $K a_{1} = 4.5 \times 10^{- 3}$ and $K a_{2} = 1.7 \times 10^{- 10}$ at 298 K [AIIMS 2004]