ElectrochemistryEasy
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 298K ?
Options
A.3.0
B.10.0
C.6.1
D.7.1
Solution
For glycine solution ;
K = Ka1 × Ka2
= 4.5 × 10-13 × 1.7 × 10-10
= 7.65 × 10-13+] =
=
= 8.7 × 10-8
Hence, pH = - log[H+]
= - log[8.7 × 10-8]
= - (log10-8 + log8.7)
8 - 0.93 = 7.07 ≈ 7.1
K = Ka1 × Ka2
= 4.5 × 10-13 × 1.7 × 10-10
= 7.65 × 10-13+] =
=
= 8.7 × 10-8Hence, pH = - log[H+]
= - log[8.7 × 10-8]
= - (log10-8 + log8.7)
8 - 0.93 = 7.07 ≈ 7.1
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
Assuming that hydrogen behaves as an ideal gas, what is the EMF of the cell at 25°C if P1 = 600 mm and P2 = 420 mm: Pt |...Faraday′s laws of electrolysis are related to the :...An electrolytic cell contains a solution of Ag2SO4 and platinum electrodes. A current is passed until 1.6 g of O2 has be...Select the correct option if it is known that Ksp (AgCl) > Ksp (AgBr) > Ksp (AgI)...Most of the copper used to make wire has been electrically refined by depositing it from copper salts solution (divalent...