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.

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. (A) 3.0 (B) 10.0 (C) 7. 1 (D) 8.2

Tardigrade Admin · Accepted Answer

K=Ka1 × Ka2 =4.5 × 10-3 × 1.7 × 10-10 =7.65 × 10-13 [ H +] =√K ⋅ C =√7.65 × 10-13 × 0.01 =8.7 × 10-8 pH =- log [ H +]=- log 8.7 × 10-8 =-( log 10-8+ log 8.7) =8-0.93 ⇒ =7.07

Q. What is the pH of 0.01M glycine solution? For glycine Ka1​​=4.5×10−3 and Ka2​​=1.7×10−10 at 298K.

3.0

10.0

7. 1

8.2

K=Ka1​​×Ka2​​=4.5×10−3×1.7×10−10 =7.65×10−13 [H+]=K⋅C​ =7.65×10−13×0.01​ =8.7×10−8 pH=−log[H+]=−log8.7×10−8 =−(log10−8+log8.7) =8−0.93 ⇒=7.07

Q. What is the $p H$ of $0.01 M$ glycine solution? For glycine $K_{a_{1}} = 4.5 \times 1 0^{- 3}$ and $K_{a_{2}} = 1.7 \times 1 0^{- 10}$ at $298 K$ .