Question

From the $K_a$ values for fumaric acid, $K_{a1} = 9.50 \times 10^{-4}$ and $K_{a2} = 3.30 \times 10^{-5}$, calculate the two $K_b$ values of fumarate.

Name: From the Ka values for fumaric acid, Ka1 = 9.50 × 10^-4 and Ka2 = 3.30 × 10^-5, calculate the two Kb values of fumarate.
Uploaded: 2023-08-18T14:39:47-08:00
Duration: 1 min 38 s
Channel: Sima Sarker
Description: From the Ka values for fumaric acid, Ka1 = 9.50 × 10^-4 and Ka2 = 3.30 × 10^-5, calculate the two Kb values of fumarate.

          From the $K_a$ values for fumaric acid, $K_{a1} = 9.50 \times 10^{-4}$ and $K_{a2} = 3.30 \times 10^{-5}$, calculate the two $K_b$ values of fumarate.

Added by Matthew H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sima Sarker

08/18/2023

Step 1

For a conjugate acid-base pair, the product of the acid dissociation constant ($ K_a $) and the base dissociation constant ($ K_b $) is equal to the ion product of water ($ K_w $), which is $ 1.0 \times 10^{-14} $ at 25°C. \[ K_a \times K_b = K_w \] Show more…

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_(0)^(infty ) From the K_(a) values for fumaric acid, K_(a1)=9.50 imes 10^(-4) and K_(a2)=3.30 imes 10^(-5), calculate the two K_(b) values of fumarate. K_(b2)= From the Ka values for fumaric acid, Ka1 = 9.50 10-4 and Ka2 = 3.30 10-5, calculate the two Kb values of fumarate Macmillan Learnin Kb1= Kb2=