The acid dissociation constant \( K_a \) of carbonic acid \((\text{H}_2\text{CO}_3)\) is \(4.5 \times 10^{-7}\).Calculate the pH of a \(1.6 \, \text{M}\) solution of carbonic acid. Round your answer to 1 decimal place.**Input Field:**pH = [ ]**Buttons:**- Clear (X)- Undo (⟲)- Help (?)

Given : Concentration of H2CO3 = 1.6 M And Ka (first dissociation) of H2CO3 = 4.5 X 10-7 The first…

Answered: The acid dissociation constant K of…

The acid dissociation constant K of carbonic acid (H,CO, is 4.5 × 10¯'. Calculate the pH of a 1.6 M solution of carbonic acid. Round your answer to 1 decimal place. pH

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...

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Question

The acid dissociation constant \( K_a \) of carbonic acid \((\text{H}_2\text{CO}_3)\) is \(4.5 \times 10^{-7}\).

Calculate the pH of a \(1.6 \, \text{M}\) solution of carbonic acid. Round your answer to 1 decimal place.

**Input Field:**
pH = [ ]

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