**Calculate the pH at the equivalence point in titrating 0.020 M solutions of each of the following with 0.039 M NaOH.**(a) **Perchloric acid (HClO₄)** pH = _______(b) **Hydrazoic acid (HN₃), Kₐ = 1.9e-05** pH = _______(c) **Carbonic acid (H₂CO₃), Kₐ = 4.3e-07** pH = _______ This section provides exercises on calculating the pH at the equivalence point for titrations involving perchloric acid, hydrazoic acid, and carbonic acid. The titrations are done using a 0.039 M NaOH solution. It includes the acid dissociation constants (Kₐ) for weak acids to assist with the calculations.

Answered: Calculate the pH at the equivalence…

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

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**Calculate the pH at the equivalence point in titrating 0.020 M solutions of each of the following with 0.039 M NaOH.**

(a) **Perchloric acid (HClO₄)**
pH = _______

(b) **Hydrazoic acid (HN₃), Kₐ = 1.9e-05**
pH = _______

(c) **Carbonic acid (H₂CO₃), Kₐ = 4.3e-07**
pH = _______

This section provides exercises on calculating the pH at the equivalence point for titrations involving perchloric acid, hydrazoic acid, and carbonic acid. The titrations are done using a 0.039 M NaOH solution. It includes the acid dissociation constants (Kₐ) for weak acids to assist with the calculations.

Expert Solution

Step 1

pH is the power of hydronium ion concentration. It is used to measure the acidity or alkalinity of a substance. For acidic substances, the pH value is less than 7 and for bases, it is more than 7. If the pH is 7, the substance is neutral.

Given: The concentration of HClO₄, HN₃, and H₂CO₃ is 0.020 M and the concentration of NaOH is 0.039 M. The value of K_a (acid dissociation constant) for hydrazine (HN₃) is $1.9 \times 10^{- 5}$ , and for carbonic acid (H₂CO₃) is $4.3 \times 10^{- 7}$ .

To calculate: pH

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