Interpretation Introduction To determine: [ H + ] and [ OH − ] for a neutral solution of water at its freezing point. Explanation Given At the freezing point of water ( 0 °C ) , K w = 1.2 × 10 − 15 . At the freezing point of water, its autoionization decreases; hence, the concentration of both H + and OH − decreases to the same extent. So, even at freezing point when K w = 1.2 × 10 − 15 , the concentration of H + and OH − in the neutral water remain the same and is given by the expression, [ H + ] = [ OH − ] .....(1) Where, [ H + ] is the hydrogen ion concentration of the given solution of water. [ OH − ] is the hydroxyl ion concentration of the given solution of water. Ionic product of water is given by the formula, K w = [ H + ] [ OH − ] Where, K w is the ion-product constant of water at freezing point

Chemistry: The Central Science, Books a la Carte Edition & Modified Mastering Chemistry with Pearson eText -- ValuePack Access Card Package

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ISBN: 9780133910919

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus

Publisher: PEARSON

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Chapter 24, Problem 68E

Interpretation Introduction

To determine: [H+] and [OH−] for a neutral solution of water at its freezing point.

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Chapter 24, Problem 67E

Chapter 24, Problem 69E

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Chapter 24 Solutions

Chemistry: The Central Science, Books a la Carte Edition & Modified Mastering Chemistry with Pearson eText -- ValuePack Access Card Package

Ch. 24.2 - Prob. 24.1.1PE Ch. 24.2 - The equilibrium constant Kc for C(s) +CO2 2CO(g)...Ch. 24.2 - Prob. 24.2.1PE Ch. 24.2 - Le Chatelier noted that many industrial processes...Ch. 24.3 - Prob. 24.3.1PE Ch. 24.3 - Prob. 24.3.2PE Ch. 24.3 - [15.91] An equilibrium mixture of H2, I2, and HI...Ch. 24.3 - Consider the hypothetical reaction A(g) + 2B(g) 2...Ch. 24.3 - Prob. 24.5.1PE Ch. 24.3 - Prob. 24.5.2PE

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