(a) Explanation i. The stated reaction, HCO 3 − ( a q ) → CO 3 − ( a q ) + H + ( a q ) The value of K a is 5 .6 × 10 − 11 . The reaction of dissociation of water is, H + ( a q ) + OH − ( a q ) → H 2 O ( a q ) The value of K eq can be calculated by the following formula, K eq × K a = K w Where, K eq is the equilibrium constant. K a is the acid dissociation constant. K w is the ionic product of water. Rearrange the above formula to calculate the value of K eq , K eq = K w × 1 / K a Substitute the value of K a and K w in the above expression, K eq = 1 .00 × 10 14 × 5 .6 × 10 − 11 = 5 (b) Interpretation Introduction To determine: The equilibria that can be written with a single arrow.

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Chapter 16, Problem 126IE

(a)

Interpretation Introduction

To determine: The value of the equilibrium constant for the given reaction.

(b)

Interpretation Introduction

To determine: The equilibria that can be written with a single arrow.

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Chapter 16, Problem 125IE

Chapter 17.1, Problem 17.1.1PE

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Chapter 16 Solutions

MAST F/ CHEM: THE CENTRAL SCI CODE ALON

Ch. 16.2 - Practice Exercise 1 Consider the following...Ch. 16.2 - Prob. 16.1.2PE Ch. 16.2 - Prob. 16.2.1PE Ch. 16.2 - Practice Exercise 2 When lithium oxide (Li2O) is...Ch. 16.2 - Based on information in Figure 16.4, place the...Ch. 16.2 - Practice Exercise 2 For each reaction, use Figure...Ch. 16.3 - Practice Exercise 1 In a certain acidic solution...Ch. 16.3 - Practice Exercise 2 Indicate whether solutions...Ch. 16.3 - Prob. 16.5.1PE Ch. 16.3 - Prob. 16.5.2PE

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