Escriba la ecuación química y la expresión de la Ka de la disociación ácida de los ácidos siguie

step 1 Chapter 16, Problem 50. Chemistry. The Central Science. So the question's asking us to write a c

Escriba la ecuación química y la expresión de la Ka de la...

Escriba la ecuación química y la expresión de la $K_{\mathrm{a}}$ de la disociación ácida de los ácidos siguientes en disolución acuosa. Primero muestre la reacción con $\mathrm{H}^{+}$(ac) como un producto y luego con el ion hidronio: (a) $\mathrm{HC}_6 \mathrm{H}_5 \mathrm{O}$; (b) $\mathrm{HCO}_3^{-}$.

Key Concepts

Acid Dissociation Reaction

This concept involves the process by which an acid donates a proton (H?) to a solvent, typically water. It is central to acid-base chemistry, and the reaction is often written showing the acid on the left side and its conjugate base along with a proton or hydronium ion on the right side. It helps in understanding how acids behave in aqueous solutions by transforming into species that affect the pH of the system.

Acid Dissociation Constant (Ka)

The acid dissociation constant, Ka, is a quantitative measure of the strength of an acid in solution. It is defined by the equilibrium expression that relates the concentrations of the products and the reactants in the dissociation reaction. A higher Ka value indicates a stronger acid that more completely donates its proton in water, while a lower Ka value signifies a weaker acid.

Chemical Equilibrium Expression

This concept refers to writing the mathematical expression that defines the state of equilibrium in a chemical reaction. In the context of acid dissociation, the equilibrium expression is the ratio of the concentration of the products (including the proton or hydronium ion and the conjugate base) to the concentration of the undissociated acid. Understanding this allows one to predict the position of equilibrium and calculate the extent of acid dissociation.

Representation of the Proton and Hydronium Ion in Acid-Base Reactions

In aqueous solutions, free protons (H?) do not exist independently but associate with water molecules to form the hydronium ion (H?O?). Recognizing this concept is essential when writing accurate chemical equations for acid dissociation, as it reflects the realistic depiction of the species present in the solvent and is critical when deriving or using the equilibrium constant expressions.

Transcript

00:01 Chapter 16, problem 50.

00:06 Chemistry.

00:10 The central science.

00:12 So the question's asking us to write a chemical equation in the ca expression for acid dissociation for different acids.

00:22 And so they want you to write it with using h -plus and then also using as a hydrogenium ion.

00:28 So for part a, our acid is c6.

00:37 H5c -o -o -h and that is going to then dissociate into c6 h5 c -o and then h -plus and that's going to be a minus.

00:58 And so we also need to make sure we write our states on here so they are all aqueous states.

01:10 So now since we have our expression for our chemical equation, now we can write our k -a expression.

01:19 And our k -a expression is always going to be our products over our products.

01:25 Sorry.

01:28 It's always our products over our reactants.

01:32 And our products are going to be the concentration of our c -6 -h -5 -c -o -0 -minus times our h -plus.

01:43 Over our c6h5c -o -h concentration.

01:51 All right, so that was the first part of it.

01:53 And so the second part, they asked us to write it with a hydronium ion.

01:56 And so to get a hydronium ion, our hydronium ion is the h3o plus.

02:02 And so to do that, we have to have it with water.

02:05 So therefore, we'll do c6h5c -o -h aqueous, plus h2o, which is the liquid, goes to c6h5 c -o -0 -minus, plus h3o -plus equates...

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