For each of the following: (11.2,11.3) 1. H2 S 2. H3 PO4 a. Write the formula for the conjugate

step 1 Hello there. Today for this problem, they want to know for each of the following, where we have

For each of the following: (11.2,11.3) 1. H2 S 2. H3 PO4 a....

For each of the following: $(11.2,11.3)$
1. $\mathrm{H}_{2} \mathrm{~S}$
2. $\mathrm{H}_{3} \mathrm{PO}_{4}$
a. Write the formula for the conjugate base.
b. Write the $K_{\mathrm{a}}$ expression.
c. Which is the weaker acid?

Key Concepts

Polyprotic Acids

Polyprotic acids are acids that can donate more than one proton, and each deprotonation step has its own equilibrium constant (Ka1, Ka2, etc.). Recognizing the stepwise dissociation process in polyprotic acids is crucial for correctly identifying the conjugate bases at different stages of deprotonation and for writing the appropriate equilibrium expressions for each dissociation step.

Conjugate Base

The conjugate base is the species that remains after an acid donates a proton. It is essential in understanding acid–base reactions because the equilibrium between an acid and its conjugate base governs the extent of proton donation. Recognizing the conjugate base helps in correctly writing acid dissociation reactions and understanding the behavior of acids in solution.

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 for the acid dissociation reaction, relating the concentrations of the products (hydronium ion and conjugate base) to the concentration of the undissociated acid. A larger Ka value indicates a stronger acid, while a smaller Ka value signifies a weaker acid.

Acid Strength Comparison

Comparing the strengths of acids involves analyzing their Ka values. In any given acid–base reaction, a higher Ka means the acid more readily donates its proton, signifying a stronger acid. Understanding this relationship is important when evaluating acid behavior and predicting the outcome of acid–base reactions.

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