If Kb for ammonia is 1.8 ×10^-5, calculate Ka for its conjugate acid, NH4^+. Note that NH3 is th

Name: Problem 16, Chapter 15: Chemistry Principles and Practice
Uploaded: 2020-07-09T15:15:40-08:00
Duration: 3 min 2 s
Channel: Ahmed Ali
Description: If Kb for ammonia is 1.8 ×10^-5, calculate Ka for its conjugate acid, NH4^+. Note that NH3 is the conjugate acid of the amide ion, NH2^-. Can Ka and Kb for the NH3 |NH2^- pair be calculated from the preceding data and the value of Kw ?

step 1 Hello everyone my name is Ahmed Ali and this question the ammonia is a weak base so when react t

If Kb for ammonia is 1.8 ×10^-5, calculate Ka for its...

If $K_{\mathrm{b}}$ for ammonia is $1.8 \times 10^{-5},$ calculate $K_{\mathrm{a}}$ for its conjugate acid, $\mathrm{NH}_{4}^{+}$. Note that $\mathrm{NH}_{3}$ is the conjugate acid of the amide ion, $\mathrm{NH}_{2}^{-}$. Can $K_{\mathrm{a}}$ and $K_{\mathrm{b}}$ for the $\mathrm{NH}_{3} \mid \mathrm{NH}_{2}^{-}$ pair be calculated from the preceding data and the value of $K_{\mathrm{w}} ?$

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Key Concepts

Conjugate Acid-Base Pairs

This concept refers to the idea that every acid has a corresponding conjugate base, and every base has a corresponding conjugate acid. When an acid donates a proton, the species left behind is its conjugate base, and when a base accepts a proton, the resulting species is its conjugate acid. Understanding this relationship is crucial for analyzing acid-base equilibria and predicting the behavior of species in solution.

Acid and Base Dissociation Constants (Ka and Kb)

Ka and Kb represent the equilibrium constants for the dissociation of acids and bases, respectively. Ka is a measure of how well an acid donates a proton in water, while Kb measures how well a base accepts a proton. These constants are essential for quantifying the strength of acids and bases and determining the direction and extent of acid-base reactions.

Relationship Between Ka, Kb, and the Water Ionization Constant (Kw)

The product of the acid dissociation constant (Ka) of a conjugate acid and the base dissociation constant (Kb) of its conjugate base is equal to the ionization constant of water (Kw). This relationship, expressed as Ka × Kb = Kw, allows one to calculate one constant if the other and Kw are known. This is particularly useful in acid-base chemistry for connecting the strengths of conjugate pairs.

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