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Chapter 15: Problem 84

What is the value of the equilibrium constant for the dissociation of the first proton of sulfuric acid? What does this value tell you?

Short Answer

Expert verified
The value of the equilibrium constant (Ka) for the dissociation of the first proton of sulfuric acid (H2SO4) is around \(10^3\). This large value indicates that H2SO4 is a strong acid, meaning it ionizes almost completely in water and readily donates its first proton, forming hydrogen ions (H+) and bisulfate ions (HSO4-) in aqueous solutions.

Step by step solution

01

Write the chemical equation for the dissociation of the first proton of H2SO4

The chemical equation for the first dissociation of sulfuric acid can be written as follows: H2SO4 (aq) -> H+ (aq) + HSO4- (aq) In this chemical equation, H2SO4 releases one hydrogen ion (H+) and forms the bisulfate ion (HSO4-).
02

Write down the Ka expression for this reaction

The equilibrium constant expression for this reaction can be written as: Ka = \([H^+][HSO4^-] / [H2SO4]\) Ka represents the equilibrium constant for the acid dissociation of H2SO4, and [H+], [HSO4-], and [H2SO4] are the equilibrium concentrations of hydrogen ions (H+), bisulfate ions (HSO4-), and sulfuric acid (H2SO4), respectively.
03

Find the equilibrium constant (Ka) value for the dissociation of the first proton of H2SO4

The Ka value for the dissociation of the first proton of H2SO4 can be found in the literature or on resources like a chemistry textbook or online databases of acid dissociation constants. The value of Ka for the first dissociation of sulfuric acid is very large, generally considered to be around \(10^3\). This indicates that the reaction is strongly favored for ions dissociation.
04

Interpret the meaning of the Ka value

Since the calculated Ka value for the first dissociation of H2SO4 (\(10^3\)) is very large, it suggests that sulfuric acid is a strong acid. A strong acid ionizes in water almost completely, meaning that it donates its first proton readily in aqueous solution. In this case, almost all sulfuric acid molecules dissociate into hydrogen ions (H+) and bisulfate ions (HSO4-) when in water. In conclusion, the Ka value for the first proton dissociation of sulfuric acid is around \(10^3\), and this large value indicates that H2SO4 is a strong acid and dissociates almost completely in aqueous solutions.

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Most popular questions from this chapter

Classify each substance as strong electrolyte, weak electrolyte, or nonelectrolyte: (a) \(\mathrm{CH}_{3} \mathrm{COOH}\) (b) \(\mathrm{KCH}_{3} \mathrm{COO}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (e) \(\mathrm{NH}_{3}\) (f) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (g) \(\mathrm{ZnSO}_{4}\)

Acetic acid is a weak acid. Upon losing a proton, acetic acid yields the acetate anion. (a) Draw a dot diagram for the acetate anion. (b) Hydrogen atoms that are bound to carbon atoms are not acidic. Knowing this, is it possible for the acetate anion to serve as an acid? Explain. (c) In fact, acetate ion is a weak base. Write a chemical equilibrium with unequal-length arrows showing how acetate in water produces a weakly basic solution. (d) Is water acting as an acid or a base? Explain.

If you dissolve \(0.250 \mathrm{~g}\) of \(\mathrm{Ba}(\mathrm{OH})_{2}\) in \(3.00 \mathrm{~L}\) of water, what is the \(\mathrm{pH}\) of the solution?

Complete the following sentence: "The lower the \(\mathrm{p} K_{\mathrm{a}}\), the (stronger/weaker) the acid." \(^{\prime \prime}\) How does this parallel pH?

How many moles of \(\mathrm{Ba}(\mathrm{OH})_{2}\) does it take to neutralize \(0.50\) mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) ? Why does the resulting solution after the neutralization no longer conduct electricity? Why does the solution then conduct electricity after an excess of \(\mathrm{Ba}(\mathrm{OH})_{2}\) is added?
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