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Chapter 15: Problem 21

Write the formula for the hydronium ion. Write an equation for the formation of the hydronium ion when an acid is dissolved in water.

Short Answer

Expert verified
The formula for the hydronium ion is \(H_3O^+\). When an acid (HA) is dissolved in water, the formation of the hydronium ion can be represented by the equation: \(HA + H_2O → H_3O^+ + A^-\).

Step by step solution

01

Determine the formula for the hydronium ion

The hydronium ion is formed when a proton (hydrogen ion, H+) reacts with a water molecule (H2O). The formula for the hydronium ion is H3O+.
02

Write an equation for the formation of the hydronium ion with a generic acid

A general formula for an acid can be represented as "HA," where "H" is the hydrogen atom, and "A" is the anion. When an acid is dissolved in water, it donates a proton (H+) to a water molecule, which then forms the hydronium ion (H3O+), and the remaining anion (A-). The equation for this process is: HA + H2O → H3O+ + A-

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Most popular questions from this chapter

For each hydroxide ion concentration listed, calculate the pOH of the solution as well as the concentration of hydrogen ion in the solution. Indicate whether the solutions are acidic or basic. a. \(\left[\mathrm{OH}^{-}\right]=4.01 \times 10^{-2} \mathrm{M}\) b. \(\left[\mathrm{OH}^{-}\right]=9.87 \times 10^{-9} \mathrm{M}\) c. \(\left[\mathrm{OH}^{-}\right]=5.23 \times 10^{-5} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=6.29 \times 10^{-12} \mathrm{M}\)

As the hydrogen ion concentration of a solution increases, does the pH of the solution increase or decrease? Explain.

Calculate the \(\mathrm{pH}\) of each of the following solutions from the information given. a. \(\mathrm{pOH}=11.31\) b. \(\left[\mathrm{OH}^{-}\right]=7.22 \times 10^{-5} \mathrm{M}\) c. \(\left[\mathrm{H}^{+}\right]=9.93 \times 10^{-4} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=1.49 \times 10^{-8} \mathrm{M}\)

Which of the following bases have relatively strong conjugate acids? a. \(\mathrm{SO}_{4}^{2-}\) b. \(\mathrm{Br}^{-}\) c. \(\mathrm{CN}^{-}\) d. \(\mathrm{CH}_{3} \mathrm{COO}^{-}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\right)\)

Write the conjugate base for each of the following: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}\) b. \(\mathrm{HCO}_{3}^{-}\) C. \(HF\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
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