Skip to main content
Ch.17 - Acids and Bases
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.17 - Acids and BasesProblema 86b
Capitolo 17, Problema 86b

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. b. 0.0112 M Ba(OH)2

Guida verificata passo dopo passo
1
Determine the concentration of hydroxide ions, [OH^-], from the dissociation of Ba(OH)_2. Since Ba(OH)_2 is a strong base, it dissociates completely in water. Each formula unit of Ba(OH)_2 produces two OH^- ions. Therefore, [OH^-] = 2 \(\times\) 0.0112 \, M.
Calculate the concentration of hydronium ions, [H_3O^+], using the relationship between [OH^-] and [H_3O^+]. The product of [OH^-] and [H_3O^+] is equal to the ion product of water, K_w = 1.0 \(\times\) 10^{-14} \, at \, 25^\(\circ\) C. Use the formula [H_3O^+] = \(\frac{K_w}{[OH^-]}\).
Determine the pOH of the solution using the formula pOH = -\(\log\)[OH^-].
Calculate the pH of the solution using the relationship between pH and pOH: pH + pOH = 14.
Summarize the results: [OH^-], [H_3O^+], pH, and pOH for the 0.0112 M Ba(OH)_2 solution.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
1m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Strong Bases

Strong bases are substances that completely dissociate in water to produce hydroxide ions (OH-). Common examples include alkali metal hydroxides and alkaline earth metal hydroxides, such as Ba(OH)2. The concentration of the base directly correlates to the concentration of OH- ions in solution.
Video consigliato:
Percorso guidato
01:09
Strong Acid-Strong Base Titration

pH and pOH Calculations

pH and pOH are measures of the acidity and basicity of a solution, respectively. pH is calculated as the negative logarithm of the hydronium ion concentration ([H3O+]), while pOH is the negative logarithm of the hydroxide ion concentration ([OH-]). The relationship between pH and pOH is given by the equation pH + pOH = 14 at 25°C.
Video consigliato:
Percorso guidato
02:09
pH and pOH Calculations

Ion Product of Water

The ion product of water (Kw) is the equilibrium constant for the self-ionization of water, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C. This relationship allows for the calculation of [H3O+] when [OH-] is known, and vice versa, which is essential for determining pH and pOH in strong base solutions.
Video consigliato:
Percorso guidato
00:53
Production of Hydrogen Example
Pratica correlata
Domanda del libro di testo

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 0.15 M NaOH b. 1.5×10–3 M Ca(OH)2 c. 4.8×10–4 M Sr(OH)2 d. 8.7×10–5 M KOH

681
views
Domanda del libro di testo

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. c. 1.9×10–4 M KOH

295
views
Domanda del libro di testo

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. a. 8.77×10–3 M LiOH

1690
views
2
rank
Domanda del libro di testo

Determine the pH of a solution that is 3.55% KOH by mass. Assume that the solution has density of 1.01 g/mL.

Domanda del libro di testo

For each strong base solution, determine [OH–], [H3O+], pH, and pOH. d. 5.0×10–4 M Ca(OH)2

375
views