Skip to main content
Ch.17 - Acids and Bases
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.17 - Acids and BasesProblema 60
Capitolo 17, Problema 60

What mass of HClO4 must be present in 0.500 L of solution to obtain a solution with each pH value? a. pH = 2.50 b. pH = 1.50 c. pH = 0.50

Guida verificata passo dopo passo
1
insert step 1> Calculate the concentration of hydrogen ions \([H^+]\) using the pH formula: \([H^+] = 10^{-\text{pH}}\). For pH = 1.50, find \([H^+]\).
insert step 2> Recognize that perchloric acid \(\text{HClO}_4\) is a strong acid and dissociates completely in water, so \([H^+] = [\text{HClO}_4]\).
insert step 3> Use the concentration of \([H^+]\) to find the moles of \(\text{HClO}_4\) in the 0.500 L solution. Use the formula: \(\text{moles} = \text{concentration} \times \text{volume}\).
insert step 4> Calculate the molar mass of \(\text{HClO}_4\) by adding the atomic masses of hydrogen, chlorine, and oxygen.
insert step 5> Convert the moles of \(\text{HClO}_4\) to mass using the formula: \(\text{mass} = \text{moles} \times \text{molar mass}\).

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.

pH and its Calculation

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. The formula pH = -log[H+] allows us to calculate the concentration of hydrogen ions in a solution. For a pH of 1.50, the hydrogen ion concentration can be determined as [H+] = 10^(-1.50), which is essential for further calculations.
Video consigliato:
Percorso guidato
02:15
pH Calculation Example

Strong Acids and Their Ionization

Strong acids, like HClO4 (perchloric acid), completely dissociate in water, meaning that the concentration of the acid equals the concentration of hydrogen ions produced. This complete ionization simplifies calculations, as the molarity of the acid directly corresponds to the molarity of H+ ions in the solution, which is crucial for determining the mass needed to achieve a specific pH.
Video consigliato:
Percorso guidato
01:09
Strong Acid-Strong Base Titration

Molarity and Mass Calculations

Molarity (M) is defined as the number of moles of solute per liter of solution. To find the mass of HClO4 required, we first calculate the moles needed using the desired hydrogen ion concentration and the volume of the solution. Then, using the molar mass of HClO4, we can convert moles to grams, allowing us to determine the mass of the acid needed to achieve the specified pH.
Video consigliato:
Percorso guidato
03:12
Molar Mass Calculation Example
Pratica correlata
Domanda del libro di testo

What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?

a. pH = 1.25 b. pH = 1.75 c. pH = 2.85

108
views
Domanda del libro di testo

Determine the [H3O+] and pH of a 0.100 M solution of benzoic acid.

801
views
Domanda del libro di testo

What is the pH of a solution in which 224 mL of HCl(g), measured at 27.2 °C and 1.02 atm, is dissolved in 1.5 L of aqueous solution?

1263
views
Domanda del libro di testo

For each strong acid solution, determine [H3O+], [OH–], and pH. d. a solution that is 0.655% HNO3 by mass (assume a density of 1.01 g/mL for the solution)

1747
views
Domanda del libro di testo

Determine the [H3O+] and pH of a 0.200 M solution of formic acid.

542
views
1
rank
Domanda del libro di testo

For each strong acid solution, determine [H3O+], [OH–], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO3

1008
views