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Ch.16 - Acids and Bases
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.16 - Acids and BasesProblem 59
Chapter 16, Problem 59

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

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1
Determine the concentration of hydrogen ions [H^+] in the solution using the pH value. Use the formula: [H^+] = 10^{-pH}.
Substitute the given pH value (1.75) into the formula to find [H^+].
Recognize that HI is a strong acid and dissociates completely in water, so the concentration of HI is equal to the concentration of [H^+].
Calculate the moles of HI required using the concentration of HI and the volume of the solution (0.250 L). Use the formula: moles of HI = [HI] * volume.
Convert the moles of HI to mass using the molar mass of HI. Use the formula: mass = moles * molar mass of HI.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

pH and Hydrogen Ion Concentration

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. A lower pH indicates a higher concentration of hydrogen ions (H+), while a higher pH indicates a lower concentration. For example, a pH of 1.75 corresponds to a hydrogen ion concentration of approximately 0.0178 M.
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Molarity and Solution Concentration

Molarity (M) is a way to express the concentration of a solution, defined as the number of moles of solute per liter of solution. To find the mass of a solute needed to achieve a specific molarity, one can use the formula: mass = molarity × volume × molar mass. This concept is essential for calculating how much HI is required to reach the desired pH.
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Dissociation of HI in Solution

Hydrogen iodide (HI) is a strong acid that completely dissociates in water to produce hydrogen ions (H+) and iodide ions (I-). This complete dissociation means that the concentration of H+ ions in the solution is equal to the concentration of HI initially added. Understanding this dissociation is crucial for determining the amount of HI needed to achieve a specific pH.
Related Practice
Textbook Question

Determine the pH of each solution. a. 0.048 M HI b. 0.0895 M HClO4 c. a solution that is 0.045 M in HClO4 and 0.048 M in HCl d. a solution that is 1.09% HCl by mass (assume a density of 1.01 g/mL for the solution)

Textbook Question

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?

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Textbook Question

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)

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Textbook Question

For each strong acid solution, determine [H3O+], [OH–], and pH. b. 0.015 M HNO3

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Textbook Question

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

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