Ch.15 - Acid and Base EquilibriumWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.95 L of an HCl solution with a pH of 1.8?

Solution: What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.95 L of an HCl solution with a pH of 1.8?

Problem

What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.95 L of an HCl solution with a pH of 1.8?

Solution

We have to determine the volume of 36.0 % by mass HCl solution required to prepare 4.95 L of a solution with a pH of 1.8.


Recall: halogen binary acids are strong acids, except HF.

HCl is a strong acid and dissociates completely in solution.

HCl → H+ + Cl-


We will solve this problem through these steps:

Step 1: Calculate the concentration of final solution using the given pH.

Step 2: Calculate the molarity of 36.0 % by mass HCl solution (stock solution).

Step 3: Use the dilution formula and calculate the required volume.

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