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 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 5.05 L of an NaOH solution with a pH of 10.6?

Solution: What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 5.05 L of an NaOH solution with a pH of 10.6?

Problem

What volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 5.05 L of an NaOH solution with a pH of 10.6?

Solution

We are being asked to what volume of a 15.0% by mass NaOH solution, which has a density of 1.116 g/mL, should be used to make 5.05 L of a NaOH solution with a pH of 10.6.


For NaOH:

Any Group 1A metal when combined with OH-, H-, O2- or NH2- makes a strong base
Na (Group 1A metal) is paired with OH-
NaOH → strong base


Since NaOH is a strong base, it will completely dissociate in the solution:

NaOH(aq) → Na+(aq) +  OH-(aq)

Since the pH of the solution is given. We need to compute for pOH to calculate for the concentration of [OH-]. 

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