Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
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: Calculate the pH of the resulting solution if 27.0 ml of 0.270 M HCl is added toa) 32.0 ml of 0.270 M NaOH(aq) b) 37.0 ml of 0.320 M NaOH(aq)

Problem

Calculate the pH of the resulting solution if 27.0 ml of 0.270 M HCl is added to

a) 32.0 ml of 0.270 M NaOH(aq)


b) 37.0 ml of 0.320 M NaOH(aq)

Solution

NaOH is a strong base while HCl is a strong acid. No ICE or ICF chart is needed.


A. First, calculate the amount of acid and base that will react

molarity (volume) → moles

Recall:

molarity (M)=moles of soluteL of solution


*convert mL to L → 1 mL = 10-3 L


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