Ch.15 - Acid and Base EquilibriumWorksheetSee 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 a solution at 25°C in which the [OH] = 5.4 x10  −7 M.A) 4.51B) 7.05C) 7.73D) 6.38E) 8.40

Solution: Calculate the pH of a solution at 25°C in which the [OH−] = 5.4 x10  −7 M.A) 4.51B) 7.05C) 7.73D) 6.38E) 8.40

Problem

Calculate the pH of a solution at 25°C in which the [OH] = 5.4 x10  −7 M.

A) 4.51

B) 7.05

C) 7.73

D) 6.38

E) 8.40

Solution

We’re being asked to calculate for the pH of a solution in which the [OH­-] = 5.4x10-7 M.


The pH and pOH of a compound determine its acidity and basicity.

• pH

▪ pH stands for the negative logarithmic function of hydronium ion concentration
can be calculated using the following equation:

Solution BlurView Complete Written Solution