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 mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each pH value?pH = 2.60

Solution: What mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each pH value?pH = 2.60

Problem

What mass of HClO4 should be present in 0.600 L of solution to obtain a solution with each pH value?

pH = 2.60

Solution

We are asked for the mass of HClO4 that should be present in a 0.600 L solution to obtain a pH value of 2.60. 

Remember that HClO4 is a strong, monoprotic oxyacid. It’s a strong oxyacid since there are 3 more O than H in the formula. 


Recall that strong acids completely dissociate in water and that acids donate H+ to the base (water in this case). The dissociation of HClO4 is as follows:


HClO4(aq) + H2O(l)  H3O+(aq) + ClO4(aq)


For strong acids, an ICE table is not necessary because it can be assumed that all of the acid or base will dissociate. 


The concentration of the strong acid is the same as its dissociated particles.


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