Ch.16 - Aqueous Equilibrium WorksheetSee 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: The samples of nitric and acetic acid shown here are both titrated with a 0.100 M solution of NaOH(aq). Determine whether each of the following statements concerning these titrations is true or false. The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration.

Solution: The samples of nitric and acetic acid shown here are both titrated with a 0.100 M solution of NaOH(aq).Determine whether each of the following statements concerning these titrations is true or false.T

Problem

The samples of nitric and acetic acid shown here are both titrated with a 0.100 M solution of NaOH(aq).
Determine whether each of the following statements concerning these titrations is true or false.
Two flasks. The left has 25.0 milliliters of 1.0 molar HNO3 (aqueous); the right has 25.0 milliliters of 1.0 molar CH3COOH (aqueous).

The pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration.

Solution

We are asked if the pH at the equivalence point in the HNO3 titration will be lower than the pH at the equivalence point in the CH3COOH titration where both were titrated with a 0.100 M solution of NaOH(aq).

1. Titration of 25.0 mL of 1.0 M HNO3 with 0.100 M NaOH solution

The reaction for this titration can be represented by:

HNO3 + NaOH → NaNO3 + H2O

In the reaction HNO3, a strong acid, will react with NaOH, a strong base to form a neutral solution.

At the equivalence point of the reaction, hydronium (H+) and hydroxide (OH-) ions will react to form water, leading to a pH of 7.

This is true for all strong acid and strong base reactions.



 2. Titration of 25 mL of 1.0 M CH3COOH with 0.100 M NaOH

This reaction is a Weak Acid – Strong Base titration.

The reaction between HCH3COO and NaOH will be a double displacement reaction where H+ reacts with OH and CH3COO reacts with Na+


 The overall reaction is:

  

 HCH3COO + NaOHH2O + NaCH3COO


 Recall that at the equivalence point of a titration:


moles acid = moles base


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