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Questions and Answers
What is transferred between a conjugate acid-base pair?
What is transferred between a conjugate acid-base pair?
a proton
Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base?
Which compound can act as both a Bronsted-Lowry acid and a Bronsted-Lowry base?
water
In the reaction CO3^2- + H2O HCO3^- + OH-, the carbonate ion is acting as a?
In the reaction CO3^2- + H2O HCO3^- + OH-, the carbonate ion is acting as a?
Bronsted-Lowry base
Which of the following represents a Bronsted-Lowry conjugate acid-base pair?
Which of the following represents a Bronsted-Lowry conjugate acid-base pair?
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Which of these solutions is the most basic?
Which of these solutions is the most basic?
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An indicator is what type of compound?
An indicator is what type of compound?
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What characterizes a strong acid or base?
What characterizes a strong acid or base?
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What is another name for the acid dissociation constant?
What is another name for the acid dissociation constant?
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How many ionization constants are associated with oxalic acid?
How many ionization constants are associated with oxalic acid?
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A 0.12 M solution of an acid that ionizes only slightly in solution would be termed?
A 0.12 M solution of an acid that ionizes only slightly in solution would be termed?
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Which of the following pairs consists of a weak acid and a strong base?
Which of the following pairs consists of a weak acid and a strong base?
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A substance with a Ka of 1 x 10^-5 would be classified as a?
A substance with a Ka of 1 x 10^-5 would be classified as a?
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The ionization constant (Ka) of HF is 6.7 x 10^-4. Which of the following is true in a 0.1 M solution of this acid?
The ionization constant (Ka) of HF is 6.7 x 10^-4. Which of the following is true in a 0.1 M solution of this acid?
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If an acid has a Ka = 1.6 x 10^-10, what is the acidity of the solution?
If an acid has a Ka = 1.6 x 10^-10, what is the acidity of the solution?
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The Ka of carbonic acid is 4.3 x 10^-7. What does this mean for H2CO3?
The Ka of carbonic acid is 4.3 x 10^-7. What does this mean for H2CO3?
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Which acid has the greatest acid dissociation constant?
Which acid has the greatest acid dissociation constant?
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Which base is strong, but never concentrated?
Which base is strong, but never concentrated?
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A base has a Kb of 2.5 x 10^-11. Which of the following statements is true?
A base has a Kb of 2.5 x 10^-11. Which of the following statements is true?
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Which base has the smallest base dissociation constant?
Which base has the smallest base dissociation constant?
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Study Notes
Conjugate Acid-Base Pairs
- A conjugate acid-base pair differs by a single proton.
- Conjugate pairs include NH4^+ and NH3, where the proton is transferred.
Bronsted-Lowry Acid and Base Concepts
- Water can function as both a Bronsted-Lowry acid and base.
- In the reaction CO3^2- + H2O ⇌ HCO3^- + OH-, carbonate ion acts as a Bronsted-Lowry base.
Acid-Base Properties
- A solution with [H+] = 1 x 10^-11 M is considered the most basic.
- Strong acids and bases exhibit complete ionization in water.
- Weak acids and bases, like acetic acid or ammonia, exhibit partial ionization.
Ionization Constants
- The acid dissociation constant is also known as the ionization constant.
- Oxalic acid has two ionization constants, reflecting its ability to donate two protons.
- A weak acid is classified with a Ka value of 1 x 10^-5 or lower.
- Carbonic acid (H2CO3) has a Ka of 4.3 x 10^-7, indicating it is a poor hydrogen-ion donor.
Solutions and Concentrations
- A 0.12 M acid solution that ionizes slightly is termed dilute and weak.
- Nitric acid has the greatest acid dissociation constant, suggesting it is a strong acid.
- Magnesium hydroxide is a strong base that is not usually found in concentrated forms.
Fundamental Relationships in Solutions
- In a 0.1 M solution of HF (with Ka = 6.7 x 10^-4), [HF] is greater than [H+][F-], indicating an equilibrium favoring the non-dissociated form.
- The acidity of a solution with a Ka of 1.6 x 10^-10 cannot be defined without additional information.
- A base with Kb of 2.5 x 10^-11 ionizes slightly in aqueous solution, indicative of weak base behavior.
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Description
Test your understanding of conjugate acid-base pairs and the Bronsted-Lowry acid-base theory. This quiz will cover properties of acids and bases, their ionization constants, and basicity of solutions. Perfect for chemistry students exploring these fundamental concepts.
