Medium pKa and pKb Practice Questions

Concept Explanation

The pKa and pKb values are the negative base-10 logarithms of the acid dissociation constant (Ka) and base dissociation constant (Kb), respectively, serving as quantitative measures of the strength of acids and bases in solution. Mastering pKa and pKb practice questions is essential for understanding how molecules behave in biological systems and chemical reactions. A lower pKa indicates a stronger acid, meaning the substance more readily donates a proton, while a lower pKb indicates a stronger base. These values are intrinsically linked through the self-ionization constant of water ($K_w$). At standard temperature (25°C), the relationship is defined by the equation $pK_a + pK_b = 14$. This relationship allows chemists to calculate the strength of a conjugate base if the strength of the parent acid is known, and vice versa. Understanding these logarithmic scales is vital for predicting the direction of equilibrium in strong acid vs weak acid comparisons and for performing complex pH calculation practice questions.

Solved Examples

Below are worked examples to demonstrate how to convert between $K_a/K_b$ and $pK_a/pK_b$, and how to use the relationship between conjugate pairs.

1. Example 1: Converting Ka to pKa
   An unknown weak acid has an acid dissociation constant ($K_a$) of $1.8 \times 10^{-5}$. Calculate its $pK_a$.

   1. Identify the formula: $pK_a = -\log(K_a)$.

   2. Substitute the value: $pK_a = -\log(1.8 \times 10^{-5})$.

   3. Calculate: $pK_a \approx 4.74$.

2. Example 2: Finding pKb from pKa
   The $pK_a$ of hydrocyanic acid (HCN) is 9.21. Determine the $pK_b$ of its conjugate base, the cyanide ion ($CN^-$).

   1. Identify the relationship: $pK_a + pK_b = 14.00$ (at 25°C).

   2. Rearrange for $pK_b$: $pK_b = 14.00 - pK_a$.

   3. Calculate: $pK_b = 14.00 - 9.21 = 4.79$.

3. Example 3: Calculating Kb from pKb
   A base has a $pK_b$ of 3.30. What is the value of its base dissociation constant ($K_b$)?

   1. Identify the formula: $K_b = 10^{-pKb}$.

   2. Substitute the value: $K_b = 10^{-3.30}$.

   3. Calculate: $K_b \approx 5.01 \times 10^{-4}$.

Practice Questions

Test your knowledge with these medium pKa and pKb practice questions. Ensure you have a scientific calculator ready for the logarithmic conversions.

1. A specific organic acid has a $K_a$ of $4.5 \times 10^{-4}$. Determine its $pK_a$.

2. If the $pK_b$ of ammonia ($NH_3$) is 4.75, what is the $pK_a$ of its conjugate acid, the ammonium ion ($NH_4^+$)?

3. Calculate the $K_b$ for a base that has a $pK_b$ of 8.90.

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4. Formic acid has a $pK_a$ of 3.75. Calculate the $K_a$ value and determine the $pK_b$ of the formate ion.

5. Arrange the following acids in order of increasing strength based on their $pK_a$ values: Acid A ($pK_a = 2.1$), Acid B ($pK_a = 4.8$), Acid C ($pK_a = 1.2$).

6. A solution of methylamine has a $K_b$ of $4.4 \times 10^{-4}$. Calculate both the $pK_b$ and the $pK_a$ of its conjugate acid.

7. Given that $K_a$ for nitrous acid ($HNO_2$) is $4.0 \times 10^{-4}$, find the $K_b$ for the nitrite ion ($NO_2^-$).

8. Which is a stronger base: Base X with $pK_b = 3.5$ or Base Y with $K_b = 1.0 \times 10^{-5}$?

9. A hypothetical acid has a $pK_a$ of -2.0. Is this a strong or weak acid, and what does this imply about its $K_a$?

10. If the $pK_a$ of a conjugate acid increases, what happens to the strength of the conjugate base?

Answers & Explanations

1. Answer: 3.35.
   Explanation: Use the formula $pK_a = -\log(K_a)$. Thus, $-\log(4.5 \times 10^{-4}) = 3.346$, rounded to 3.35.

2. Answer: 9.25.
   Explanation: Using $pK_a + pK_b = 14$, we get $14 - 4.75 = 9.25$. This is a common calculation when working with buffer solution practice questions.

3. Answer: $1.26 \times 10^{-9}$.
   Explanation: $K_b = 10^{-pKb} = 10^{-8.90} \approx 1.26 \times 10^{-9}$.

4. Answer: $K_a = 1.78 \times 10^{-4}$; $pK_b = 10.25$.
   Explanation: $K_a = 10^{-3.75} = 1.78 \times 10^{-4}$. For the conjugate base, $pK_b = 14 - 3.75 = 10.25$.

5. Answer: Acid B < Acid A < Acid C.
   Explanation: Strength increases as $pK_a$ decreases. Acid C (1.2) is the strongest, and Acid B (4.8) is the weakest.

6. Answer: $pK_b = 3.36$; $pK_a = 10.64$.
   Explanation: $pK_b = -\log(4.4 \times 10^{-4}) = 3.356$. $pK_a = 14 - 3.356 = 10.644$.

7. Answer: $2.5 \times 10^{-11}$.
   Explanation: $K_a \times K_b = 10^{-14}$. So, $K_b = 10^{-14} / (4.0 \times 10^{-4}) = 2.5 \times 10^{-11}$.

8. Answer: Base X.
   Explanation: Convert Base Y's $K_b$ to $pK_b$: $-\log(1.0 \times 10^{-5}) = 5.0$. Since Base X has a lower $pK_b$ (3.5), it is the stronger base.

9. Answer: Strong acid; $K_a = 100$.
   Explanation: A negative $pK_a$ indicates a very strong acid that dissociates completely or nearly completely in water. $K_a = 10^{-(-2)} = 10^2 = 100$.

10. Answer: The conjugate base becomes stronger.
    Explanation: As $pK_a$ increases, the acid becomes weaker. Because $pK_a + pK_b = 14$, a higher $pK_a$ means a lower $pK_b$, which signifies a stronger conjugate base.

1. Which of the following pKa values represents the strongest acid?

• A10.5
• B4.2
• C1.5
• D7.0

Frequently Asked Questions

What is the difference between Ka and pKa?

Ka is the acid dissociation constant that measures the equilibrium concentration of ions, while pKa is the negative logarithm of that constant. The pKa scale is more convenient for comparing acid strengths because it uses smaller, more manageable numbers rather than scientific notation.

Can a pKa value be negative?

Yes, extremely strong acids like hydrochloric acid or sulfuric acid have negative pKa values. A negative pKa indicates that the acid dissociation constant (Ka) is greater than 1, meaning the acid dissociates almost completely in aqueous solution.

How does temperature affect pKa and pKb?

Since pKa and pKb are derived from equilibrium constants, they are temperature-dependent. As temperature increases, the self-ionization of water ($K_w$) typically increases, which shifts the $pK_a + pK_b = 14$ relationship to a lower sum.

Why is the sum of pKa and pKb always 14?

This relationship is derived from the water auto-ionization constant, $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. Taking the negative log of both sides of the equation $K_a \times K_b = K_w$ results in $pK_a + pK_b = 14$.

How do pKa values help in predicting reaction direction?

Acid-base reactions favor the side with the weaker acid and weaker base. By comparing the pKa values of the acids on both sides of the equation, you can predict that the equilibrium will shift toward the species with the higher pKa value.