Question 37 of 69beginner🔧 ApplyShort Answer1 mark

What will be the conjugate bases for the Brönsted acids: HF, H2SO4H_2SO_4 and HCO3−HCO_3^-?

Correct Answer

The conjugate bases for the given Brönsted acids are F−F^-, HSO4−HSO_4^-, and CO32−CO_3^{2-} respectively.

Exercise: EXERCISES | Q: 6.37 | (Page 45)
For More Understanding

Explanation

According to the Brönsted-Lowry theory, a conjugate base is formed when a Brönsted acid donates a proton (H+H^+). Therefore, the conjugate base will have one proton less than its corresponding acid. For HF, the conjugate base is F−F^-. For H2SO4H_2SO_4, the conjugate base is HSO4−HSO_4^-. For HCO3−HCO_3^-, the conjugate base is CO32−CO_3^{2-}.

Solution Steps

  1. Step 1: Identify that a conjugate base is formed by the loss of one proton (H+H^+) from a Brönsted acid.

  2. Step 2: Remove one H+H^+ from HF to get its conjugate base F−F^-.

  3. Step 3: Remove one H+H^+ from H2SO4H_2SO_4 to get its conjugate base HSO4−HSO_4^-.

  4. Step 4: Remove one H+H^+ from HCO3−HCO_3^- to get its conjugate base CO32−CO_3^{2-}.

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