Question

question 3 (2 points)
answer each of the following for the following reaction
h₂so₃ + h₂o ↔ hso₃⁻¹ + h₃o⁺¹
for polyprotic acids only one acidic hydrogen is removed by a very weak base such
as water
1 is the acid
2 is the base
3 is the conjugate acid
4 is the conjugate base
h₂so₃ is not on the list of seven strong acid so is treated like a 5 acid and we
use a double - sided arrow
a. h₂so₃ b. h⁺ c. h₃o⁺¹ d. hso₃⁻¹ e. so₃⁻²
f. h₂o g. strong h. weak

Explanation:

Step1: Identify the acid (1)

An acid donates a proton ($H^+$). In the reaction $\ce{H2SO3 + H2O <=> HSO3^{-1} + H3O^{+1}}$, $\ce{H2SO3}$ donates a proton to $\ce{H2O}$. So the acid is A. $\ce{H2SO3}$.

Step2: Identify the base (2)

A base accepts a proton. $\ce{H2O}$ accepts a proton from $\ce{H2SO3}$ to form $\ce{H3O^{+1}}$. So the base is F. $\ce{H2O}$.

Step3: Identify the conjugate acid (3)

The conjugate acid is formed when a base accepts a proton. $\ce{H2O}$ (base) accepts a proton to become $\ce{H3O^{+1}}$, so the conjugate acid is C. $\ce{H3O^{+1}}$.

Step4: Identify the conjugate base (4)

The conjugate base is formed when an acid donates a proton. $\ce{H2SO3}$ (acid) donates a proton to become $\ce{HSO3^{-1}}$, so the conjugate base is D. $\ce{HSO3^{-1}}$.

Step5: Identify the type of acid (5)

$\ce{H2SO3}$ is not a strong acid (not in the list of seven strong acids), so it is a weak acid. So the answer is H. weak.

Answer:

1. A. $\ce{H2SO3}$
2. F. $\ce{H2O}$
3. C. $\ce{H3O^{+1}}$
4. D. $\ce{HSO3^{-1}}$
5. H. weak