Question

question 4 (2 points)
answer each of the following for the following reaction
nh₃ + h₂o ↔ nh₄⁺¹ + oh⁻¹
1 is the acid
2 is the base
3 is the conjugate acid
4 is the conjugate base
nh₃ does not have oh⁻¹ in the formula so is treated like a 5 base and we use a double - sided arrow
a. nh₃ b. h⁺ c. h₃o⁺¹ d. nh₄⁺¹ e. oh⁻¹
f. h₂o g. nh₂⁻¹ h. strong i. weak

Explanation:

Step1: Identify the acid

In the reaction $\ce{NH3 + H2O <=> NH4+ + OH-}$, an acid donates a proton ($\ce{H+}$). $\ce{H2O}$ donates a proton to become $\ce{OH-}$, so the acid is $\ce{H2O}$ (option F).

Step2: Identify the base

A base accepts a proton. $\ce{NH3}$ accepts a proton from $\ce{H2O}$ to become $\ce{NH4+}$, so the base is $\ce{NH3}$ (option A).

Step3: Identify the conjugate acid

A conjugate acid is formed when a base accepts a proton. $\ce{NH3}$ accepts a proton to form $\ce{NH4+}$, so the conjugate acid is $\ce{NH4+}$ (option D).

Step4: Identify the conjugate base

A conjugate base is formed when an acid donates a proton. $\ce{H2O}$ donates a proton to form $\ce{OH-}$, so the conjugate base is $\ce{OH-}$ (option E).

Step5: Identify the type of base for $\ce{NH3}$

$\ce{NH3}$ is a weak base because it does not dissociate completely in water, and the reaction is reversible (double - sided arrow), so it is a weak base (option I).

Answer:

1. F. $\ce{H2O}$
2. A. $\ce{NH3}$
3. D. $\ce{NH4+1}$
4. E. $\ce{OH-1}$
5. I. weak