CH 104 - Acid Base Equilibrium Reactions - Division of Chemistry and Chemical Engineering Assignment Help

Assignment Task :

1. In the following reactions, indicate the acid, base, conjugate acid, and conjugate base.
(a) HF + NH3 → NH4 + + F –

(b) NaHSO4 + HClO3 ? H2SO4 + NaClO3

2. Write the formula for the following.

(a) Conjugate base of H2O

(b) Conjugate base of H2PO4 –

(c) Conjugate acid of HS –

(d) Conjugate acid of CH3NH2

3. Answer the following questions about acid-base equilibrium reactions.

(a) Which is a stronger acid HX or HY in the reaction below?

(b) What is the difference between a strong acid and a weak acid in terms of equilibrium position?

(c) If the Ka of H2CO3 is 4.3 x 10 –7 and the Ka of HF is 6.8 x 10 –4, then is the reaction below reactant favored or product favored?

(d) Based on the following Ka values, which is the strongest acid and which is the weakest acid?

4. Indicate whether the following solutions are acidic (A), basic (B), or neutral (N).

5. Assuming complete dissociation, what is the pOH of a 0.00247 M H2SO4 solution? Is this solution acidic or basic?
 

6. Complete the table below:

7. Answer the following questions about buffers.
(a) Circle the set of compounds that could act as a buffer.

• HNO2 and NaNO2
• KCl and KCN
• HF and NaF
• H2CO3 and NaHCO3

(b) How does a buffer solution prevent a larger change in pH? What does it mean when a solution has exceeded the buffer capacity?

(c) Write an equation for the following buffering action.

8. Assign oxidation number to the following elements.
(a) Mg in MgCO3

(b) Ti in Ti3P2

(c) N in N2O

(d) I in IBr3

9. Indicate whether the following change in oxidation number is an oxidation or a reduction.
(a) +3 → +1
(b) -2 → -3
(c) -1 → +1
(d) 0 → -1

10. In each reaction below, indicate which element is being oxidized, which element is being reduced, which element is the oxidizing agent, and which element is the reducing agent.
(a) 2 Na + CaO → Na2O + 2 Ca

(b) Zn + Cl2→ ZnCl2

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