State if each system would be useful as a buffer or not. Then explain the reason

Question

State if each system would be useful as a buffer or not. Then explain the reason(s) for your choice. a. A solution containing 0.08 M NaCN and 0.10 M HCN b. A solution containing 0.05 M NaOH in H_2 O c. A solution containing 0.25 M HC1 and 0.20 M NaCl d. A solution containing 0.05 M NH_4 Cl and 0.10 M NH_3 e. A solution containing 0.20 M KF and 0.15 M HF Considering the solution in Exercise 1b. a. Write the three chemical species that would be present in significant amounts. b. Is there any species present that can neutralize added hydroxide? Explain. Read the assigned pages in your textbook, and work the assigned problems.

Explanation / Answer

Buffer should be either a mixture of weak acid and it's salt or a weak base and it's salt.

A) HCN is a weak acid so this is a buffer

B) No eventhough it will neutralise acid, addition of any base will increase the pH

C)Not a buffer. Since HCl is strong it cannot neutralise any added acid

D) Ammonia is weak base and the mixture is a buffer

E) HF is a weak acid and hence this mixture is also a buffer

3

A) Na+, OH-, H2O

B) No there is no species which can neutralize the added hydroxide. Na+ will react to form again sodium hydroxide and water being a weak acid cannot neutralize hydroxide.

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