6. In part C you prepared two buffer solutions using acetic acid and sodium acet

Question

6. In part C you prepared two buffer solutions using acetic acid and sodium acetate. Why are two solutions required, and what is common to both these solutions? 7. Identify whic h of the following solutions may act as buffers by placing a check in the box next to the mixture. A. HNO2, KNO2 B. HNOs, NaNO3 O D. NHOH, NHAC2Hs02 E. H2S04, NaHS04 8. What is meant by the term buffer capacity? Which buffer solution (A or B) has the higher buffer capacity? Buffer 'B" is approximately 2.0 imes stronger than buffer A, using your volume data, show that the relationship between the strength of the buffer solution is directly related to its buffer capacity

Explanation / Answer

6) part C is not given. To solve this question, part C is required.

Buffer = weak acid + salt formed from strong base (or) weak base + salt formed from strong acid

Acidic buffer = weak acid and salt formed from strong base

Basic buffer = weak base and salt formed from strong acid

7)  

Buffer = weak acid + salt formed from strong base (or) weak base + salt formed from strong acid

Acidic buffer = weak acid and salt formed from strong base

Basic buffer = weak base and salt formed from strong acid

Since HNO3, H2SO4 are strong acids, the solutions containing these two are not act as buffer solutions.

Therefore,

HNO2, KNO2 = buffer

HNO3, NaNO3 = Not a buffer

H2CO3, NaHCO3 = buffer

NH4OH , NH4C2H3O2 = Not a buffer    [ NH4C2H3O2 = CH3COOH + NH3. Here, CH3COOH is a weak acid]

H2SO4, NaHSO4 = Not a buffer

HCHO2, NaCHO2 = buffer

[HNO2, H2CO3 , HCHO2 are weak acids.]

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