What is the common ion in a solution prepared by mixing 0.01 M NaCH_3CO_2 with 0

Question

What is the common ion in a solution prepared by mixing 0.01 M NaCH_3CO_2 with 0.01 M CH_3CO_2H? CH_3CO_2^- OH^- H_3O^+ Na^+ Which statement about buffers is true? Buffers resist change in pH upon addition of small amounts of strong acid or strong base. A buffer does not change pH on addition of a strong acid or strong base. Buffers consist of a strong acid and its conjugate base. Buffers have a pH - 7. What is the Henderson-Hasselbalch equation for the acidic buffer HA/A^-? pH - pK_a + log{[A^-]/[HA]} pH - pK_a - log{[A^-]/[HA]} pH - -log[H_3O^+] pH - 14 - pOH A 50.0 mL solution of 0.01 M HF has a pH of 2.1. When 50 mL. Of 0.01 M NaF is added to the HF solution the pH of the resulting solution will HF is a weak acid NaF is a strong electrolyte F(aq) + HOH(liq) rightarrow(aq) + OH. (aq) increase. decrease NaF - (aq) + HOH(liq) rightarrow HF(aq) + OH - (aq) remain the same. become 7.

Explanation / Answer

10) Answer : A CH3COO-

11) Answer : A Buffer resists changes in pH upon addition of small amount of strong acid or strong base

12) Answer : A pH= pKa + log([A-]/[HA])

13) Answer : A increases

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