A) Why does a buffer solution require a weak acid/base conjugate pair, as opposed to a...

A) Why does a buffer solution require a weak acid/base conjugate pair, as opposed to a strong acid, and its conjugate?

		A strong acid will completely dissociate, suggesting that the conjugate base is really weak and will not neutralize any additional H⁺ ions.
		A strong acid will completely dissociate, suggesting that the conjugate base is really strong and will not neutralize any additional H⁺ ions.
		A strong acid will only partially dissociate, suggesting that the conjugate base is really weak and will not neutralize any additional H⁺ ions.
		A strong acid will only partially dissociate, suggesting that the conjugate base is really strong and will not neutralize any additional H⁺ ions.

B) Write out reactions that show how a buffer of HCN/NaCN is able to control pH after the addition of HCl.

		NaCN_(aq) + HCN_(aq)↔ HCl_(aq) + NaCl_(aq)
		HCN_(aq)+ HCl₍_aq)↔ NaCN_(aq) + H₂O_(l)
		NaCN_(aq) + HCl₍_aq)↔ HCN_(aq) + NaOH_(aq)
		NaCN_(aq) + HCl_(aq) ↔ HCN_(aq) + NaCl_(aq)

Expert Solution

queen_honey_blossom answered 3 years ago

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