Consider the following equilibrium:

Chemistry

2 answers:

balu736 [363]3 years ago

8 0

Answer:

see explanataion

Explanation:

Buffer solutions are defined as solutions containing a weak electrolyte (wk acid or wk base) and the salt of the weak electrolyte.

Given HF(aq) + H₂O(l) ⇄ H₃O(l) + F⁻, a buffer solution would result from a solution composition when [F -] is equal to [HF]. Such is commonly referred to as a 50/50 buffer as the acid and salt are in equal concentrations. However, a buffer solution still will exist even if the concentrations of acid and salt are not equal. The presence of the weak acid or weak base and the salt of the electrolytes is the only requirement.

Veseljchak [2.6K]3 years ago

3 0

Answer:

Explanation:

Buffer has equal concentrations of A- and HA.

B. when [F -] is equal to [HF]

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A multistep reaction can only occur as fast as its slowest step. Therefore, it is the rate law of the slow step that determines

kodGreya [7K]

Answer : The rate law for the overall reaction is, $Rate=k[A][B]$

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

As we are given the mechanism for the reaction :

Step 1 : $A+B\rightarrow AB$ (slow)