Chemistry, 25.07.2019 16:30 katerin4738

The ph of a sodium acetate-acetic acid buffer is 4.70. calculate the ratio [ch3coo−] / [ch3cooh]

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According to Henderson–Hasselbalch Equation,

pH = pKa + log [Acetate] / [Acetic Acid]

As, pKa of Acetic Acid = 1.76

So, pH = 1.76 + log [Acetate] / [Acetic Acid]

4.70 = 1.76 + log [Acetate] / [Acetic Acid]

4.70 - 1.76 = log [Acetate] / [Acetic Acid]

-0.04 = log [Acetate] / [Acetic Acid]

Taking Antilog on both sides,

[Acetate] / [Acetic Acid] = 0.912

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C) the increase in atmospheric pressure pushes the walls of the balloon outward thus making it is the answer.hope i you.

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Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbf₂(s) ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is $k_{sp} = [\text{pb}^{2+}][\text{f}^- ]^2 = 4 \times 10^{-8}$ (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as $q = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}}$ then, we can interpret q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product: $\begin{aligned} q & = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}} \\ & = (1.9 \times 10^{-3} ) (3.8\times 10^{3})^2 \\ & = 2.7 \times 10^{-8} \end{aligned}$ since q = 2.7 × 10⁻⁸ < ksp = 4 × 10⁻⁸, a precipitate will not form.

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The ph of a sodium acetate-acetic acid buffer is 4.70. calculate the ratio [ch3coo−] / [ch3cooh]...

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