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The pH of a sodium acetate-acetic acid buffer is 4.50. Calculate the ratio $\left[\mathrm{CH}_{3} \mathrm{COO}^{-}\right] /\left[\mathrm{CH}_{3} \mathrm{COOH}\right]$

$$=.58$$

Chemistry 102

Chapter 16

Acid-Base Equilibria and Solubility Equilibria

Acid-Base Equilibria

Aqueous Equilibria

Rice University

University of Maryland - University College

Brown University

Lectures

00:41

In chemistry, an ion is an atom or molecule that has a non-zero net electric charge. The name was coined by John Dalton for ions in 1808, and later expanded to include molecules in 1834.

24:14

In chemistry, a buffer is a solution that resists changes in pH. Buffers are used to maintain a stable pH in a solution. Buffers are solutions of a weak acid and its conjugate base or a weak base and its conjugate acid, usually in the form of a salt of the conjugate base or acid. Buffers have the property that a small change in the amount of strong acid or strong base added to them results in a much larger change in pH. The resistance of a buffer solution to pH change is due to the fact that the process of adding acid or base to the solution is slow compared to the rate at which the pH changes. In addition to this buffering action, the inclusion of the conjugate base or acid also slows the process of pH change by the mechanism of the Henderson–Hasselbalch equation. Buffers are most commonly found in aqueous solutions.

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this question is asking us for the ratio of our continent base over our starting acid mark. A value is he will do 1.8 times 10 to the negative. And we console for this question by using our Henderson Hasselbach equation. Which is Ph is PK A plus the log of our contact base over the concentration of her weak acid. So we can rearrange this question. Two pH minus. P K. Is equal to the log of our ratio. And then to cancel the log, we will take 10 to the ph minus PK to get our final answer. Now, if it's easier we can solve for the Ph. Mayes PK and then take 10 to the value that we receive. Um, for the sake of cleaning up, I'm just going to plug all of our values into this equation right here. So we get 10 to the given pH, which is 4.5. Subtract that from the negative log of R K. A value because P K is equal to the negative log of a K A value which in this case is 1.8 times 10 to the negative, and that will get us. Our answer, which is 0.58 were 0.57 depending on where you decided to use scientific notation and where you, um, decided to use true values, so you should get something around 0.58 as your ratio.

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