RDGBufferstxt

RDGBufferstxt - brady_c16_642-691hr 2:32 PM Page 666 666...

This preview shows pages 1–2. Sign up to view the full content.

666 Chapter 16 Equilibria in Solutions of Weak Acids and Bases This is the identical value obtained using the quadratic equation. Notice also that the change in x between the two approximations grew smaller. The second approximation gave a smaller correction than the first. Each succeeding approximation differs from the preceding one by smaller and smaller amounts. We stop the calculation when the difference between two approximations is insignificant. Try this approach by reworking Practice Exercise 26 and solving for [OH 2 ] in the 0.0010 M CH 3 NH 2 solution using the method of successive approximations. 3 16.5 B UFFERS ENABLE THE CONTROL OF pH Many chemical and biological systems are quite sensitive to pH. For example, if the pH of your blood were to change from what it should be, within the range of 7.35 to 7.42, either to 7.00 or to 8.00, you would die. Thus, a change in pH can produce unwanted effects, and sys- tems that are sensitive to pH must be protected from the H 1 or OH 2 that might be formed or consumed by some reaction. Buffers are mixtures of solutes that accomplish this. The solu- tion containing this mix of solutes is said to be buffered or it is described as a buffer solution . Buffers contain a weak acid and a weak base A buffer contains solutes that enable it to resist large changes in pH when small amounts of either strong acid or strong base are added to it. Ordinarily, the buffer consists of two solutes, one providing a weak Brønsted acid and the other a weak Brønsted base. Usually, the acid and base represent a conjugate pair. If the acid is molecular, then the conjugate base is supplied by a soluble salt of the acid. For example, a common buffer system consists of acetic acid plus sodium acetate, with the salt’s acetate ion serving as the Brønsted base. In your blood, carbonic acid (H 2 CO 3 , a weak diprotic acid) and the bicarbonate ion (HCO 3 2 , its conjugate base) serve as one of the buffer systems used to maintain a remarkably constant pH in the face of the body’s production of organic acids by metabolism. Another common buffer consists of the weakly acidic cation, NH 4 1 , supplied by a salt like NH 4 Cl, and its conjugate base, NH 3 . One important point about buffers is the distinction between keeping a solution at a particular pH and keeping it neutral—at a pH of 7. Although it is certainly possible to prepare a buffer to work at pH 7, buffers can be made that will work around any pH value throughout the pH scale. A buffer works by neutralizing small additions of strong acid or base To work, a buffer must be able to neutralize either a strong acid or strong base that is added to it. This is precisely what the weak base and weak acid components of the buffer do. Consider, for example, a buffer composed of acetic acid, HC 2 H 3 O 2 , and acetate ion, C 2 H 3 O 2 2 , supplied by a salt such as NaC 2 H 3 O 2 . If we add extra H 1 to the buffer (from a strong acid) the acetate ion (the weak conjugate base) can react with it as follows.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

Page1 / 8

RDGBufferstxt - brady_c16_642-691hr 2:32 PM Page 666 666...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online