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Chapter 19: Q19.1P (page 872)

What is the purpose of an acid-base buffer?

Short Answer

Expert verified

Buffers can withstand a large pH change.

Step by step solution

01

Acidic buffer solution

An acidic buffer solution is formed by mixing a weak acid with the salt having its conjugate base.

02

Basic buffer solution

A basic buffer solution is the one which is formed by combining a weak base with a salt solution of its conjugate acid.

03

Step 3:Purpose of buffer solution

Buffer solutions can withstand pH changes because their weak acid or base and conjugate salt parings allow them to neutralise any changes within a specified range that differs between buffers. A buffer solution may begin to fail to stabilise the pH level if the pH is changed substantially.

Hence Buffers resist the dramatic change in pH.

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Most popular questions from this chapter

Find the solubility of $Cr {(OH)}_{3}$ in a buffer of pH 13.0 [ $K_{sp}$ of ${Cr(OH)}_{3} {=6.3×10}^{- 31}$ ; $K_{f}$ of $Cr(OH {)_{4}}^{-} {=8.0×10}^{29}$ ].

Ethylenediaminetetraacetic acid (abbreviated $H_{4} EDTA$ ) is a tetraprotic acid. Its salts are used to treat toxic metal poisoning by forming soluble complex ions that are then excreted. Because ${EDTA}^{4 -}$ also binds essential calcium ions, it is often administered as the calcium disodium salt. For example, when ${Na}_{2} Ca$ (EDTA) is given to a patient ${[Ca (EDTA)]}^{2 -}$ , the ions react with circulating ions and the metal ions are exchanged:

$\begin{array}{l} {[Ca (EDTA)]}^{2 -} (aq) + P b^{2 +} (aq) \\ {[Pb (EDTA)]}^{2 -} (aq) + C a^{2 +} (aq) K_{c} = 2.5 \times 10^{7} \end{array}$

A child has a dangerous blood lead level of $120 μg / 100 mL$ . If the child is administered $100 mL$ of $0.10 M {NaNa}_{2}$ (EDTA), assuming the exchange reaction and excretion process are $100 %$ efficient, what is the final concentration of ${Pb}^{2 +}$ in $μg / 100 mL$ blood? (Total blood volume is $1.5 L$ .)

A lake that has a surface area of $10 . 0 acres (1 acre = 4 . 840 \times 10^{3} {yd}^{2})$ receives $1.00 in .$ of rain of $pH 4.20$ . (Assume that the acidity of the rain is due to a strong, monoprotic acid.)

(a) How many moles of $H_{3} O^{+}$ are in the rain falling on the lake?

(b) If the lake is unbuffered $(pH = 7 . 00)$ and its average depth is $10.0 ft$ before the rain, find the $pH$ after the rain has been mixed with lake water. (Ignore runoff from the surrounding land.)

(c) If the lake contains hydrogen carbonate ions role="math" localid="1663280552167" ${(HCO}_{3}^{-})$ , what mass of ${(HCO}_{3}^{-})$ would neutralize the acid in the rain?

Choose specific acid-base conjugate pairs to make the following buffers: (a) $[O H^{-}] \approx 1 \times 10^{- 6} M$ ; (b) $[H_{3} O^{+}] \approx 4 \times 10^{- 4} M$ . (See Appendix C.)

An environmental technician collects a sample of rainwater. Back in the lab, hermeter isn't working, so she uses indicator solutions to estimate the. A piece of litmus paper turns red, indicating acidity, so she divides the sample into thirds and obtains the following results: thymol blue turns yellow; bromophenol blue turns green; and methyl red turns red. Estimate theof the rainwater.

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