Two different questions, any help is appreciated. About buffers
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It is made up of a weak acid and its conjugate base or a weak base and its conjugate acid. Buffers are important in many biological and chemical processes because they help maintain a stable pH environment. Show more…
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Give two examples of the practical uses of buffers.
Acids and Bases
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What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? $0.01 M$ acetic acid/0.01 $M$ sodium acetate $0.1 \mathrm{M}$ acetic acid/0.1 $\mathrm{M}$ sodium acetate $1.0 \mathrm{M}$ acetic acid/ $1.0 \mathrm{M}$ sodium acetate Which of the following can be classified as buffer solutions? a. $0.25 M \mathrm{HBr}+0.25 \mathrm{M} \mathrm{HOBr}$ b. $0.15 M \mathrm{HClO}_{4}+0.20 \mathrm{M} \mathrm{RbOH}$ c. $0.50 M \mathrm{HOCl}+0.35 \mathrm{M} \mathrm{KOCl}$ d. $0.70 M \mathrm{KOH}+0.70 \mathrm{M} \mathrm{HONH}_{2}$ e. $0.85 M \mathrm{H}_{2} \mathrm{NNH}_{2}+0.60 \mathrm{M} \mathrm{H}_{2} \mathrm{NNH}_{3} \mathrm{NO}_{3}$
What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? $0.01 M$ acetic acid/0.01 $M$ sodium acetate $0.1 \mathrm{M}$ acetic acid/0.1 $\mathrm{M}$ sodium acetate $1.0 \mathrm{M}$ acetic acid/ $1.0 \mathrm{M}$ sodium acetate How many of the following are buffered solutions? Explain your answer. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity.
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