Buffer Theory
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Buffer TheoryQuestions
- What are the applications of a buffer?
- How do you calculate buffer pH for polyprotic acids?
- How do you calculate buffer pH for monoprotic acids?
- What is the buffer capacity of a buffer solution?
- How many Good's buffer agents exist?
- Question #ea6ed
- Question #0d9d2
- Question #26e0c
- Question #c5de8
- What do you mean by physiological buffers? What are the different types of buffers found in the blood? If possible, please state examples.
- What is the "Carbonic acid-bicarbonate" buffer system?
- What buffers are in our body?
- Question #fcc4b
- When acid or base is added to water, the #pH# changes dramatically. Why, when acid or base is added to a buffer solution, does the #pH# change only marginally?
- Why does pH = pK when pH = 7, according to the Henderson-Hasselbalch equation?
- Question #431bf
- What are the factors that affect buffer capacity?
- At what pH does a buffer solution exhibit maximum buffer capacity?
- Using Henderson-Hasselbalch equation, calculate the volume of 0.20 M Acetic Acid and 0.2 M Sodium Acetate needed to prepare 50 mL of 0.1 M Acetate Buffer solution (pH = 4.5). pKa of Acetic Acid is 4.74?
- Normally, the pH of the human body is fixed in a very narrow range between 7.35 and 7.45. A patient with an acidotic blood pH of 7.3 may be treated with an alkali such as sodium bicarbonate. Why would this treatment raise the pH of the blood?
- Is a buffer supposed to keep the pH of a solution at 7?
- How do buffers regulate the pH of a fluid?
- Question #34d98
- How does a buffer work in chemistry?
- What is a buffer solution?
- If a buffer made by dissolving 20.0 g of sodium benzoate (144g/mol) and 10 grams of benzoic acid (122g/mol) in water to a final volume of 500.0 ml, what is the pH of the buffer?
- What are five examples of buffer solutions?
- Is it possible to prepare a buffer solution using nitric acid (#HNO_3#) and sodium hydroxide (#NaOH#)?
- How do you find the pH of a buffer solution?
- When #HCl# and #NH_3# are mixed why is the buffer #NH_3-NH_4Cl#?
- When #NH_4Cl# mixed with #NH_3# what happens?
- A 250.0 mL buffer solution is 0.250 M in acetic acid and 0.250 M in sodium acetate. What is the initial pH of this solution? What is the pH after addition of 0.0050 mol of HCl? What is the pH after addition of 0.0050 mol of NaOH?
- A buffer solution of a weak acid and its salt had a pH of 7.85 when the acid was 0.251 M and the anion was 1.10 M. How do you calculate the equilibrium dissociation constant (Ka)?
- How do you calculate the molarities of #CH_3COOH# and #CH_3COO^-# in buffer solution?
- #"A buffer equation contains appreciable quantities of a (i)................"# #"and its (ii) ..................?"#
- What is the difference between carbonate and bicarbonate?
- Henderson Hasselbalch help? Phosphoric acid is a triprotic acid. To find the pH of a buffer composed of #"H"_2"PO"_(4(aq))^(-)# and #"HPO"_(4(aq))^(2-)#, which #pK_a# value would you use in the Henderson-Hasselbalch equation?
- What is a volatile buffer?
- How does a buffer work?
- Why are buffers important to living things?
- What do buffers do and why are they important in biological systems?
- What is a buffer? How do they work? How can they maintain pH?
- What is the function of a buffer?
- What are the uses of buffer solutions?
- How would you use #NaHCO_3# and #H_2CO_3# (a buffer sometimes added to swimming pools) to explain how buffers work?
- What is the effect of buffer concentration on pH?
- How do buffers resist pH change?
- Is the purpose of a buffer system to keep a solution neutral? If not, what is the purpose?
- Why would a buffer be important to homeostasis?
- How do buffers work to maintain pH?
- How do buffers maintain pH?
- How are buffers prepared?
- How are buffers made?
- Why do buffers resist pH change?
- How does a buffer affect pH?
- How do buffers effect pH?
- How do buffers change pH?
- Why is a buffer solution used?
- Why is the #pH# of a buffer close to the #pK_a# of the acid used to make the buffer...?
- Question #c644d
- What is buffering capacity? How is buffering capacity measured?
- If a buffer solution is prepared from 5.15g #NH_4NO_3# and 0.10L of 0.15M #NH_3#, what is the pH of the solution?
- When an acid is added to a buffer, does the acid in the buffer turn into base to neutralize the acid? Or is there some other that the buffers maintains constant pH?
- A buffer solution contains 0.20 M #CH_3COOH# and 0.30 M #CH_3COONa# at #25^oC#? (#Ka=1.8 x10^-5#). What is the pH after the addition of (a) 20.0 mL of 0.050 M #NaOH# or (b) 20.0 mL of 0.050 M #HCl# to 80.0 mL of this buffer solution?
- What is an example of buffering capacity?
- What is a buffer in chemistry?
- How do you write the chemical equation for the acetate buffer equilibrium [same for both buffers]?
- How would you write the chemical equation for how the acetate buffer neutralizes excess acid, #H_3O^+#? How do you write the chemical equation for how the acetate buffer neutralizes excess base, #OH^-#?
- How do buffer systems affect pH?
- How do pH buffer systems work?
- How do you make a buffer in chemistry?
- Why should you use a buffer in chemistry?
- Do buffers resist pH change? If so, why?
- How can you identify a buffer in chemistry?
- Why is a buffer important in chemistry?
- We prepare a buffer by adding 0.5289 mol #HNO_3# to 0.5291 L of a solution containing 1.924 M trimethylamine [#(CH_3)_3N#, #Kb = 6.500x10^-5#]. What is the pH of this buffer? How do you solve this? Please help!?
- A buffer solution of pH = 5.15 is to be prepared from acetic acid (Ka = #1.80 x 10^-5#), sodium acetate and water. What must be the molar ratio of acetate ion to acetic acid in this solution to obtain this pH?
- Which of the following couples are buffer systems? How do you determine this?
- Why do solutions that contain buffers tend to resist pH changes?
- What happens in a buffer when the level of H+ ions in solution increases?
- Determine the final pH of a 0.200M triprotic phosphoric acid solution?
- What is a #"buffer"#, and how is it used to maintain #pH#?
- Question #560cd
- Question #e9b66
- When weak acid #"HAsp"# is titrated with a strong base and #pH# is plotted against volume of titrant, at what point in the titration will #pH=pK_a#?
- Could it be possible to make a buffer of pH 12.3 from solutions of disodium hydrogen phosphate and trisodium phosphate?
- Could a buffered solution be made by mixing aqueous solutions of HCl and NaOH? Explain. Why isn't a mixture of a strong acid and its conjugate base considered a buffered solution?
- Question #bb8ec
- Question #d8740
- Question #ce2a2
- Why does the conjugate base of a strong acid have no effect on solution #pH#?
- Addition of #"sodium hydroxide"# to an #"acetic acid/sodium acetate buffer"# only marginally increases the #pH# of the solution. Why so?
- Question #694c2