23)
Blood buffer system is bicarbonate buffer system
The components are
1. Bicorbonate : HCO3-
2. Carbonate : CO32-
24)
An buffer is a combination of weak acid and its conjucate basr or weak base and its conjucate acid
examples
weak acid /conjucate base
acetic acid(CH3COOH) / acetate ( CH3COO-)
Formic acid(HCOOH) / Formate (HCOO-)
weak base / conjucate acid
ammonia(NH3)/ammonium ion (NH4+)
pyridine( C5H5N) / pyridonium(C5H5NH+)
HI is strong acid , as an acid it react with weak base or conjucate base
For example consider CH3COOH/CH3COO- buffer system
HI reacts with conjucate base CH3COO-
CH3COO-(aq) + H+ (aq) -------> CH3COOH
so, the added H+ ions are consumed
Henderson- Hasselbalch equation gives pH of an buffer solution
pH = pKa + log([A-]/[HA])
where ,
A- : coniucate base or base
HA : acid or conjucate acid
pKa : pKa of acid or conjucate acid
25)
An buffer system is combination of weak acid and its salt with strong base or weak base and its salt with strong acid
HCl is a strong acid and NaCl is salt of HCl with strong base
So, it is not possible to use HCl and NaCl as components of a buffer system.
23. What are the names and formulas of the components of the principle buffer system of...
What is the main property of a buffer solution? A buffer does not allow any change in pH. A buffer resists drastic changes in pH upon addition of acid or base. Buffer solutions have an unlimited capacity to resist pH change. Upon adding a small amount of a strong acid or strong base, a buffer increases the change in pH to a very large amount
Please explain Buffers: Solutions That Resist pH Change. Below you will find questions. 1. Define buffer and know that a buffer typically consists of a weak acid and its conjugate base. 2. Know that the common ion effect is an example of Le Châtelier’s principle. 3. Calculate the pH of a buffer solution starting with initial concentrations of weak acid and its conjugate base. 4. Use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution from the pKa...
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
19. What chemical conversions take place among the general components of a buffer system when small amounts of a strong acid are added to the buffer? 20. HNO2 is a weak acid. What is the formula for the conjugate base of HNO,?
2. What is the pH of a buffer containing 0.050 M NH3 and 0.050 M NHACI? 3. What is meant by buffer capacity? 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NH3 solution and indicate the "buffer zone". 4. Sketch a pH titration curve for the addition of 0.10 M HCl to 25.0 mL of a 0.10 M NHz solution and indicate the "buffer zone".
21. What are the characteristics of the carbonic acid-bicarbonate buffer system (select all that apply? a CO2 is eliminated by the lungs b. Neutralizes HCl acid to yield carbonic acid and salt c. H2CO3 formed by neutralization dissociates into H2O and CO2 d. Shifts H+ in and out of cell in exchange for other cations such as potassium and sodium e. Free basic radicals dissociate into ammonia and OH-, which combines with Ho to form water 22. What are characteristics...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
Post Lab Activity Acids, Bases, pH, and Buffers 1. Calculate the pH of a 0.08 M NaOH solution. 2. Hydrochloric acid is a strong acid and dissociate almost 100% in aqueous solution. If two drops (0.1 mL) of 1.0 MHCI are added to pure water to make 1.0 L solution. What is the pH of this solution? 3. M. What will be the A dilute solution of hydrochloric acid (HCI) has a concentration of 0.1 pH of this solution? 4....
Select the solution that would resist a change in pH upon the addition of a small amount of acid or base. a. A solution containing 0.10 M NaCl and 0.10 M HCl b. A solution containing 0.05 M NH3 and 0.10 M NH4Cl c. A solution containing 0.10 M HCl and 0.05 M NaOh d. A solution containing 0.10 M NaOH and 0.75 M NaCl
For the following buffer system: a. Calculate the concentrations of the major species present in a buffer solution prepared by mixing 12.5g of sodium acetate (NaCH3CO2, a salt) in 325mL of 1.5M acetic acid (CH3CO2H(aq), a weak acid). Ka,CH3CO2H = 1.8x10-5 . b. Write out the acid-base reaction of this solution and identify the conjugate acid base pairs. c. Calculate the pH of this acidic buffer solution. d. By how much would the pH of the solution change if 10.0mL...