Consider the reaction: H2SO3 + HCO3- ----> H2CO3 + HSO3-
If HCL is added to the buffer you proposed (H2SO3,HSO3-), show with a chemical equation how this buffer maintains the pH.
The given buffer reaction: H2SO3 + HCO3- ----> H2CO3 + HSO3- and pH = pKa + log( HSO3- / H2SO3)
If small amount of HCl is added to the given buffer, then added HCl reacts with the equivalent amount of conjugate base, HSO3- according to following equation
HSO3- + HCl
H2SO3 + Cl-
The above reaction results in the formation of undissociated H2SO3 (due to common ion effect). Therefore, the ratio of [HSO3-] /[ H2SO3] is changed slightly and the buffer maintains the pH.
Consider the reaction: H2SO3 + HCO3- ----> H2CO3 + HSO3- If HCL is added to the...
Consider a solution consisting of the following two buffer systems: H2CO3 HCO3– + H+ pKa = 6.4 H2PO4– HPO42– + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? ***Please explain why the right answer is right and why the other ones are wrong. a. [H2CO3] > [HCO3- ] and [H2PO4- ] > [HPO42- ] b. [HCO3- ] > [H2CO3] and [HPO42- ] > [H2PO4-...
A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.
Consider the following buffer system: 0.0024 M H2CO3 and 0.024 M HCO3-. What is the pH of such a system (Kg = 4.3 x 10-7? Ca) pH = 7.37 b) pH = 7.00 c) pH = 5.36 Od) pH = 8.90 Question 6 (5 points) Water can act as a buffer system since it has hydroxide and hydronium ions both present at the same time. True False
3. a. Use the Henderson-Hasselbach equation to determine the ratio of HCO3- to H2CO3 in the patient’s blood 10 hours after aspirin ingestion. b. How does this compare to the ratio of HCO3- to H2CO3 in normal blood (indicate value used from the range given in the table). (pKa1=6.35). c. Can the H2CO3/HCO3- system serve as an effective buffer in this patient? Explain
Consider the reaction below. Which species are conjugate
acid/base pairs?
HSO3-(aq)+HCN(aq)H2SO3(aq)+CN-(aq)
In waters affected by acid rain the concentrations of the three carbonic acid species (H2CO3, HCO3-, CO32-) are determined by concentration of the strong acid deposited by acid rain, as well as the concentration of H2CO3 which is controlled by the solubility of carbon dioxide . Under these conditions (constant H2CO3 and relatively low pH) the only carbonic acid equilbrium of importance is the conjugate base reaction of HCO3-, which is related to, but not identical to - and not...
4. Consider the following reaction: H2CH:07 "(ag) + H2CO3(aq) = HCO3(aq) +H3C6H501(a) a. Label the acid, conjugate acid, base, and conjugate base in the equation above. (4 points) b. In the table below, you will find some potentially useful information to answer the following question: Do you expect products or reactants to be favored at equilibrium? Explain. (Use one or two complete sentences to explain your answer.) (4 points) Compound/Ion HCO, H2CO3 HAC-HO- H.C.H.O K. 4.80 x 10" 4.30 x...
complete the following acide base reaction:
HCL + HCO3-->
QUESTION 2 Complete the following acid base reaction: HCI (aq) + HCO3- (aq) → H2CIO (aq) + CO2(g) O Cl2 (g) + H2CO3 (aq) H2C11+ (aq) + CO32- (aq) 017- (aq) + H2CO3 (aq)
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
17. Which of these acids is the strongest? A) H2SO3 B) H2SO3 C) H2TeO3 18. Which one of these net ionic equations represents the reaction of a strong acid with a weak base? A) H(aq) + OH(aq) + H2O(aq) B) H(aq) + CH3NH2(aq) → CH3NH3(aq) C) OH(aq) + HCN(aq) → H2O(aq) + CN-(aq) D) HCN(aq) + CH3NH2(aq) → CH3NH3+ (aq)+ CN (aq) 19. Predict the direction in which the equilibrium will lie for the reaction H2CO3 + HCO,- + HF....