Answer :
Buffer contain H2CO3 and HCO3 - species .
(5) Balanced Reaction when HCl was added to the buffer
Carbonic acid being acid will not react with HCl , however bicarbonate ion react with HCl to produce more carbonic acid which decreases the pH .
HCO3 - (aq) + HCl -----> H2 CO3 (aq) + Cl- (aq)
(6) : Balanced Reaction when NaOH is added to the buffer
Carbonic acid will react with OH- ions produced by NaOH , to form bicarbonate ion which are basic in nature and increase pH of the system
H2 CO3 (aq) + OH- (aq) ----> HCO3 - (aq) + H2O
Part 3: Preparing and testing the carbonic acid/bicarbonate buffer 3) and 6) Buffer 0.1 MHCI A:...
\ Part 3: Preparing and testing the carbonic acid/bicarbonate buffer 3) and 6) Buffer 0.1 MHCI A: Buffer A: Buffer B: Butter B: Buffer Part 4: Testing water for pH resistance 2) and 5) DFDFDF A: HO B: H0 Question 6 1 pts pH in Beaker A pH in Beaker B After 5 drops NaOH Solution Initial After 5 drops HCI After 20 drops HCI Initial After 20 drops NaOH Buffer (part 3) Water (part 4) Use the data...
The question is Did the combination of carbonic acid and bicarbonate function as a buffer? Support your response with data. Buffers are chemical mixtures that resist pH change when exposed to acids or bases. They contain both a weak proton donor and weak proton acceptor. The former neutralizes any strong bases added and the latter neutralizes any strong acids added to the buffer. Our bodies rely upon a combination of three different buffers to maintain stable pH: the bicarbonate buffer...
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...
Activity 4: Double-Replacement Reaction Describe the reaction of sodium bicarbonate and vinegar. Refer to the section in the Background titled, “Standard Tests Gaseous Products.” Use a flaming splint and a glowing splint to identify the gas above the liquid in the cup. Write the name and formula of the gas in the space provided. Write a balanced chemical equation for this double-replacement reaction. One of the two products of this reaction is carbonic acid (H2CO3), which immediately forms water and...
A chemist prepared an aqueous buffer containing both formic acid (HCOOH) and the formate anion. The volume of the buffer is 100 mL ; with [HCOOH] = 0.110 mol L-1 and [HCOO- ] = 0.101 mol L-1 . The pKa of HCOOH = 3.74. What is the pH of this buffer? Write down the balanced chemical equation that describes the reaction of this buffer when an HCl solution is added. c) What is the resultant pH of this solution after...
Please answer questions 1-6 Drops of HCI added PH Beaker 1 Acetic Acid + Sodium Acetate pH Beaker 2 Blood Buffer PH Beaker 3 Water O drops 14.83 15.01 9.73 9.00 4.83 4.78 3.00 2.66 8.92 NJ 0 = 8.82 2.44 4:75 4.71 4.66 8 69 2. 29 I 2.18 8.44 4.60 nos 2,10 Drops of NaOH added pH Beaker 1 Acetic Acid + Acetate pH Beaker 2 Blood Buffer pH Beaker 3 Water 0 drops wastlab Questions 1. According...
Part 3: Working with the Titration Curve for a Polyprotic Acid and Strong Base Consider carbonic acid, H.CO, (which is polyprotic) - a) Write the multi-step dissociation equilibrium for this acid in water (ie, there should be three chemical dissociation stages connected by two equilibrium arrows, given below): b) Below is an idealized titration curve showing the exhibited pH for 25.00 mL of a 0.100 M aqueous carbonic acid solution as a function of added 0.100 M NaOH in units...
2) Draw the 2 reactions of the weak acid, Carbonic Acid (H2CO3) with water. Which form of carbonic acid predominates at physiological pH? The two pKas of carbonic acid are the following: pK,1 = 6.4 pK,2 = 10.3. (3 points) 3) You have a 0.1 M solution of HCl in water. HCl is a strong acid. What is the pH of this solution? (Show your work or will not receive credit.) (2 pts.) 4) Calculate the pOH of a solution...
You need to prepare a buffer with pH of 4.35. You are to start with 20.0 mL of 0.30 M HCl (aq). The other reagents that you have available to add to this HCl solution are: a.) 1.00 M NaH2PO4 (aq) b.) 1.00 M Na2C2O4 (aq) c.) Solid NaNO2 1.) Using only the reagents you have available (listed above), choose an appropriate weak acid/ conjugate base pair for this buffer. 2.) Write the balanced net-ionic equation for the chemical reaction...
Part IV. Decomposition Into a test tube, place about 2 mL of 3% hydrogen peroxide along with a pea size amount of Mnog Manganese dioxide, the common name, is used as a catalyst. Remember, that a catalyst is used to lower the activation energy of a reaction, thereby speeding up the reaction. It does not get con- sumed in the reaction and therefore is not part of your balanced chemical equation. It is written above the reaction arrow in a...