For the second dissociation of H, CO3: HCO3(aq) + H,O=H;O) + COaq) + CO3(aq) (1) a. At what volume of added HNO, does the pH = pKa? b. What is the pH at this point? c. What is the pk, for the first dissociation according to the literature?
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- For the first dissociation of H,CO3: H,CO3(aq) + H,O = H;O Cag) + HCO3(aq) a. At what volume of added HNO, does the pH = pKg? b. What is the pH at this point? c. What is the pką for the first dissociation according to the literature? d. What is your percent error for this pka value? Show your work. Experimental value-Accepted value Accepted value :) × 100% Percent Error3) What is the pH of a 0.02 M solution of sodium propionate? (12 pts) Reaction of sodium propionate in water: Pr (aq) + H₂O (1) ⇒ HPr (aq) + OH-(aq) Ka= 10-4.⁹ *Hint* This is a Kb problem therefore you must convert ka to Kb. You can assume that the sodium propionate dissociates completely from the propionate and is not involved in any other important reactions. a) Is this the conjugate base or an acid that you are adding to solution? b) Write down the Mass-Balance Relations, the Proton Balance Relation and the c) Equilibrium Relation. Calculate the pH using both an analytic method, and by drawing the predominance diagram. *Hint* [OH-]=[HPr].Unit 20 3. The carbonate buffer system is very important in regulating blood pH levels. Carbonic acid is diprotic and therefore has two Ką values: H₂CO3(aq) H+(aq) + HCO3-(aq) HCO3-(aq) = H+(aq) + CO3²-(aq) Kaj = 4.2 x 10-7 Ka2 = 4.8 x 10-11 Since the second dissociation has a Ka value significantly smaller than that of the first dissociation, it can be assumed to have no effect on the H₂CO3(aq)/HCO3(aq) equilibrium. blood? The pH of blood is 7.4. What is the ratio of carbonic acid to bicarbonate ion in stalvols) .seang obixoib sullus bre obitlure nog notionen eidt tot agaedo
- 1. The Kb of HONH2 is 1.1 x 10-8. Calculate the pH and percent dissociation of a solution containing 0.100 M HONH2. а. b. Calculate the pH and percent dissociation of a mixture containing 0.100 MHONH2 and 0.100 M HONH3CI.At 25oC, the Ka for a certain monoprotic acid HA is 6.2x10-10. What will be the Ka value for the given reaction below?1/2Ha(aq) + 1/2H2O(l) <-> 1/2A-(aq) + 1/2H3O+(aq) Choices:1.6x10-53.8x10-192.5x10-56.2x10-10The concentration of carbonic acid, H2CO3, in a typical carbonated drink is approximately 7.0 x 10-2 M. Carbonic acid is a diprotic weak acid with the following pKa values for the 1st and 2nd ionizations: H2CO3 + H2O <===> H3O+ + HCO3- pKa = 6.3 HCO3- + H2O <===> H3O+ + CO32- pKa = 10.3 From highest concentration to lowest concentration, what are the molecular and ionic species present in an aqueous solution of 7.0 x 10-2 M H2CO3 (note: you do not have to calculate the concentrations, just rank them in order of highest to lowest).
- 1. Calculate [H+], [OH-], pH and pOH of:a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4) 2. In the preparation of the standard curve for protein analysis, 50 mnBSA (bovine serum albumin) dissolved in H2O to a final volume of 5mL was used as stock solution. What is the weight of BSA in 0.1 mL ofstock solution? In 0.2 mL? 3. . The above mentioned aliquots (#9) which were diluted with enoughwater to a final volume of 1 mL were assayed colorimetrically andyielded the following absorbance readings:mL stock mL H2O Absorbance0.2 0.8 0.1000.4 0.6 0.2000.6 0.4 0.3000.8 0.2 0.4001.0 0.0 0.500 i. Tabulate mg BSA vs. absorbance readingii. Draw the curve where mg BSA is on x-axis and absorbance ony-axis (use graphing paper).iii. Calculate the slope of the curveiv. If a sample solution has an…Asiacell 36, Asiacel 9:18 1 %OY A 46 Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate the ionization constant for the weak acid 10-2 O 10-6 10-5 Q2// 1000 ml ofo.1M hydrochloric acid were added to 1000 ml of o.IM ammonium hydroxide, ammonium chloride salt was formed. Calculate the pH for the salt solution. Kb=1.8 ×10-5 10.02 3.98 5.28 Q3// Calculate the sodium acetate10:06 PM Mon Apr 11 < 88 Q A O Exp 7 Prelab x Worksheet 16 Wea. x Worksheet 19 Titr Planne Exp 7 Prelab x S22 1020 Unit 1 P. x Worksheet 15 Acid. Anatomy T 2. A solution has a [H,O" 0]= 1.00x10“ M. WAD a. Calculate the pH. UN (aq) b. Is the solution acidic or basic? NAN
- please answer on 1-a,b,c,d. Clear handwriting or type in, thank you! 1. The mixture of anions is an effective blood buffer with the following acid-base equilibrium: HO" (aq) + HPO* (aq) H:POs (aq) + H;O (1) a. For the equilibrium above, what is the effect of decreasing the pH? (give shift) b. As a result of the shift, which ion H:PO, or HPO, would appear to increase? c. For the equilibrium above, what is the effect of increasing the pH? (give shift) d. As a result of the shifl, which ion H:PO, or HPO would appear to increase?A group of students perform a titration experiment. The buret tube is filled to the 0.00ml line with 0.100M NaOH solution. The E. flask contains 50.0ml ov 0.100M HC2H3O2 solution. The Ka of the acetic acid is: Ka = 1.8 x 10-5. A) Write the ionic equation for the conjugate acid reactihng with water. One product is the OH- polyatomic ion. B) What is the pH of the equivalence point?10. The K₂ of HONH₂ is 1.1 x 10-8. a. Calculate the pH and percent dissociation of a solution containing 0.100 M HONH2. b. Calculate the pH and percent dissociation of a mixture containing 0.100 M HONH2 and 0.100 M HONH3CI. (Assume complete dissociation of HONH3CI.)