Find the pH of a 0.135 M aqueous solution of hypobromous acid (HOBr), for which Ka = 2.06 x 10-9. The add dissociation constant K_a of carbonic acid (H_2CO_3) s 4.5 * 10^-7. It is generated both biologically and commercially as a disinfectant. Its chemical and physical properties are similar to those of other hypohalites. Plug the values into Henderson-Hasselbalch equation. (Ka = 2.0 x 10-9), Calculate the H3O+ in a 1.4 M solution of hypobromous acid. Let's assume that it's equal to 0.1 mol/L. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. To determine :- conjugate base of given species. What is the pH of a 0.00100 F solution of hypobromous acid (HOBr) in pure water? All other trademarks and copyrights are the property of their respective owners. Hypochlorus acid has an acid ionization constant K_a, equal to 2.9 x 10^{-8}. pyridine Kb=1.710 5.0 times 10^{-9} c. 3.4 times 10^{-7} d. 3.5 times 10^{-5} e. 7.1 times 10^{-5}. Calculate the pH of the solution at . name: Given that acetic acid hasKa= 1.8 x 105, what is the pH of a solution that contains the molar ratio of conjugate base-to-acid: [CH3CO2]/[CH3CO2H] = 1/10? {/eq} at 25 degree C, what is the value of {eq}K_b Kb of NH3 = 1.76 105, What is the pH of a 0.150 M solution of CH3COOH? Calculate the concentration of OH- and the pH value of an aqueous solution in which (H3O+) is 3.65 x 10^-9 M at 25 degrees Celsius. $ What is the pH of a 0.200 M H2S solution? What is the value of Ka for HBrO? A 0.190 M solution of a weak acid (HA) has a pH of 2.98. Determine the acid ionization constant (K_a) for the acid. Calculate the acid dissociation constant K_{a} of carbonic acid. What is the pH of a 0.040 M solution of chloroacetic acid, for which Ka = 1.36 * 10^{-3}? The value of Ka for HBrO is 1.99 10. Calculate the acid dissociation constant Ka of pentanoic acid. The Kb of NH3 is 1.8 x 10-5. Addition of bromine to water gives hypobromous acid and hydrobromic acid (HBr) via a disproportionation reaction. Express your answer using two significant figures. A 0.115 M solution of a weak acid (HA) has a PH of 3.33. Calculate the pH of a 0.719 M hypobromous acid solution. Using the answer above, what is the pH, A:Given: NH/ NH3 What is the pH of a 0.0157 M solution of HClO? What is the, Q:The value pKw is 11.05 at 78 C. (Ka = 2.0 x 10-9), Calculate the H3O+ in a 1.7 M solution of hypobromous acid. (Ka = 2.0 x 10-9). b) What is the % ionization of the acid at this concentration? Ka of HBrO is 2.3 x 10-9. Express your answer using two decimal places. Kb of C5H5N = 1.7 109, What is the pH of a solution that has 0.200 M HF and 0.200 M HCN? {/eq} for {eq}BrO^- Calculate the pH of a 0.591 M aqueous solution of phenol. A 9.0 times 10^{-2} M solution of a monoprotic acid has a percent dissociation of 0.58%. What is the value of Ka for the acid? is a STRONG acid, meaning that much more than 99.9% of the HBr A)9.9 10-2 B)1.2 10-5 C)2.8 10-12 D)6.9 10-9 E)1.4 10-10 16) 17)The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25.0 C is 4.48. What is the value of K_a for HBrO? An 8.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.63%. All other trademarks and copyrights are the property of their respective owners. Round your answer to 2 decimal places. (Ka for HF = 7.2 x 10^-4). What is the pH of an aqueous solution at 25 degrees C in which (H+) is 0.025 M? (Ka = 2.5 x 10-9). Ka of HBrO = 2.8 109 4.74 What is the pH of a 0.250 M solution of HCN? Round your answer to 1 decimal place. conjugate acid of SO24:, A:According to Bronsted-Lowry concept A:The given reaction is an acid-base reaction, Q:Consider the following acid-base pairs: Kaof HBrO is 2.3 x 10-9. The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25 C is 4.48. Given that Kb for CH3CH2NH2 is 6.3 10-4 at 25 C, what is the value of Ka for CH3CH2NH3 at 25 C? Study with Quizlet and memorize flashcards containing terms like Which of the following is the correct expression for the pressure based equilibrium constant for the reaction: 2 HI (g) H (g) + I (s), For the reaction below, Kc = 9.2 10. What is the pH of an aqueous solution of 3.80 x 10^{-2} M hydroiodic acid? 0.0003), Calculate the pH, the fraction of dissociation (alpha, alpha), and the alpha % of a 0.020 M solution of hypochlorous acid (HOCl), a monoprotic acid with a K_a = 3.0 times 10^{-8}. What is the pH of a 0.35 M aqueous solution of sodium formate? What is the pH of a 0.150 M NH4Cl solution? The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25^\circ C is 4.48. Calculate the pH of a 0.50 M NaOCN solution. Calculate the H3O+ in a 0.285 M HClO solution. 80 The Ka for hypobromous acid, HBrO, is 2.0 x 10-9. esc e. H2C2O4(aq) + H2O (l) HC2O4-(aq) + H3O+(aq) =. Other relevant reactions in such oscillating reactions are: Bromites reduce permanganates to manganates (VI):[1]. Find the percent dissociation of this solution. + PO,3 The Ka of HCN is 6.2 times 10^(-10). What is the K_b and a (degree of ionization) of NH_3 (aq) for the following pH and concentrations? 7.1 10 4 b. 2007-2023 Learnify Technologies Private Limited. Step by step would be helpful. HPO24+HBrO acid+base Acid: Base: chemistry. 8.3. c. 9.0. d. 9.3. A 0.150 M weak acid solution has a pH of 4.31. In a 0.25 M solution, a weak acid is 3.0% dissociated. 2.3 10 M. A neutral solution of water at a particular temperature has a concentration of OH of 2.3 10 M. What is Kw at this temperature? Round your answer to 1 decimal place. Find th. 6.67. c. 3.77. d. 6.46. e. 7.33. :. Each compound has a characteristic ionization constant. Part A Given that Ka for HCN is 4.9 * 10-10 and Kb for NH3 is 1.8 * 10-5, calculate Kb for CN- and Ka for NH4+. What is the pH of an aqueous solution with H3O+ = 9.2 x 10-2 M? What is the [OH-] in an aqueous solution with a pH of 7? Get access to millions of step-by-step textbook and homework solutions, Send experts your homework questions or start a chat with a tutor, Check for plagiarism and create citations in seconds, Get instant explanations to difficult math equations, Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. What is the pH of a 0.14 M HOCl solution? What is the pH of an aqueous solution of 2.20 \times 10^{-2} M potassium hydroxide? What is [OH]? what is the value of Kb for C_2H_3O_2-? The Ka of HBrO is at 25 C. . The H-O bond is weakened or increasingly polarized by the additional oxygen atoms bonded to the central bromine atom in HBrO3. (a) Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. Upon treatment of these aqueous solutions with salts of Pb2+, Hg2+, and Ag+, the corresponding heavy metal bromites precipitate as solids. Q. NH3, A:When valence electrons present in atoms of a compound are represented by dots in a structure then it, Q:Lithium dihydrogen borate (LIH2BO3) is the lithium salt Find the pH of an aqueous solution that is 0.0500 M in HClO. A 9.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.58%. pH =, Calculate the pH of a 0.225 M monoprotic acid (HA). The Ka of HCN is 4.9 x 10-10. E) 1.0 times 10^{-7}. (a) HSO4- (Ka of HC?H?O? Ka1 of H2S = 8.9 108 and Ka2 = 1 1019, Elementary Differential Equations and Boundary Value Problems, Douglas B. Meade, Richard C. Diprima, William E. Boyce, Elementary Differential Equations & Boundary Value Problems, Fundamentals of Differential Equations and Boundary Value Problems, Arthur David Snider, Edward B. Saff, R. Kent Nagle, Solve each equation. The concentration of an aqueous solution of HCN is 0.05 M. Calculate the pH of the solution. W The acid dissociation constant of bromous acid, Ka = .mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num,.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0 0.1em}.mw-parser-output .sfrac .den{border-top:1px solid}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}[H+][BrO2]/[HBrO2], was determined using different methods. The chemical formula of hydrobromic acis is HBr. (Ka = 2.8 x 10-8), What is the hydronium ion concentration in a 0.410 M OCl- solution? The K_a for formic acid (HCO_2H) is 1.8 .10^{-4}. (Ka = 1.0 x 10-10). The pH of a 1.3 M solution of carbonic acid (H_{2}CO_{3} is measured to be3.12. What is the pH of a 0.186 M aqueous solution of sodium fluoride, NaF? K, =, Q:For each pair of molecules or ions, select the stronger base and write its Lewis structure. Ka of HCOOH = 1.8 104, What is the pH of a 0.350 M MgF2 solution? Determine the Ka value for an acid where a 0.05 M solution has a measured pH of 3. Get access to this video and our entire Q&A library. 2 . (Ka (HCOOH) = 1.8 x 10-4). : \qquad \small \rm HCOOH = HCOO^- + H^+ HCOOH = HCOO +H+ \qquad \rm \small Ka = \frac { [H^+] [HCOO^-]} { [HCOOH]}, Ka = [HCOOH][H+] [HCOO], where: Based on Henderson-Hasselbalch equation, pH = pKa + log ( (A-)/ (HA)) Initially, there are 0.0035 M of HBrO. Q:what is the conjugate base and conjugate acid products with formal charges? 1.25 B. Calculate the pH of a 4.0 M solution of hypobromous acid. Step 1: To write the reaction equation. Calculate the acid ionization constant (Ka) for the acid. The pH of a 0.68M solution of pentanoic acid HC5H9O2 is measured to be 2.50. Vip Thumbnail | 2 Thumbnail ,android phone se youtube thumbnail kaise banaye,how to make thumbnail for . A diprotic acid, H2A, has acid dissociation constants of Ka1 = 1.29 * 10^{-4} and Ka2 = 2.77 * 10^{-12}. 3.28 C. 1.17 D. 4.79 E. 1.64. Given that Ka for HCN is 6.2 x 10^-10 at 25 C, what is the value of Kb for CN- at 25 C? (Ka = 2.0 x 10-9), Calculate the pH of a 1.3 M solution of hypobromous acid. For the above reaction determine the Kb of the base (CN-) if the Ka of the conjugate acid is 2.3 x 10-4. hich of the following bases has the greatest degree of ionization? (Ka for HNO2 = 4.5 x 10-4). x = 38 g 1 mol. Calculate the concentration of OH- and the pH value of an aqueous solution in which (H3O+) is 0.014 M at 25 degrees Celcius. With four blue flags and two red flags, how many six flag signals are possible? Calculate the acid ionization constant (K_a) for the acid. $6 \%$ of $\underline{\qquad}$ is $0.03$. What is Kb for the conjugate base of HCN (Ka = 4.9 10)? What is the hydronium ion concentration and pH of a 0.10M solution of hypochlorous acid, ka =3.5 x10^-8? A 0.0115 M solution of a weak acid has a pH of 3.42. Given that Kb for CH3NH2 is 5.0 x 10-4 at 25 C, what is the value of Ka for CH3NH3 at 25 degree C, 1.) %3D pH = A: Click to see the answer Q: What is the pH of a 0.0620 M solution of hydrocyanic acid, HCN (Ka = 4.9 101)? All rights reserved. pH of, Q:(a) Give the conjugate base of the following BrnstedLowry acids: (i) HCOOH, (ii) HPO42-. Find the pH of a 0.0191 M solution of hypochlorous acid. Remember to convert the Ka to pKa. (The Ka of HOCl = 3.0 x 10-8. hydroxylamine Kb=9x10 K_a = Our experts can answer your tough homework and study questions. The pH of an aqueous 0.50 M hypochlorous acid solution is 3.88. R Acid : Acid is, Q:Carbon dioxide (CO2) will react with an oxide ion (O2-) to form CO32- (Ka = 3.0 x 10-8), What is the pH of 0.015 M aqueous benzoic acid? Q:Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5. Calculate the pH of an aqueous solution with H3O+ = 1.20 x 10-12 M. Calculate the pH of an aqueous solution with H3O+ = 4.8 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 3.11 x 10-5 M. Calculate the pH of an aqueous solution with H3O+ = 0.000524 M. Calculate the pH of an aqueous solution with H3O+ = 3.9 x 10-4 M. Calculate the pH of an aqueous solution with H3O+ = 0.000485 M. Calculate the pH of an aqueous solution with H3O+ = 3.22 x 10-11 M. Calculate the pH of an aqueous solution with H3O+ = 0.000085 M. Calculate the pH of an aqueous solution with H3O+ = 7.0 x 10-10 M. Calculate the pH of an aqueous solution with H3O+ = 3.50 x 10-3 M. Calculate the pH of an aqueous solution with H3O+ = 1.78 x 10-11 M. Calculate the pH of an aqueous solution with H3O+ = 2.65 x 10-5 M. Calculate the pH of an aqueous solution with H3O+ = 2.4 x 10-5 M. Calculate the pH of an aqueous solution with H3O+ = 0.022 M. Calculate the pH of an aqueous solution with H3O+ = 6.88 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 1.58 x 10-4 M. Calculate the pH of an aqueous solution with H3O+ = 3.79 x 10-7 M. Calculate the pH of an aqueous solution with H3O+ = 0.000032 M. Calculate the pH of an aqueous solution with H3O+ = 0.000559 M. Calculate the pH of an aqueous solution with H3O+ = 0.000364 M. Calculate the pH of an aqueous solution with H3O+ = 0.000240 M. Calculate the pH of an aqueous solution with H3O+ = 3.42 x 10-3 M. Calculate the pH of an aqueous solution with H3O+ = 0.000745 M. Calculate the pH of an aqueous solution with H3O+ = 1.86 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 6.2 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 9.15 x 10-6 M. Calculate the pH of an aqueous solution with H3O+ = 8.45 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 2.85 x 10-4 M. Calculate the pH of an aqueous solution with H3O+ = 0.0000830 M. Calculate the pH of an aqueous solution with H3O+ = 2.0 x 10-5 M. Calculate the pH of an aqueous solution with H3O+ = 8.69 x 10-9 M. Calculate the pH of an aqueous solution with H3O+ = 1.34 x 10-4 M. The pH of a 0.250 M cyanuric acid solution is 3.690. (Ka for CH3COOH = 1.8 x 10-5). 5.90 b. The Ka for formic acid is 1.8 x 10-4. 1 point earned for mol NaOBr (e) HOBr is a weaker acid than HBrO3. 2.5 times 10^{-9} b. The dissociation constant, Ka, for gallic acid is 4.57 x 10-3. Round your answer to 2 decimal places. Part A What is the [H_3O^+] of 0.146 M HNO? However the value of this expression is very high, because HBr A)1.1 10-9 B)3.3 10-5 C)2.0 10-9 D)3.0 104 E)6.0 10-5 17) 2. pH =. Ximenes, V. F., Morgon, N. H., & de Souza, A. R. (2015). Is this solution acidic, basic, or neutral? A:We have given that (The value of Ka for hypochlorous acid is 2.9 * 10-8. solution of formic acid (HCOOH, Ka = 1.8x10 What is the pH of a 6.00 M H3PO4 solution? The hypobromite anion is a weak base that will Our experts can answer your tough homework and study questions. What is the pH of a 0.546 M hypochlorous acid, HOCl, solution? (Ka = 2.9 x 10-8). An aqueous solution has a pH of 4. Write answer with two significant figures. An acid donates a hydrogen ion to form its conjugate base, A:Given :- chemical formula = HCO3- (Ka = 4.9 x 10-10), Calculate the pH of a 1.7 M solution of hydrocyanic acid. A 0.180 M solution of a weak acid (HA) has a pH of 2.96. CO2 + O2- --> CO3^2- An 8.0 x 10^-2 M solution of a monoprotic acid has a percent dissociation of 0.56%. What is the value of k_b for the hydrolysis reaction: A^- + H_2O to HA + OH^-. The Ka of HCN = 4.0 x 10-10. We store cookies data for a seamless user experience. Our experts can answer your tough homework and study questions. k a for hypobromous acid, hbro, is 2.0 10-9. karlibghs5921 karlibghs5921 07/30/2018 Chemistry College answered expert verified . Since the moles are the same, this tells us that ALL of the KOH was converted to KBrO. Ka of HF = 3.5 104, What is the pH of a solution that has 0.300 M HNO2 and 0.300 M HCN? K a = [product] [reactant] K a = [H 3 O + ] [CH . The value of Ka for HCOOH is 1.8 times 10-4. Round your answer to 1 decimal place. T Y U, Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell, Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres. Identify the, A:The given reaction is an acid base reaction the species releasing a proton is an acid while the, A:According to the Bronsted-Lowry theory, a proton (H+) donor is an acid and a proton acceptor is a, Q:What is the pH of a 0.0570 M solution of hydrocyanic acid, HCN (Ka = A:The given anion C4H5O3 is also basically a conjugated base generated from C4H6O3 on deprotonation. (b) calculate the ka of the acid. What is the pH of 0.25M aqueous solution of KBrO? Kb of CH3NH2 = 4.4 104, What is the pH of a 0.280 M solution of (CH3)2NH? What is the buffer component ratio, ([BrO-]/[HBrO]) of a bromate buffer that has a pH of 9.88. A 0.159M solution of a monoprotic acid has a percent ionization of 1.25%. nearly zero. Calculate the pK_a of an acid if its K_a is 2.3 \times 10^{-3}. The Ka for hypobromous acid, HOBr is 2.5 x 10-9. a) What is the pH of a 0.11 M solution of the acid? The Ka for acetic acid is 1.7 x 10-5. a. (Ka = 2.0 x 10-9), Calculate the pH of a 1.7 M solution of hypobromous acid. Calculate (KF) in a buffer where (HF) = 0.14 M and pH = 3.90. The Ka for HBrO is 2.3 x 10-9. b. What is the value of Ka for the acid? The Ka of HBrO is at 25 C. What is the pH of What is the pH of a 0.25 M aqueous solution of KCHO2 at 25 C? All other trademarks and copyrights are the property of their respective owners. [10] Rate constants of bromite towards carbocations and acceptor-substituted olefins are by 13 orders of magnitude lower than the ones measured with hypobromite. Calculate the pH of a 2.3 M aqueous solution of benzoic acid. What is the pH of a 0.225 M KNO2 solution? Hypobromous acid (HBrO) is a weak acid. What is the percent ionization of the acid at this concentration? v.25 1906", "Spatial and Temporal Control of Information Storage in Cellulose by Chemically Activated Oscillations", https://en.wikipedia.org/w/index.php?title=Bromous_acid&oldid=1021731481, This page was last edited on 6 May 2021, at 10:59. Alternatively, you can determine this constant by solving the {eq}K_a {/eq} expression using a known hydronium ion molarity (from the pH) and starting acid molarity. Calculate the acid dissociation constant Ka of propanoic acid. What is the value of Ka for the acid? Using this method, the estimated pKa value for bromous acid was 6.25. # Determine the pH of a 0.98 x 10^(-2) mol L solution of hydrocyanic acid (HCN) Ka = 4.0 x 10^(-10). The pH of your solution will be equal to 8.06. What is the pKa? What is the value of it"s k_a? Calculate the pH of a 1.60 M KBrO solution. a. Ka of HF = 3.5 104 and Ka of HClO = 2.9 108. Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka = 1.1 times 10-5. The pH of a 0.051 M weak monoprotic acid solution is 3.33. What are the 4 major sources of law in Zimbabwe. Learn about conjugate acid. HCO, + HPO,2 H2CO3 Kb of base = 1.27 X 10-5 Therefore the molarity values of hydronium ion (responsible for the solution pH) and weak conjugate base products are significantly smaller than the starting acid molarity before dissociation. What is the pH of a 0.1 M aqueous solution of NaF? What is the pH of the buffer after the addition of the KOH (assuming the addition of KOH does not affect the volume)? (Ka of C5H6CO2H = 6.3 * 10-5), What is the hydronium ion concentration of an aqueous solution of 0.523 M hypochlorous acid? A strong acid ionizes completely in an aqueous solution by losing one proton, according to the following equation: where HA is a protonated acid, H + is the free acidic proton, and A - is the conjugate base. Salt hydrolysis is the reaction of a salt with water. 4.9 x 1010)? On this Wikipedia the language links are at the top of the page across from the article title. Weekly leaderboard Home Homework Help3,800,000 Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. What is the value of Kb for CN-? [BrO-] = 0.006 mols / 0.06 L = 0.1 M (0.06 L comes from adding 40 ml + 20 mls to get final volume) To find the pH, we need to look at the hydrolysis of the salt. pH = What is the pH of a 0.0944 M aqueous solution of formic acid, HCOOH? What is the % ionization of the acid at this concentration? Given that Ka for HBrO is 2.8 * 10^-9 at 25 degree C, what is the value of Kb for BrO- at 25 degree C 2.) F6 Bromic acid | HBrO3 or BrHO3 | CID 24445 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities . a. HSO3-(aq) + H2O (l) SO32-(aq) + H3O+(aq) = H2CO/ HCO b) What quantity in moles of C7H5O2 would be present before the reaction takes place? hypobromous acid, bromic(I) acid, bromanol, hydroxidobromine, Except where otherwise noted, data are given for materials in their. Hence it will dissociate partially as per the reaction 6) Consider the mixing of sodium hypobromite (NaBrO) into 2.00 of 0.25 M hypobromous acid (HBrO) to form a buffer solution (Ka of HBrO = 2.3 x 10-92 Assuming that no volume change occurs when the NaBrO is added, Calculate the number of moles of NaBrO need to be added into the solution to form buffer solution with pH of &8.20 ii, Calculate the Ka for HNO_2 is 5.0X 10^-4. a. A 0.120 M solution of a weak acid (HA) has a pH of 3.33. Round your answer to 1 decimal place. (Ka = 2.0 x 10-9), What is the pH of a solution that is 0.026 M in HA and also 0.0060 M in NaA? of the conjugate base of boric acid. We know that x = [ H 3 O +] = [ CH 3 COO] .Since CH 3 COOH is a weak acid, its K a must be very small. A solution of formic acid 0.20 M has a pH of 5.0. Calculate the pH of a 1.4 M solution of hypobromous acid. 2 4. Round your answer to 2 significant digits. The Ka of HCN is 6.2 x 10-10. Ka of HBrO = 2.8 109, What is the pH of a 0.250 M solution of HCN? The ka of hypochlorous acid HClO is 3.5 \times 10^{-8}. Ka of HF = 3.5 104. A 0.060 M solution of an acid has a pH of 5.12. What is the value of K_a, for HA? A 9.0 times 10^{-2} M solution of a monoprotic acid has a percent dissociation of 0.55%. What is the Ka of a particular acid if a 2.10 x 10-2 M aqueous solution of it has a pH of 4.87? Calculate the pH of a 0.43M solution of hypobromous acid. What is the pH of a 0.435 M CH3CO2H solution? copyright 2003-2023 Homework.Study.com. The K_a for HCOOH is 1.8 x 10^-4 M. As usual, report pH to 2 decimal places. What is the value of K_a for HBrO? What is the pH of a 0.55 M aqueous solution of HBrO at 25 degree C?