Based on Henderson-Hasselbalch equation, pH = pKa + log ( (A-)/ (HA)) Initially, there are 0.0035 M of HBrO. The Ka of HCN = 4.0 x 10-10. (Ka = 1.8 x 10-4), What is the pH of a 9.87 x 10-2 M aqueous solution of potassium nitrite, KNO2? Ka of HNO2 = 4.6 104. Determine the pH of each of the following solutions (Ka and Kb values are 3.0 * 10^-8 and 1.1 * 10^-8 Part A 9.00 * 10-2 M hypochlorous acid. {/eq} for {eq}HBrO What is Kb value for CN- at 25 degree C? Createyouraccount. And a, Q:Give the formula of the conjugate acid:(a) NH(b) NH(c) nicotine, CHN, A:The species which accepts a proton in the bronsted acid base theory. A student takes the full 1000.0 mL of the buffer prepared in part (a) and adds 1.00 g KOH. The Ka for hydrocyanic acid, HCN is 6.8 times 10^-10. c. HClO3(aq) + H2O (l) ClO3-(aq) + H3O+(aq) = Ka of HNO2 = 4.6 104 and Ka of HCN = 4.9 1010, What is the pH of a 0.145 M solution of (CH3)3N? Calculate the pH of a 4.0 M solution of hypobromous acid. Ka for HNO_2 is 5.0X 10^-4. [HBrO] = ([HBrO]initial x 1000 mL - 0.0178 mol) / 1000 mL [HBrO] = 4.982 x 10^-4 M. Calculate the acid dissociation constant K_a of 3-hydroxypropanoic acid. If the concentration of a HC2H3O2 solution is 0.1 M at a pH of 3.45, what is the value of Ka? Ka of HBrO is 2.3 x 10-9. Kb= Kw=. Round your answer to 2 significant digits. A:An acid can be defined as the substance that can donate hydrogen ion. What is the pH of a 6.00 M H3PO4 solution? What is the pH of the solution, the Ka, and pKa of HC2H3O2? Hypobromous acid (HBrO) is a weak 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? Acid with values less than one are considered weak. Trichloroacetic acid has a pK_a of 0.66 at 25 degrees C, determine the K_a of trichloroacetic acid, calculate K_b and pK_b of trichloroacetate. What is the Kb for the cyanide ion, CN? What is the pH of a 0.350 M HBrO solution? Q:What is the relationship between Ka of the acid and Kb of its conjugate base? Strength of Acids | Boundless Chemistry | | Course Hero (Ka = 1.0 x 10-10). a. Calculate the acid ionization constant (K_a) for the acid. After the reaction is in equilibrium, there is (0.0035 - x) M, x M, and x M of HBrO, H+, and BrO- respectively. %3D Study with Quizlet and memorize flashcards containing terms like What is the pH of a 0.150 M NH4Cl solution? The pH of your solution will be equal to 8.06. What is the pH of an aqueous solution with OH- = 0.775 M? The Ka of HCN at 25.0 degrees Celsius is 4.9 x 10-10. A 0.150 M weak acid solution has a pH of 4.31. a. The conjugate base obtained in a weak acid is always a weak base. (Ka = 2.5 x 10-9). What is the pH of a 0.199 M solution of HC_3H_5O_2? Ka of HCN = 4.9 1010 11.20 What is the pH of a 0.200 M KC7H5O2 solution? (Ka = 2.0 x 10-9). Calculate the Ka for this acid. Calculate the pH of a 0.315 M HClO solution. Science Chemistry 20.0 ml of 0.200M hypobromous acid, HBrO, is titrated with 0.250M sodium hydroxide, NaOH. Determine the acid ionization constant (K_a) for the acid. What is the pH of a 0.420 M hypobromous acid solution? 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. Given that Kb for CH3CH2NH2 is 6.3 10-4 at 25 C, what is the value of Ka for CH3CH2NH3 at 25 C? The Ka of HBrO is at 25 C. What is the pH of 0.25M aqueous solution of KBrO? Your question is solved by a Subject Matter Expert. The Ka for hypobromous acid, HBrO, is 2.0 x 10-9. An acid donates a hydrogen ion to form its conjugate base, A:Given :- chemical formula = HCO3- 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 = PH of the HBrO and NaBrO mixture - BrainMass What is the [OH^-] ion in an aqueous solution that has a pH of 11.70? 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. Salts of hypobromite are rarely isolated as solids. Conjugate acid of HCO, A:Proton (H+)donar is Bronsted acid. {/eq} for HBrO? Acid Ionization: reaction between a Brnsted-Lowry acid and water . What is the pH of an aqueous solution of 0.042 M NaCN? Kb of CH3NH2 = 4.4 104, What is the pH of a 0.200 M solution of HCOOH? Kb of NH3 = 1.76 105, What is the pH of a solution that has 0.300 M HNO2 and 0.300 M HCN? HCN -----> H+ + CN-, Q:A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. The percentage ionization of 0.150 M CH3CO2H (aq) is: (given Ka = 1.8 x 10-5 at 25 degree C) The pH of 0.150 M CH3CO2H (aq) is: (given Ka = 1.8 x 10-5 at 25 degree C), What is the hydronium-ion concentration of a 1.5 M solution of HCN (Ka = 4.9 \times 10^{-10}) at 25 degree C? Calculate the acid ionization constant (Ka) for the acid. Acid is a species which can donate a proton to another species, A:Acid is substance which release hydrogen ions and base is substance which release hydroxyl ions when, Q:For each conjugate acid-base pair, identify the first species as an acid or a base and the second, Q:Based on their compositions and structures and on conjugateacidbase relationships, select the, A:An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions, A:A conjugate base is that which is formed when a acid releases a H+ion in the solution A 0.159 M solution of a monoprotic acid has a percent ionization of 1.25%. a) 4.57 x 10-3 b) 2.19 x 10-12 c) 5.43 x 10-5 d) 7.81 x 10-6 e) 2.19 x 102. Calculate the pH of a 6.6 M solution of alloxanic acid. What is the pH of a 0.10 M solution of NaCN? 6.51 b. What is the value of Ka for the acid? Obtain the: Kb value for NO2- The Ka value for NH3OH+ (hydroxylammonium ion). (Ka = 2.9 x 10-8), What is the pH of a 0.95 M solution of HClO? 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^+ ??? Answer link So, the expected order is H3P O4 > H3P O3 > H3P O2. The value of Ka for HCOOH is 1.8 times 10-4. So, assume that the x has no effect on 0.240 -x in the denominator. Using this method, the estimated pKa value for bromous acid was 6.25. (Ka = 3.5 x 10-8). 5.90 b. Determine the pH of each of the following solutions (Ka and Kb values are 3.0 * 10^-8 and 1.1 * 10^-8 Part A 9.00 * 10-2 M hypochlorous acid.. What is the pH of a 0.530 M solution of HClO? A 0.115 M solution of a weak acid (HA) has a pH of 3.29. 2.83 c. 5.66 d. 5.20 e. 1.46. What is the pH and pK_a of the solution? The K_a for HClO is 2.9 times 10^{-8}. Solved Consider the reaction of 56.1 mL of 0.310 M NaCHO | Chegg.com 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. A:We have given that 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.) The ka of hypochlorous acid HClO is 3.5 \times 10^{-8}. Kb of NH3 = 1.76 105, What is the pH of a 0.225 M (CH3)2NH2Br solution? The K_a for formic acid (HCO_2H) is 1.8 .10^{-4}. 7.54. b. What is the Ka of this acid? (Ka for HF = 7.2 x 10^-4). Hypobromous acid has a pKa of 8.65 and is therefore only partially dissociated in water at pH7. An aqueous solution has a pH of 4. What is the pH of an aqueous solution with H+ = 8.3 x 10-7 M? The Ka for benzoic acid is 6.3 * 10^-5. @ The Ka for hypobromous acid, HOBr is 2.5 x 10^{-9}. What is the pH of a 0.25 M HBrO(aq) H B r O ( a q) solution? Ka of HNO2 = 4.6 104 and Ka of HCN = 4.9 1010, What is the pH of a 0.300 M solution of CH3NH2? (Ka = 3.5 x 10-8). What is Kb for the conjugate base of HBRO (Ka = 2.5 10)? What is the pH of a 0.546 M hypochlorous acid, HOCl, solution? Kb of (CH3)3N = 6.4 105, What is the pH of a 0.110 M solution of HBrO? What is the pH of a 0.350 M HBrO solution? The pH of a 0.94 M solution of 3-hydroxypropanoic acid (HC_3H_5O_3) is measured to be 2.27. What is the pH of an aqueous solution at 25 deg C in which H+ is 0.0025 M? HBrO, Ka = 2.3 times 10^{-9}. The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. HBrO is a weak acid according to the following equation. With an increasing number of OH groups on the central P-atom, the acidic strength . See Answer (Ka = 3.0 x 10-8), What is the pH of 0.015 M aqueous benzoic acid? $6 \%$ of $\underline{\qquad}$ is $0.03$. The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25 C is 4.48. In comparison to other oxygen-centered oxidants (hypohalites, anions of peroxides) and in line with its low basicity, bromite is a rather weak nucleophile. k a for hypobromous acid, hbro, is 2.0 10-9. karlibghs5921 karlibghs5921 07/30/2018 Chemistry College answered expert verified . Calculate the H3O+ in a 1.7 M solution of hypobromous acid. The K_a of 0.1M acetic acid is 1.8 \times 10^{-5}. Calculate the pH of the resulting solution at 25 C. Molarity of NaC H O = 3.00 g Before there were radios and satellite communication systems, ships would communicate with each other by using a string of colored flags. The pH of 0.255 M HCN is 4.95. (b) Give, Q:Identify the conjugate base The pH of a 0.051 M weak monoprotic acid solution is 3.33. What is the value of the ionization constant, Ka, for the acid? The Ka of HCHO2 is 1.8\times10-4 at 25 C. What is the pH of a 0.200 M solution for HBrO? Except where otherwise noted, data are given for materials in their, Egon Wiberg, Arnold Frederick Holleman (2001), "Journal of the Society of Chemical Industry. Get access to this video and our entire Q&A library, What is Salt Hydrolysis? The equilibrium expression of this ionization is called an ionization constant. Janel S. asked 10/14/19 What is the buffer component ratio, (BrO-)/(HBrO) of a bromate buffer that has a pH of 9. What is the pH of a neutral solution at the same Calculate the H3O+ and OH- concentrations in this solution. Other relevant reactions in such oscillating reactions are: Bromites reduce permanganates to manganates (VI):[1]. (The Ka of HOCl = 3.0 x 10-8. Q:What is Kb for the conjugate base of CH3COOH (Ka = 1.8 x 10)? a. What is [OH]? ( pKa p K a = 8.69) a. All rights reserved. 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. Given that Ka for HBrO is 2.8 times 10^ (-9) at 25 degree C, what is The K_{a} for HC_{2}H_{3}O_{2} is 1.8\times 10^{-5}. Kw = ka . What is the pH of a 0.35 M aqueous solution of sodium formate? How do I calculate the pH of a 0.093 M NaF solution, where the Ka for HF = 7.1 x 10^-4? 3 days ago. Calculate the pH of a 0.25 M solution of F- at 25 degrees Celsius. What is the pH of an aqueous solution of 4.69 x 10^-2 M hydrobromic acid? Determine the [KBrO] if the [HBrO] is 0.625 M. AI Recommended Answer: To calculate the [KBrO], we need to know the Ka of HBrO and the pH of the solution. d. CH3NH3+(aq) + H2O (l) CH3NH2(aq) + H3O+(aq) = Like the acid, hypobromite salts are unstable and undergo a slow disproportionation reaction to yield the respective bromate and bromide salts. What is the pH of a 0.20 m aqueous solution? Was the final answer of the question wrong? A 9.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.58%. The Ka for HBrO = 2.8 x 10^{-9}. Calculate the pH of a 0.86 M, A:Equilibrium constant is the ratio of product of concentration of products raised to their, A:Conjugate base is the chemical species which is formed when acid donates a proton to another, Q:Construct the expression for Ka for the weak acid, CH,COOH. Bromic acid | HBrO3 - PubChem solution of formic acid (HCOOH, Ka = 1.8x10 What is the, Q:The value pKw is 11.05 at 78 C. Step 1: To write the reaction equation. Round your answer to 2 significant digits. Calculate the pH of an aqueous solution of 0.15 M NaCN. 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. The Ka for formic acid is 1.8 x 10-4. OneClass: ka of hbro The pH of a 0.15 M solution of a weak monoprotic acid, HA, is 3.62. The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25 Hypobromous acid is a weak, unstable acid with chemical formula of HOBr. What is the acidic strength order of H3PO2, H3PO3, H3PO4 ? Why? - Byju's Perbromic acid | HBrO4 or BrHO4 | CID 192513 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities . Find the value of pH for the acid. Q:What is the conjugate base of C4H5O3? (Ka = 2.8 x 10-8), What is the hydronium ion concentration in a 0.410 M OCl- solution? The Ka for the acid is 3.5 x 10-8. 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.) Discussion section worksheet 09 - Properties of acid-base buffer a Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with. HBrThe formula for hydrobromic acid is HBr, but in the absence of water this compound should properly be called hydrogen bromide rather than hydrobromic acid. A 0.110 M solution of a weak acid has a pH of 2.84. Given that Kb for CH_3NH_2 is 5.0 10-4 at 25^o C, what is the value of Ka for CH3NH3 at 25^o C? Answer to Ka of HBrO, is 2X10-9. KaKb=Kw Kw=1.010-14 So, Kb=1.010-14Ka Q: Calculate the pH of a 0.0158 M aqueous solution of formic acid (HCOOH, Ka = 1.8x10 4). (Ka = 2.9 x 10-8). What is the OH- in an aqueous solution with a pH of 8.5? What is the pH of a 0.100 M aqueous solution of NH3? F5 Salt hydrolysis is the reaction of a salt with water. What is the expression for Ka of hydrobromic acid? - Answers Ka of HCN = 4.9 1010, What is the pH of a 0.200 M KC7H5O2 solution? The acid HOBr has a Ka = 2.5\times10-9. Calculate the pH of a 0.00323 M solution of NaF, give that the Ka of HF = 6.80 x 10-4 at 25 degrees C. Part A Given that at 25.0 C 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+. The research measured the rate of bromite decomposition as a function of hydrogen and bromite ion concentrations. 8.3. c. 9.0. d. 9.3. What is the pH of an aqueous solution with H+ = 7.8 x 10-9 M? What is the pH of a 0.0137 M solution of HClO with ka = 3.0*10^-8? What is its Ka? The value of acid dissociation constant measured by this method is Ka = (3.70.9)104M and pKa = 3.430.05.[9]. Weekly leaderboard Home Homework Help3,800,000 These three species exist in a chemical equilibrium and they are interrelated by a known acid dissociation constant {eq}K_a {/eq}. What is its Ka value? Find answers to questions asked by students like you. The Ka of hypochlorous acid (HClO) is 3.00 x 10-8 at 25.0 degrees C. Calculate the pH of a 0.0385 M hypochlorous acid solution. First week only $4.99! The add dissociation constant K_a of carbonic acid (H_2CO_3) s 4.5 * 10^-7. Find the pH of a 0.0075 M aqueous solution of hypochlorous acid (HClO), for which Ka = 3.5 x 10-8. What is are the functions of diverse organisms? What is the pH of an aqueous solution with [H3O+] = 4 * 10-13 M ? Given that Ka for HCOOH is 1.8 * 10-4 at 25 degree C, what is the value of Kb for COOH- at 25degree C? The larger Ka. What is the base dissociation constant, Kb, for the gallate ion? What is the ph of a solution that is 0.25 M KNO2 and 0.35 M HNO2(nitrous acid)? Concentration of NH4Cl = 0.140 M. Q:Use the Kb for the nitrite ion, NO2, to calculate the Ka for its conjugate acid. What is the expression for Ka of hydrobromic acid? Calculate the H3O+ in a 1.4 M solution of hypobromous acid. The Ka of HC7H5O2 is 6.5 x 10-5. 8.14 (You can calculate the pH using given information in the problem. What is the pH of a buffer solution that is 1.00 M in HCN and 0.100 M in KCN? 18)A 0.15 M aqueous solution of the weak acid HA . Calculate the pH and molar concentrations of H2A, HA , and A2 at equilibrium for each of the solutions below (a) a 0.136 M solution of NaHA (b) a 0. HPO, (aq) + H20(1) = H;O*(aq) + PO, (aq), Q:1. Become a Study.com member to unlock this answer! Round your answer to 1 decimal place. Hydrobromic is stronger, with a pKa of -9 compared to You must use the proper subscripts, superscripts, and charges. With 0.0051 moles of C?H?O?? What is the pH of 0.070 M dimethylamine? A solution of formic acid 0.20 M has a pH of 5.0. Q:. 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. Get access to this video and our entire Q&A library, Acid-Base Equilibrium: Calculating the Ka or Kb of a Solution. % SOLVED: If the Ka of HBrO is 2.01 x 10-9, and the pH of a solution made The species which can, Q:What is the pH of a 0.21 M solution of methylamine, A:Given :- It is generated both biologically and commercially as a disinfectant. What is the value of Ka for the acid? The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2, is 5.0 x 10^-2. Learn about salt hydrolysis. Upon treatment of these aqueous solutions with salts of Pb2+, Hg2+, and Ag+, the corresponding heavy metal bromites precipitate as solids. Find Ka for the acid. Assume that the Ka 72 * 10^-4 at 25 degree C. The pH of a 0.175 M aqueous solution of a weak acid is 3.52. A 0.081 M solution of a monoprotic acid has a percent ionization of 2.34%. The Ka for HBrO is 2.3 x 10-9. b. In a 0.600 M aqueous solution of a monoprotic acid, 4.46 % of the acid is ionized. esc But the strong acid is not like that, they dissociate completely into its ions when it is added with water. HZ is a weak acid. Understand what a conjugate is, how it is formed, how to identify conjugate acid, and see examples of conjugate acids with their pairs. moles HBrO present = 20.0 ml x 1 L / 1000 ml x 0.300 mol/L = 0.006 moles HBrO. What is the pH of an aqueous solution of 0.345 M hypochlorous acid? what is the ka value for Pka 3.0, 8.60, -2.0? pH = ____ What is the hydroxide ion concentration, [OH^-], in an aqueous solution with a hydrogen ion con. The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10{eq}^{-9}. 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 What is the Ka value of the conjugate acid of a base with a Kb value of 8.2 x 10^-7? Learn the definition of weak acids, study common examples, discover the difference between strong and weak acids, and understand how to write weak acid equilibrium equations. %3D A: Given data,Molarity of HCN=0.0620MKa=4.910-10 question_answer question_answer :. for HBrO = 2.5x10 -9) HBrO + H 2 O H . What is K_a for this acid? Calculate the pH of the following aqueous solution: 0.34 M C6H5NH3NO3. What is Ka for C5H5NH+? For a certain acid pK_a = 5.40. Get access to this video and our entire Q&A library. K_a for hypobromous acid, HBrO, is 2 \times 10^{-9}. K_a = 2.8 times 10^{-9}. , 35 Br ; . Ka of acetic acid = 1.8 x 10-5 Determine the pH of a 0.045 M hypobromous acid (HBrO) solution. Createyouraccount. The Ka of HCN is 4.9 x 10-10. Calculate the acid ionization constant (K_a) for the acid. (Ka = 4.9 x 10-10), Calculate the K_a of a weak acid if a 0.029 M solution of the acid has a pH of 2.97 at 25^o C. K_a = \boxed{\space} \times 10^ \boxed{\space} ( Enter your answer in scientific notation.). What is the value of Ka for HBrO? HBrO, Ka = 2.3 times 10^{-9}. The acid dissociation K_a of benzoic acid (C_6H_5CO_2H) is 6.3 \times 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.