ka of hbro ka of hbro

This begins with dissociation of the salt into solvated ions. HZ is a weak acid. (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? An 8.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.63%. What is the pH of an aqueous solution of 0.042 M NaCN? What is the pH of the buffer after the addition of the KOH (assuming the addition of KOH does not affect the volume)? c. HClO3(aq) + H2O (l) ClO3-(aq) + H3O+(aq) = Round your answer to 2 significant digits. temperature? Kb of base = 1.27 X 10-5 calculate its Ka value? Calculate the pH of a 0.12 M HBrO solution. What is the pH of a 0.0137 M solution of HClO with ka = 3.0*10^-8? HBrO2 is the stronger acid. Calculate the Ka of the acid. What is the pH of a 0.420 M hypobromous acid solution? This begins with dissociation of the salt into solvated ions. Vip Thumbnail | 2 Thumbnail ,android phone se youtube thumbnail kaise banaye,how to make thumbnail for . The k_b for dimethylamine is 5.9 times 10^{-4}. Determine the acid ionization constant (Ka) for the acid. Our experts can answer your tough homework and study questions. What is the pH of a 0.200 M solution for HBrO? Spell out the full name of the compound. The value of acid dissociation constant measured by this method is Ka = (3.70.9)104M and pKa = 3.430.05.[9]. Its Ka is 0.00018. A:The relation between dissociation constant for acid, base and water is given as follows, The K_a for HClO is 2.9 times 10^{-8}. 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? Become a Study.com member to unlock this answer! The add dissociation constant K_a of carbonic acid (H_2CO_3) s 4.5 * 10^-7. (Ka = 1.8 x 10-5). Determine the pH of a 0.045 M hypobromous acid (HBrO) solution. With 0.0051 moles of C?H?O?? Kb BrO- = Kw / Ka HBrO = (1 x 10^-14) / (2.0 x 10^-9) = 5.0 x 10^-6 . Our experts can answer your tough homework and study questions. The pH of an aqueous 0.50 M hypochlorous acid solution is 3.88. What is the base dissociation constant, Kb, for the gallate ion? What is Ka for C5H5NH+? HBrO H + BrO Given the pH is 4.48, the concentration of H is: Given the initial concentration of the acid ( Ca) is 0.55 M, we can calculate the acid dissociation constant ( Ka) using the following expression. This is confirmed by their Ka values . Adipic acid has a pKa of 4.40. Express your answer using two significant figures. Calculating pKa Calculate the Ka for a 0.505 M solution of a monoprotic acid that has a pH of 3.36. What is the pH of an aqueous solution of 0.042 M NaCN? Since the moles are the same, this tells us that ALL of the KOH was converted to KBrO. The pH of a 0.200M HBrO solution is 4.67. Then Determine 25.0 ml of 0.600M hypobromous acid, HBrO, is titrated with 0.400M sodium hydroxide, NaOH. Was the final answer of the question wrong? What is the pH of a 0.11 M solution of the acid? - Definition & Examples. (Ka = 2.5 x 10-9). Determine the pH of a 0.045 M hypobromous acid (HBrO) solution. 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 K_b and a (degree of ionization) of NH_3 (aq) for the following pH and concentrations? W F4 Calculate (KF) in a buffer where (HF) = 0.14 M and pH = 3.90. E) 1.0 times 10^{-7}. The value of Ka for HBrO is 1.99 10. Q:what is the conjugate base and conjugate acid products with formal charges? Between 4 and 5 C. Approximately = 7 D. Between 8 and 9 E. Between 9 and 10 Justify your answer with a calculation All rights reserved. The Ka of HCHO2 is 1.8\times10-4 at 25 C. What is the pH of a 0.200 M solution for HBrO? 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). An organic acid has pKa = 2.87. Q:. 8.3. c. 9.0. d. 9.3. 7.1 10 4 b. Ka = [H+]. ), Find the pH of a 0.0176 M solution of hypochlorous acid. Calculate the acid ionization constant (Ka) for the acid. HClO, Ka = 3.0 108 HBrO, Ka = 2.0 109 Of these, the only ones that are conceptually reasonable to explain are HClO vs. HBrO. A. 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+. What is the pH of a 0.350 M HBrO solution? 3 A 0.145 M solution of a weak acid has a pH of 2.75. The chemical formula of hydrobromic acis is HBr. Calculate the pH of a 1.45 M KBrO solution. Determine the acid ionization constant (K_a) for the acid. Calculate the pH of a 0.111 M solution of H2A. What is Ka for this acid? (Ka = 3.5 x 10-8). K, =, Q:For each pair of molecules or ions, select the stronger base and write its Lewis structure. The Ka for hypochlorous acid, HOCl, is 3.5 x 10-8. Given that Kb for C6H5NH2 is 1.7 * 10-9 at 25 degree C, what is the value of Ka for C6H5NH3 at 25 degree C? The pH of 0.042 M Hypobromous acid (HOBr) is 5.07. Calculate the pH and fractional dissociation of 0.83M of the weak base methylamine assuming that its Ka = 2.27 x 10^-11. CN- + H2O <---> HCN + OH- Bronsted Lowry Base In Inorganic Chemistry. (Ka = 3.5 x 10-8). What is the hydronium ion concentration of a 1.5 M solution of HCN (Ka = 4.9 x 10^-10) at 25 degrees Celsius? What is Kb for the conjugate base of CHCOOH (Ka = 1.8 10)? Given that Kb for (CH3)2NH is 5.4\times0-4 at 25C, what is the value of Ka for (CH3)2NH2 at 25 C? What is the value of Ka for HClO, given that a 0.10 M solution has a pH of 4.27? (Ka = 2.9 x 10-8). The dissociation constant of hypobromous acid (HBrO) is {eq}K_a\ =\ 2.3\times 10^{-9}\ \rm M{/eq}. Q:Kafor ammonium, its conjugate acid. (Ka = 2.0 x 10-9). Using the answer above, what is the pH, A:Given: What is the pH of a 0.200 M H2S solution? What is are the functions of diverse organisms? Find the pH of. What is the acid dissociation constant (Ka) for the acid? Consider the reaction of 59.5 mL of 0.310M NaC7H5O2 with 50.0 mL of 0.245MHBr. The pH of 0.042 M Hypobromous acid (HOBr) is 5.07. Createyouraccount. Your question is solved by a Subject Matter Expert. A:The given anion C4H5O3 is also basically a conjugated base generated from C4H6O3 on deprotonation. Part A What is the [H_3O^+] of 0.146 M HNO? How do I calculate the pH of a 0.093 M NaF solution, where the Ka for HF = 7.1 x 10^-4? What is the pH of an aqueous solution of 0.523 M hypochlorous acid? 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.) Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. pyridine Kb=1.710 (Ka = 1.8 x 10-4), What is the pH of a 0.530 M solution of hypochlorous acid? Calculate the H3O+ and OH- concentrations in this solution. %3D, A:HCN is a weak acid. Hypobromous acid is a weak, unstable acid with chemical formula of HOBr. A) 1.5 times 10^-11 B) 1.5 times 10^-5 C) 1.5 times 10^9 D) 6.8 times 10^10 E) 6.8 times 10^-24. Is this solution acidic, basic, or neutral? one year ago, Posted esc and ? Weak Acid: The dissociation of a weak Bronsted acid species in aqueous. [CH3CO2][CH3COOH]=110 What is the value of Kb? (Ka = 2.5 x 10-9). A:An acid can be defined as the substance that can donate hydrogen ion. See Answer (Ka of C5H6CO2H = 6.3 x 10-5), What is the pH of 0.035 M aqueous benzoic acid? Createyouraccount. Calculate the value of ka for this acid. Calculate the pH of a 4.0 M solution of hypobromous acid. 3 months ago, Posted hydroxylamine Kb=9x10 All ionic compounds when dissolved into water break into different types of ions. The Ka of HBrO is at 25 C. What is the pH of 0.25M aqueous solution of KBrO? This video shows how you can calculate the Ka of an acid, if you're given the pH of the solution (and its concentration, of course). What is its Ka value? A weak acid can be defined as the acid which dissociates partially into its ions when it is added with water. Calculate the concentration of OH- and the pH value of an aqueous solution in which (H3O+) is 0.014 M at 25 degrees Celcius. All rights reserved. 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 0.010 M solution of iodic acid (HIO3, Ka = 0.17). (Ka for HF = 7.2 x 10^{-4}) . A 0.159 M solution of a monoprotic acid has a percent ionization of 1.25%. Calculate the acid ionization constant (Ka) for the acid. The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. 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? What is the value of it's K_a? pH =? The pH of a 0.051 M weak monoprotic acid solution is 3.33. Given a diprotic acid, H_2A, with two ionization constants of K_a1 = 2.1 * 10^-4 and K_a2 = 3.1 * 10^-12, calculate the pH FOR A 0.182 M solution of NaHA. But the actual order is : H3P O2 > H3P O3 > H3P O4. The pH of a 0.250 M cyanuric acid solution is 3.690. The pH of a 0.21 M solution of a weak monoprotic acid, HA, is 2.92. What is the pH of a 0.113 M aqueous solution of sodium benzoate, NaC6H5COO? What is the pH of an aqueous solution with OH- = 0.775 M? A certain organic acid has a K_a of 5.81 times 10^{-5}. The Ka for formic acid is 1.8 x 10-4. The species which can, Q:What is the pH of a 0.21 M solution of methylamine, A:Given :- Kb of (CH3)3N = 6.4 105, What is the pH of a 0.110 M solution of HBrO? H2CO/ HCO Round your answer to 1 decimal place. What is the value of Ka for the acid? 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. Calculate the pH of a 0.43M solution of hypobromous acid. What is the ph of a solution that is 0.25 M KNO2 and 0.35 M HNO2(nitrous acid)? The Ka of hydrofluoric acid (HF) at 25 degree C is 6.8 x 10^-4. 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. moles HBrO present = 20.0 ml x 1 L / 1000 ml x 0.300 mol/L = 0.006 moles HBrO. After the reaction is in equilibrium, there is (0.0035 - x) M, x M, and x M of HBrO, H+, and BrO- respectively. Round your answer to 2 significant digits. Calculate the pH of a 1.60 M KBrO solution. Acid with values less than one are considered weak. What is the value of Ka for the acid? What is the pH of an aqueous solution with H+ = 8.3 x 10-7 M? Kw = ka . 7.52 c. -1.41 d. 4.47 e. 8.94. Ka of HBrO = 2.8 109, What is the pH of a 0.250 M solution of HCN? Calculate the H+ in an aqueous solution with pH = 11.93. Plug the values into Henderson-Hasselbalch equation. Were the solution steps not detailed enough? copyright 2003-2023 Homework.Study.com. What is its Ka value? HPO24+HBrO acid+base Acid: Base: chemistry. The pH of a 0.79 M solution of butanoic acid (HC4H7O2) is measured to be 2.46. What is the value of k_b for the hydrolysis reaction: A^- + H_2O to HA + OH^-. In an aqueous solution, the (OH^-) is 1.0 times 10^{-5} M. What is the pH? Ka for HNO_2 is 5.0X 10^-4. What is the pH of an aqueous buffer solution prepared from 0.95 M NH_3 and 1.22 M NH_4Cl? Sodium fluoride, NaF, is a soluble salt that dissociates completely in aqueous solution to give sodium cations, Na+, and fluoride anions, F. The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10^-9 . Calculate the acid ionization constant (Ka) for the acid. what is the ka value for Pka 3.0, 8.60, -2.0? What is the pH of a 0.035 M solution of benzoic acid (Ka = 6.3 x 10-5) at 25 degrees Celsius? what is the value of Kb for C_2H_3O_2-? What is the H+ in an aqueous solution with a pH of 8.5? What is the pH of a 6.00 M H3PO4 solution? 4 Calculate the concentration of OH- and the pH value of an aqueous solution in which (H3O+) is 0.014 M at 25 degrees C. Is this solution acidic, basic, or neutral? (Ka = 2.5 x 10-9). (Ka = 3.5 x 10-8). Ka of HCN = 4.9 1010. Ka of HC7H5O2 = 6.5 105, What is the pH of a 0.375 M solution of HF? A 0.120 M solution of a weak acid (HA) has a pH of 3.33. 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.. pH= pKa+log [base] [acid] pH=log (2.510^ (9))+ log (0.1200.350)=8.14) x = 38 g 1 mol. Calculate the acid ionization constant (K_a) for the acid. To know more check the Conjugate acid of HCO, A:Proton (H+)donar is Bronsted acid. What is the pH of a 0.55 M aqueous solution of HBrO at 25 degree C? HCO, + HPO,2 H2CO3 What is the pH of a neutral solution at the same 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 = In direct contrast with HCl vs. HBr, HClO is a stronger acid than HBrO, because Cl is more electronegative, which dominates over the size difference between Cl and Br due to the presence of the oxygen. Calculate the pH of the solution. To summarize: Ka * Kb is equivalent to adding the acid and base reactions together, which results in a net equation of the autoionization of water. (remember,, Q:Calculate the pH of a 0.0158 M aqueous 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+. Janel S. asked 10/14/19 What is the buffer component ratio, (BrO-)/(HBrO) of a bromate buffer that has a pH of 9. The equilibrium expression of this ionization is called an ionization constant. (Ka = 1.8 x 10-4), What is the pH of a 9.87 x 10-2 M aqueous solution of potassium nitrite, KNO2? a. What is the value of Ka for the acid? Calculate the pK_a of an acid if its K_a is 2.3 \times 10^{-3}. b) What is the Ka of an acid whose pKa = 13. Given that Ka for HF is 6.3 x 10-4 at 25^o C, what is the value of Kb for F- at 25^o C? Perbromic acid | HBrO4 or BrHO4 | CID 192513 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities . Upon treatment of these aqueous solutions with salts of Pb2+, Hg2+, and Ag+, the corresponding heavy metal bromites precipitate as solids. 2.2 10-5 What is the pH of a 0.135 M NaCN solution? If the Ka of HBrO is 2.01 x 10-9, and the pH of a solution made from an HBrO and KBrO solution is 8.98. Find the pH of an aqueous solution of 0.081 M NaCN. B. It is mainly produced and handled in an aqueous solution. x / 0.800 = 5 10 x = 2 10 For propanoic acid (HC3H2O2; Ka = 1.3 x 10-5), determine the pH and percent dissociation of a 0.100 M solution. Acetylsalicylic acid (aspirin, HC 9 H 7 O 4) is a weak acid with Ka = 2.75x10 -5 at 25 C. 3.00 g of sodium acetylsalicylate (NaC 9 H 7 O 4) is added to 200.0 mL of 0.100 M solution of this acid. What is [OH]? Ka of HBrO is 2.3 x 10-9. Become a Study.com member to unlock this answer! 2x + 3 = 3x - 2. A) 1.0 times 10^{-8}. solution of formic acid (HCOOH, Ka = 1.8x10 Journal of inorganic biochemistry, 146, 61-68. (Ka = 2.0 x 10-9), Calculate the pH of a 1.4 M solution of hypobromous acid. 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. (K_b for C_2H_5NH_2 = 4.7 times 10^{-4} at 25 degree Celsius). The Ka of HCN is 6.2 x 10-10. What is the pH of a 0.135 M NaCN solution? HCN -----> H+ + CN-, Q:A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. e. H2C2O4(aq) + H2O (l) HC2O4-(aq) + H3O+(aq) =. The Ka for hypobromous acid, HOBr is 2.5 x 10^{-9}. Chemistry questions and answers. What is Kb for the conjugate base of HCN (Ka = 4.9 10)? You must use the proper subscripts, superscripts, and charges. (Ka = 3.5 x 10-8). a. Calculate the pH of a 0.400 mol cdot L^{-1} KBrO solution. 1- Draw structure of the acid and its conjugate base, use any available resource, and assign Ka for the acid. (Ka = 2.0 x 10-9), Calculate the H3O+ in a 1.7 M solution of hypobromous acid. A concentration of 0.020M in aqueous solution gives a pH of 4.93 what is the Ka? 0.25 M KI Express your answer to two. 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^+ ??? (a) Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. What is the pH of a 0.530 M solution of HClO? Kb of NH3 = 1.76 105, What is the pH of a 0.150 M solution of CH3COOH? Dissociation Constants at 25 degree C 0.25 M CH_3NH_3I Express your answer to two decimal places. Express your answer using two significant figures. Ka of HF = 3.5 104, What is the pH of a solution that has 0.300 M HNO2 and 0.300 M HCN? Hypobromous acid (HBrO) is a weak acid. Who is Katy mixon body double eastbound and down season 1 finale? Conjugate acid is that, Q:The base protonation constnt K, of morpholine (C,H,ONH) is 2.14 x 10 . The acid dissociation constant of HCN is 6.2 x 10-10. An acid donates a hydrogen ion to form its conjugate base, A:Given :- chemical formula = HCO3- A 0.115 M solution of a weak acid (HA) has a pH of 3.29. K, = 6.2 x 10 What is the value of K_a for HBrO? What is the pH of a 0.420 M hypobromous acid solution? Then substitute the K a to solve for x. Find the value of pH for the acid. The concentration of an aqueous solution of HCN is 0.05 M. Calculate the pH of the solution. Solve a) The Ka of formic acid (HCO_2H) is 1.77 \times 10^{-4}. The Ka of HBrO is at 25 C. The K_a of hydrazoic acid (HN_3) is 1.9 x 10^{-5} at 25.0^{o} C. What is the pH of a 0.15 M aqueous solution of HN_3? Ximenes, V. F., Morgon, N. H., & de Souza, A. R. (2015). What is the pH of 0.264 M NaF(aq)? Hypobromous acid is a weak acid (Ka = 2.8 * 10-9 M). The acid dissociation constant Ka of hypobromous Step1 Degree of dissociation = sqrt [Ka/C] = sqrt [ 2.3x10^-9/.43]=7.314x10^-5 Step2 [H Posted The K_a of hydrazoic acid (HN_3) is 1.9 times 10^{-5} at 25 degree C. What is the pH of a 0.35 M aqueous solution of HN_3? Start your trial now! Determine the value of Ka for this acid. (Ka = 2.8 x 10-9). What is the pH of a 0.199 M solution of HC_3H_5O_2? HBrO2 has Ka = 1.2 105, while HBrO has Ka = 2 109. Calculate the pH of a 4.5 M solution of carbonic acid. What is the pH of a 0.84 M solution of NaCN (Ka of HCN=6.2X10-10)? The value of Ka for HCOOH is 1.8 times 10-4. If the concentration of a HC2H3O2 solution is 0.1 M at a pH of 3.45, what is the value of Ka? What is the, Q:The value pKw is 11.05 at 78 C. The acid dissociation K_a of benzoic acid (C_6H_5CO_2H) is 6.3 \times 10^{-5}. a. %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)? Round your answer to 2 significant digits. (e.g. Hydrobromic is stronger, with a pKa of -9 compared to What is the pH of a 0.2 M KCN solution? Determine the pH of a 0.98 x 10^(-2) mol L solution of hydrocyanic acid (HCN) Ka = 4.0 x 10^(-10). Which works by the nature of how equilibrium expressions and . A. The strength of an acid refers to the ease with which the acid loses a proton. 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? Calculate the pH of a 0.719 M hypobromous acid solution. What is the pH of an aqueous solution with H+ = 2.0 x 10-9 M? hydrochloric acid's -8. Calculate the present dissociation for this acid. What is the pH of 0.35 M solution of sodium formate (NaHCOO)? (Hint: The H_3O^+ due to the water ionization is not negligible here.). A 0.200 M solution of a weak acid has a pH of 2.50. 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.