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What is the pH of a 0.84 M solution of NaCN (Ka of HCN=6.2X10-10)? What is the, Q:The value pKw is 11.05 at 78 C. The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10^{-9}. Get access to this video and our entire Q&A library, Acid-Base Equilibrium: Calculating the Ka or Kb of a Solution. (NH4+) = 5.68 x 10^-10 A 0.148M solution of a monoprotic acid has a percent dissociation of 1.55%. What is the pH of a 0.2 M KCN solution? Calculate the acid ionization constant (Ka) for this acid. KOH + HBrO KBrO + HO This salt, when dissolved in HO, produces an alkaline solution. A 0.110 M solution of a weak acid has a pH of 2.84. Median response time is 34 minutes for paid subscribers and may be longer for promotional offers. Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO. :. (Ka = 3.50 x 10-8). A 0.159 M solution of a monoprotic acid has a percent ionization of 1.25%. Become a Study.com member to unlock this answer! Kb of (CH3)3N = 6.4 105, What is the pH of a 0.110 M solution of HBrO? Calculate the pH of a 1.45 M KBrO solution. Type it in sub & super do not work (e. g. H2O) What is the value of K_{b} for C_{2}H_{3}O_{2}^-. What is the pH of 0.25M aqueous solution of KBrO? Enter the Kb value for CN- followed by the Ka value for NH4+, separated by a comma, usi. Spell out the full name of the compound. What is the pH of an aqueous solution that is 0.20 M HNO_2 (Ka = 4.3 x 10^(-4)) and 0.20 M NaNO_2? The Kb for NH3 is 1.8 x 10-5. K_a for hypobromous acid, HBrO, is 2.0 times 10^{-9}. Kb of NH3 = 1.76 105, What is the pH of a 0.150 M solution of CH3COOH? (Ka = 2.9 x 10-8), What is the pH of a 0.95 M solution of HClO? A 0.145 M solution of a weak acid has a pH of 2.75. Get access to this video and our entire Q&A library. Ka of HC7H5O2 = 6.5 105 Calculate the acid ionization constant (Ka) for the acid. What is delta G at 25 degree C for a solution in which the initial concentrations are: [CH3CO2H]0 = 0.10 M [H+]0 = 4.5 * 10-8 M. Determine the dissociation constant K_a for pK_a=2.0. copyright 2003-2023 Homework.Study.com. What is the conjugate base of HSO4 (aq)? Calculate the pH of a 1.4 M solution of hypobromous acid. Each compound has a characteristic ionization constant. 80 c. HClO3(aq) + H2O (l) ClO3-(aq) + H3O+(aq) = For example, the general equation for the ionization of a weak acid in water, where HA is the parent acid and A is its conjugate base, is as follows: HA ( aq) + H2O ( l) H3O + ( aq) + A ( aq) The . 2 . What is Kb for the conjugate base of HBRO (Ka = 2.5 x 10)? 3. What is the pH of an aqueous solution at 25 degrees C in which (H+) is 0.025 M? HBrO, Ka = 2.3 times 10^{-9}. What is the pH of an aqueous solution with H+ = 2.0 x 10-9 M? In an aqueous solution of a certain acid the acid is 0.079% dissociated and the pH is 4.59. 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. (Ka for CH3COOH = 1.8 x 10-5). The K_a of HCN is 4.9 times 10^{-10}. Hypobromous acid has a pKa of 8.65 and is therefore only partially dissociated in water at pH7. The conjugate base obtained in a weak acid is always a weak base. The larger Ka. Vip Thumbnail | 2 Thumbnail ,android phone se youtube thumbnail kaise banaye,how to make thumbnail for . Ionic equilibri. Ka of HBrO is 2.3 x 10-9. pH =. The pH of a 0.25 M weak monoprotic acid (HA) solution is 3.50. The Ka of HCOOH is 1.8 10-4 and the Ka of HBrO is 2.8 10-9. With an increasing number of OH groups on the central P-atom, the acidic strength . Calculate the value of ka for this acid. What is the value of Ka for the acid? So, assume that the x has no effect on 0.240 -x in the denominator. of the conjugate base of boric acid. Nov 18 2022 08:12 AM 1 Approved Answer Mark B answered on November 20, 2022 4 Ratings ( 9 Votes) (Ka = 1.8 x 10-4), What is the pH of a 0.530 M solution of hypochlorous acid? The pH of a 1.3 M solution of carbonic acid (H_{2}CO_{3} is measured to be3.12. A 0.120 M weak acid solution has a pH of 3.75. A 9.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.58%. The pH of a 0.051 M weak monoprotic acid solution is 3.33. We store cookies data for a seamless user experience. Become a Study.com member to unlock this answer! Ka of HCOOH = 1.8 104, What is the pH of a 0.350 M MgF2 solution? If the concentration of a HC2H3O2 solution is 0.1 M at a pH of 3.45, what is the value of Ka? Given that Kb for CH3CH2NH2 is 6.3 10-4 at 25 C, what is the value of Ka for CH3CH2NH3 at 25 C? ), A 0.115 M solution of a weak acid (HA) has a pH of 3.30. What is the pH of an aqueous solution with H3O+ = 9.2 x 10-2 M? The Ka of HBrO is at 25 C. What is the pH of 0.25M aqueous solution of KBrO? Set up the equilibrium equation for the dissociation of HOBr. 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? (Ka = 2.5 x 10-9). What is the value of Ka for HBrO? Calculate the OH- in an aqueous solution with pH = 3.494. b. HPO42-(aq) + H2O (l) PO43-(aq) + H3O+(aq) = Calculate the pH of a 0.50 M NaOCN solution. But the actual order is : H3P O2 > H3P O3 > H3P O4. An aqueous solution has a pH of 4. : a. HSO3-(aq) + H2O (l) SO32-(aq) + H3O+(aq) = 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? Write the base dissociation reaction (equilibrium) for benzoate ion (C,H$CO2) in water; B) 1.0 times 10^{-4}. Round your answer to 2 significant digits. Round your answer to 1 decimal place. Learn about salt hydrolysis. To find a concentration of H ions, you have to. Let's assume that it's equal to 0.1 mol/L. So, the expected order is H3P O4 > H3P O3 > H3P O2. See Answer Calculate the acid ionization constant (Ka) for the acid. 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.) What is the pH of a .11 M solution of C6H5OH (Ka = 1.3x10^-10). What is the equilibrium concentration of D if the reaction begins with 0.48 M A? {/eq} is {eq}2.8 \times 10^{-9} The K_a for HClO is 2.9 times 10^{-8}. nearly zero. The Ka of HCN is 6.2 x 10-10. What is the expression for Ka of hydrobromic acid? pH =, Q:Identify the conjugate acid for eachbase. in the beaker, what would be the pH of this solution after the reaction goes to completion? 7.54. b. (Ka = 2.5 x 10-9), What is the pH of a 0.185 M aqueous solution of potassium hypochlorite, KCIO? (The value of Ka for hypochlorous acid is 2.9 x 10^-8.) What is the pH of an aqueous solution of hypobromous acid with an initial concentration of 0.183 M? Ka. The Ka of hydrofluoric acid (HF) at 25 degree C is 6.8 x 10^-4. A:The relation between dissociation constant for acid, base and water is given as follows, The Ka of hydrocyanic acid, HCN, is 5.0 x 10-10. The acid dissociation K_a of acetic acid (HCH_3CO_2) is 1.8 \times10^{-5} . Find the base. To know more check the Calculate the acid dissociation constant K_a of barbituric acid. Find the pH of a 0.0106 M solution of hypochlorous acid. What is the pH of a 0.22 M solution of the acid? k a for hypobromous acid, hbro, is 2.0 10-9. karlibghs5921 karlibghs5921 07/30/2018 Chemistry College answered expert verified . Calculate the value of the acid-dissociation constant. K, = 6.2 x 10 The dissociation of HA is: HA + H_2O rightleftharpoons H_3O^+ + A^-. Given that K_a for HBrO is 2.8 times 10^{-9} at 25 degrees C, what is the value of K_b for BrO^- at 25 degrees C? What is the pH of an aqueous solution of 2.20 \times 10^{-2} M potassium hydroxide? (Ka = 1.75 x 10-5). 5.0 times 10^{-9} c. 3.4 times 10^{-7} d. 3.5 times 10^{-5} e. 7.1 times 10^{-5}. conjugate acid of HS: The Ka of HC7H5O2 is 6.5 x 10-5. %3D Is this solution acidic, basic, or neutral? The Ka for HF is 6.9 x 10-4. %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)? 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+. Find the pH of a 0.0075 M aqueous solution of hypochlorous acid (HClO), for which Ka = 3.5 x 10-8. The pH of a 0.175 M aqueous solution of a weak acid is 3.52. What is the value of Ka for the acid? Round your answer to 1 decimal place. What is the pH of a 0.435 M CH3CO2H solution? An 8.0 \times 10^{-2} M solution of a monoprotic acid has a percent dissociation of 0.62%. Kb of base = 1.27 X 10-5 The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25 degree C is 4.48. 7.1 10 4 b. General Chemistry - Standalone book (MindTap Cour Introduction to General, Organic and Biochemistry. Find th. Part A What is the [H_3O^+] of 0.146 M HNO? Calculate the pH of a 0.010 M solution of iodic acid (HIO3, Ka = 0.17). What is the pH of a 0.546 M hypochlorous acid, HOCl, solution? After the reaction is in equilibrium, there is (0.0035 - x) M, x M, and x M of HBrO, H+, and BrO- respectively. 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 The dissociation of a weak Bronsted acid species in aqueous solution is an incomplete process that generally favors the reactant side of the equation. Q:What is Kb for the conjugate base of CH3COOH (Ka = 1.8 x 10)? (a) Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. Between 4 and 5 C. Approximately = 7 D. Between 8 and 9 E. Between 9 and 10 Justify your answer with a calculation What is the pH of an aqueous solution of 0.523 M hypochlorous acid? The Ka of HCN at 25.0 degrees Celsius is 4.9 x 10-10. What is the pH of an aqueous buffer solution prepared from 0.95 M NH_3 and 1.22 M NH_4Cl? Kb of NH3 = 1.76 105, What is the pH of a solution that has 0.300 M HNO2 and 0.300 M HCN? What is the value of Ka for hydrocyanic acid? Journal of inorganic biochemistry, 146, 61-68. What is its Ka value? (Ka = 4.60 x 10-4). Find the percent dissociation of this solution. Calculate the H+ in an aqueous solution with pH = 3.494. The k_a for HA is 3.7 times 10^{-6}. Ka = 2.8 x 10^-9. Upon treatment of these aqueous solutions with salts of Pb2+, Hg2+, and Ag+, the corresponding heavy metal bromites precipitate as solids. 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. Ka = 1.8 \times 10^{-4}. An 8.0 x 10^-2 M solution of a monoprotic acid has a percent dissociation of 0.56%. A:Ka x Kb = Kw = 1 x 10-14 Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. Then, from following formula - 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. (b) calculate the ka of the acid. The Kb of NH3 is 1.8 x 10-5. Createyouraccount. Chemistry questions and answers. Ka of HBrO = 2.8 109, What is the pH of a 0.250 M solution of HCN? The acid dissociation constant Ka of hydrocyanic acid HCN is 6.21010. The K_a for HCOOH is 1.8 x 10^-4 M. As usual, report pH to 2 decimal places. Ka of HCN = 4.9 1010 4.96 A 0.145 M solution of a weak acid has a pH of 2.75. Like the acid, hypobromite salts are unstable and undergo a slow disproportionation reaction to yield the respective bromate and bromide salts. 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.) Given that Kb for (CH3)2NH is 5.4 * 10-4 at 25degree C, what is the value of Ka for (CH3)2NH2, Given that at 25.0 degree 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 Ka for benzoic acid is 6.3 * 10^-5. HCN -----> H+ + CN-, Q:A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. 8.14 (You can calculate the pH using given information in the problem. What is the pH of a 0.11 M solution of the acid? *Response times may vary by subject and question complexity. Determine the acid ionization constant (ka) for the acid. Get access to this video and our entire Q&A library, What is Salt Hydrolysis? What is the value of Ka? (Ka for HNO2 = 4.5 x 10-4). (The value of Ka for hypochlorous acid is 2.9 * 10-8. Round your answer to 1 decimal place. Express the pH numerically using one decimal place. Since OH is produced, this is a Kb problem. (Ka = 2.9 x 10-8). This begins with dissociation of the salt into solvated ions. Q:. The ka of hypochlorous acid HClO is 3.5 \times 10^{-8}. What is the value of Ka for HClO, given that a 0.10 M solution has a pH of 4.27? What is the value of it"s k_a? A 0.0115 M solution of a weak acid has a pH of 3.42. Calculate the acid dissociation constant, Ka, of butanoic acid. Thus, we predict that HBrO2 should be a stronger acid than HBrO. 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 dissociation constant, Ka, for gallic acid is 4.57 x 10-3. The Ka of HF is 6.8 x 10-4. What is its Ka? First week only $4.99! Calculate the pH of a 4.0 M solution of hypobromous acid. Ka = 5.68 x 10-10 (Ka of HCHO = 6.3 x 10) With 0.0051 moles of CHO and 0.0123 moles of HCHO in the beaker, what would be the pH of this solution after the reaction goes to completion? HClO 3 HBrO 3 HBrO 2 A. HClO 3 < HBrO 3 < HBrO 2 B. HBrO 2 < HBrO 3 < HClO 3 C. HBrO 3 < HClO 4 < HBrO 2 D. HBrO 3 < HBrO 2 < HClO 3 Brnsted-Lowry Acids and Bases. These three species exist in a chemical equilibrium and they are interrelated by a known acid dissociation constant {eq}K_a {/eq}. Ka of HF = 3.5 104 and Ka of HCN = 4.9 1010, What is the pH of a 0.100 M NaClO2 solution? CN- + H2O <---> HCN + OH- pH = What is the pH of a 0.0944 M aqueous solution of formic acid, HCOOH? (Ka = 6.3 x 10-5), What is the pH of a 0.0250 M solution of HCN? 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? A weak acid can be defined as the acid which dissociates partially into its ions when it is added with water. This is confirmed by their Ka values . Check your solution. Round your answer to 1 decimal place. Concentration of NH4Cl = 0.140 M. Q:Use the Kb for the nitrite ion, NO2, to calculate the Ka for its conjugate acid. A student takes the full 1000.0 mL of the buffer prepared in part (a) and adds 1.00 g KOH. What is the pH of a 0.150 M solution of NaC2H3O2? The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25^\circ C is 4.48. F4 What is the pH of the solution? With four blue flags and two red flags, how many six flag signals are possible? What is the pH of a 0.350 M HBrO solution? The pH of a 0.20 M solution of a weak monoprotic acid is 3.95. (Ka = 2.0 x 10-9), Calculate the pH of a 0.719 M hypobromous acid solution. Kb= Kw=. What is the pH of a 0.55 M aqueous solution of HBrO at 25 degree C? Become a Study.com member to unlock this answer! esc The given compound is hypobromous acid (weak acid). (Ka = 1.0 x 10-10). 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.) 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? The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10^{-9}. 8.46. c. 3.39. d. 11.64. e. 5.54. Acid with values less than one are considered weak. What is the pH of a buffer solution that is 1.00 M in HCN and 0.100 M in KCN? Be sure to include the proper phases for all species within the reaction. What is the pH of a neutral solution at the same (Ka = 4.9 x 10-10), Calculate the pH of a 1.7 M solution of hydrocyanic acid. 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. R The pH of a 0.68M solution of pentanoic acid HC5H9O2 is measured to be 2.50. In comparison to other oxygen-centered oxidants (hypohalites, anions of peroxides) and in line with its low basicity, bromite is a rather weak nucleophile. What is the value of Ka? [10] Rate constants of bromite towards carbocations and acceptor-substituted olefins are by 13 orders of magnitude lower than the ones measured with hypobromite. Determine the pH of a 1.0 M solution of NaC7H5O2. What is the pH of a 0.176 M aqueous solution of sodium fluoride, NaF? A 0.110 M solution of a weak acid (HA) has a pH of 3.28. [8], Using another method, the pKa for bromous acid was measured based on the initial velocity of the reaction between sodium bromites and potassium iodine in a pH range of 2.98.0, at 25C and ionic strength of 0.06M. The first order dependence of the initial velocity of this disproportionation reaction on [H+] in a pH range of 4.58.0. Kb BrO- = Kw / Ka HBrO = (1 x 10^-14) / (2.0 x 10^-9) = 5.0 x 10^-6 . What is the pH of a 1.24 mol/L solution of HCN(aq) if its Ka = 6.2 x 10-10? A. What is the acid dissociation constant (Ka) for the acid? Calculate the pH of a 4.0 M solution of hypobromous acid. You must use the proper subscripts, superscripts, and charges. An acid donates a hydrogen ion to form its conjugate base, A:Given :- chemical formula = HCO3- Was the final answer of the question wrong? The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25 C is 4.48. The K_{a} for HC_{2}H_{3}O_{2} is 1.8\times 10^{-5}. If the degree of dissociation of one molar monoprotic acid is 10 percent. What is the K a value for this acid? Ka: is the equilibrium constant of an acid reacting with water. K_a for hypobromous acid, HBrO, is 2 \times 10^{-9}. What is Ka for this acid? A 0.190 M solution of a weak acid (HA) has a pH of 2.92. A diprotic acid, H2A, has acid dissociation constants of Ka1 = 2.71 x 10-4 and Ka2 = 2.72 x 10-12. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate the pK_a value for riboflavin with a K_a of 9.55 times 10^{-11}. A diprotic acid, H2A, has acid dissociation constants of Ka1 = 1.29 * 10^{-4} and Ka2 = 2.77 * 10^{-12}. The Ka for hypochlorous acid, HOCl, is 3.5 x 10-8. A:The given reaction is an acid-base reaction, Q:Consider the following acid-base pairs: What is the pH of a 0.420 M hypobromous acid solution? The value of acid dissociation constant measured by this method is Ka = (3.70.9)104M and pKa = 3.430.05.[9]. Calculate the pH of a 0.12 M HBrO solution. ), Find the pH of a 0.0176 M solution of hypochlorous acid. 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. Remember to convert the Ka to pKa. If one of the resulting ions is appreciably basic then it will hydrolyze as well to produce a basic pH for the salt solution. What is the pH of the buffer after the addition of the KOH (assuming the addition of KOH does not affect the volume)? What is the value of Ka for the acid? Round your answer to 1 decimal place. What is the value of K_a for HBrO? # Calculate the pH of a solution made by adding 39.0 g of sodium formate, NaHCOO, to 200. mL of 0 76 M formic acid, HCOOH. The experimental data of the log of the initial velocity were plotted against pH. 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. Calculate the pH of a 3.3 M solution of trimethylacetic acid. What is the pH of a 0.113 M aqueous solution of sodium benzoate, NaC6H5COO? The strength of an acid refers to the ease with which the acid loses a proton. a. Calculate the K_a of the acid. What is the value of K{eq}_a pH= pKa+log [base] [acid] pH=log (2.510^ (9))+ log (0.1200.350)=8.14) Initial concentration of CH3NH2solution = 0.21M 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.