ASK AN EXPERT. Hence it will dissociate partially as per the reaction 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. 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. Calculate the H+ in an aqueous solution with pH = 11.93. Round your answer to 2 significant digits. The equilibrium expression of this ionization is called an ionization constant. An 8.0 x 10^-2 M solution of a monoprotic acid has a percent dissociation of 0.56%. Round your answer to 2 significant digits. Round your answer to 1 decimal place. The Ka of HF is 6.8 x 10-4. Salts of hypobromite are rarely isolated as solids. What is the pH of a buffer solution that is 1.00 M in HCN and 0.100 M in KCN? (b) To write the K a expression of CH 3 COOH in water, we should write the balanced reaction first -. What is the Ka of a 0.80 M HClO solution whose pH is 3.81? Bronsted Lowry Base In Inorganic Chemistry. 11 months ago, Posted (Ka = 2.5 x 10-9). CH,COOH(aq) + H,O(1) = H,O*(aq) +, A:According to Bronsted-Lowry concept of Acids and Bases an acid is a substance which give a proton, Q:When calculating [H3O +] for weak acid solutions, we can often use the x is small approximation., A:Nature of approximation and its validity:The smaller value of the equilibrium constant of the weak, Q:calculate delta H^ , Delta S^ , and delta G^ of 3H 2(g) +N 2(g) NH 3(g), Q:the conjugate base for C6H4(CO2H)2 is called, A:Conjugate base What is the pH of an aqueous solution with H+ = 2.0 x 10-9 M? What is the percent ionization of the acid at this concentration? To find a concentration of H ions, you have to. What is the pH of a 0.176 M aqueous solution of sodium fluoride, NaF? What is are the functions of diverse organisms? 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 pH of the solution? Hydrobromic is stronger, with a pKa of -9 compared to What is the [OH-] in an aqueous solution with a pH of 7? 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? Determine the pH of a 1.0 M solution of NaC7H5O2. The pH of a 0.68M solution of pentanoic acid HC5H9O2 is measured to be 2.50. (The value of Ka for hypochlorous acid is 2.9 x 10 8. Find the base. What is the pH of a solution which is 0.0100 M in HA and also 0.0020 M in NaA (Ka = 9.0 x 10-6)? Thus, we predict that HBrO2 should be a stronger acid than HBrO. copyright 2003-2023 Homework.Study.com. Ka = 2.8 x 10^-9. What is the pH of a 0.350 M HBrO solution? What is the OH- of an aqueous solution with a pH of 2.0? Learn about salt hydrolysis. All other trademarks and copyrights are the property of their respective owners. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3 = 4.2 1013. What is the pH of the buffer after the addition of the KOH (assuming the addition of KOH does not affect the volume)? Given that {eq}K_a HBrO, Ka = 2.3 times 10^{-9}. What is the pH of 0.264 M NaF(aq)? Concentration of NH4Cl = 0.140 M. Q:Use the Kb for the nitrite ion, NO2, to calculate the Ka for its conjugate acid. +OH. Q:What is Kb for the conjugate base of HCN (Ka = 4.9 10)? A:Given : Initial concentration of weak base B = 0.590 M The K_a of 0.1M acetic acid is 1.8 \times 10^{-5}. b) What quantity in moles of C7H5O2 would be present before the reaction takes place? What is the pH of a 0.00100 F solution of hypobromous acid (HOBr) in pure water? A 9.0 times 10^{-2} M solution of a monoprotic acid has a percent dissociation of 0.55%. A 0.190 M solution of a weak acid (HA) has a pH of 2.98. {/eq} for {eq}HBrO Ka = 5.68 x 10-10 Salt hydrolysis is the reaction of a salt with water. [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. (a) Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. calculate its Ka value? BrO + HO HBrO + OH Kb = [HBrO] [OH]/ [BrO] = (x) (x)/ (0.800 -x) = 5.0 10 Since Kb is small compared to 0.800, we can neglect the x-term to simplify the calculation. (Ka of NH4+ = 5.6 x 10-10), What is the pH of a 0.402 M aqueous solution of NaCH3COO? What is the pH of an aqueous solution of 4.69 x 10-3 M hydrobromic acid? What is the pH of 0.25M aqueous solution of KBrO? A 0.060 M solution of an acid has a pH of 5.12. %3D What is the pH of a 0.420 M hypobromous acid solution? Calculate the concentration of OH- and the pH value of an aqueous solution in which (H3O+) is 0.014 M at 25 degrees Celcius. 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. What is the pH of an aqueous solution of 0.523 M hypochlorous acid? Determine the Ka value for an acid where a 0.05 M solution has a measured pH of 3. What is Kb for the conjugate base of HCN (Ka = 4.9 10)? Hypobromous acid, a powerful endogenous electrophile: Experimental and theoretical studies. What is the value of Ka for the acid? What is the pH of a 0.225 M KNO2 solution? Kb of base = 1.27 X 10-5 [CH3CO2][CH3COOH]=110 ( pKa p K a = 8.69) a. The pH of 0.042 M Hypobromous acid (HOBr) is 5.07. 3.4 \times 10^{-6} M c. 2.7 \times 10^{-5} M d. 1.2 \times 10^{-5} M e. 4.0 \times 10^{-5} M. the Ka for HC_2H_3O_2 is 1.8 * 10^-5. Each compound has a characteristic ionization constant. 2.2 10-5 What is the pH of a 0.135 M NaCN solution? The acid dissociation constant K_a of alloxanic acid (HC_4H_3N_2O_5) is 2.24 \times 10^{-7}. Round your answer to 2 significant digits. The Ka for benzoic acid is 6.3 * 10^-5. What is Kb for the hypochlorite ion? What is the value of Ka for the acid? Ka for NH4+. Ka (NH_4^+) = 5.6 \times 10^{-10}. First week only $4.99! This can be explained based on the number of OH, groups attached to the central P-atom. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]= 6.1 x 10-4 pH=? What is K_a for this acid? Calculate the H3O+ and OH- concentrations in this solution. The pH of a 0.10 M solution of a monoprotic acid is 2.96. x / 0.800 = 5 10 x = 2 10 Round your answer to 1 decimal place. (Ka for HCIO = 3.5 x 10-8), What is the pH of a 0.20 M solution of HOCl? Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with. (Ka = 2.0 x 10-9), Calculate the pH of a 1.7 M solution of hypobromous acid. Calculate the Ka of the acid. Kb = 4.4 10-4 The acid HOBr has a Ka = 2.5\times10-9. For propanoic acid (HC3H2O2; Ka = 1.3 x 10-5), determine the pH and percent dissociation of a 0.100 M solution. What is the pH of a 0.420 M hypobromous acid solution? 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? What is the value of Ka. Calculate the pH of a 0.300 KBrO solution. 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? 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. Round your answer to 2 decimal places. (Ka = 1.8 x 10-4), What is the pH of a 9.87 x 10-2 M aqueous solution of potassium nitrite, KNO2? Who is Katy mixon body double eastbound and down season 1 finale? Calculate the pH of the following aqueous solution: 0.34 M C6H5NH3NO3. Round your answer to 2 decimal places. (Ka = 2.5 x 10-9). Part B What is the pH of 0.146 M HNO_2? Given that Kb for CH3NH2 is 5.0 * 10^-4 at 25 degree C, what is the value of Ka for CH3NH. The pH of a 0.79 M solution of butanoic acid (HC4H7O2) is measured to be 2.46. 1.0 10 7 c. 1.3 10 3 d. 4.0 10 7 e. 1.0 10 7. The acid dissociation K_a of acetic acid (HCH_3CO_2) is 1.8 \times10^{-5} . Given that Ka for HBrO is 2.8 x 10-9 at 25 degree C, what is the value of Kb for BrO- at 25 C? The pH of a 1.3 M solution of carbonic acid (H_{2}CO_{3} is measured to be3.12. Calculate the Ka for this acid. copyright 2003-2023 Homework.Study.com. (Ka = 2.0 x 10-9). 1. a. Determine the pH of each solution. Acid with values less than one are considered weak. D) 1.0 times 10^{-6}. 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. 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. What is the value of Kb for CN-? Get plagiarism-free solution within 48 hours, Submit your documents and get free Plagiarism report. The add dissociation constant K_a of carbonic acid (H_2CO_3) s 4.5 * 10^-7. Round your answer to 1 decimal place. (Ka = 1.8 x 10-4), What is the pH of a 0.530 M solution of hypochlorous acid? The dissociation of a weak Bronsted acid species in aqueous solution is an incomplete process that generally favors the reactant side of the equation. a. 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? Express the pH numerically using one decimal place. Calculate the k_a of a weak acid if a 0.075 M solution of the acid has a pH of 3.97 at 25 C. K_a = ..* 10 ^ (Enter your answer in scientific notation.). [3] Bromide is also used in hot tubs and spas as a germicidal agent, using the action of an oxidizing agent to generate hypobromite in a similar fashion to the peroxidase in eosinophils. Calculate the Ka for a 0.10 M HClO solution that is found to have a pH of 4.23. {/eq} is {eq}2.8 \times 10^{-9} Except where otherwise noted, data are given for materials in their, Egon Wiberg, Arnold Frederick Holleman (2001), "Journal of the Society of Chemical Industry. - Definition & Examples. 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? K_a for hypobromous acid, HBrO, is 2 \times 10^{-9}. Start your trial now! What is the pH of a 0.420 M hypobromous acid solution? 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. (Ka = 2.0 x 10-9), Calculate the pH of a 0.719 M hypobromous acid solution. A 0.110 M solution of a weak acid (HA) has a pH of 3.28. Determine the Ka and percent dissociation of a monoprotic weak acid if a 0.50 M solution has a pH of 2.75. Kb of C5H5N = 1.7 109, What is the pH of a solution that has 0.200 M HF and 0.200 M HCN? The pH of a 0.200M HBrO solution is 4.67. Plug the values into Henderson-Hasselbalch equation. Is this solution acidic, basic, or neutral? Find the value of pH for the acid. A 0.152 M weak acid solution has a pH of 4.26. A 0.148M solution of a monoprotic acid has a percent dissociation of 1.55%. Round your answer to 1 decimal place. hydrochloric acid's -8. Given that Ka for HCN is 4.9 x 10^-10 and Kb for NH3 is 1.8 x 10^-5, calculate Kb for CN- and Ka for NH4+. 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 Kb of (CH3)3N = 6.4 105 and more. A:We have given that (Ka = 3.5 x 10-8). What is the pH of a 0.15 M aqueous solution of sodium formate (NaHCO_2)? 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). A 0.110 M solution of a weak acid (HA) has a pH of 3.30. Calculate the pH of a 4.5 M solution of carbonic acid. (Ka = 2.8 x 10-9). (Ka = 3.5 x 10-8). Ka of HNO2 = 4.6 104. Bromous acid is an intermediate stage of the reaction between bromate ion (BrO3 ) and bromine (Br):[6][7]. What is the value of Ka for the acid? The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases. 4 View this solution and millions of others when you join today! A 0.159M solution of a monoprotic acid has a percent ionization of 1.25%. (Ka = 4.0 x 10-10). Spell out the full name of the compound. A:An acid can be defined as the substance that can donate hydrogen ion. 8.14 (You can calculate the pH using given information in the problem. 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 What is the Ka value of the conjugate acid of a base with a Kb value of 8.2 x 10^-7? (Ka of HC?H?O? The concentration of an aqueous solution of HCN is 0.05 M. Calculate the pH of the solution. 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 . Ka for HCN is 4.9 x 10^-10 and Kb for NH3 is 1.8 x 10^-5, calculate? Calculate the H3O+ in a 0.285 M HClO solution. What is the pH of a 0.0157 M solution of HClO? 5.90 b. The pH of a 1.25 M solution of an unknown monoprotic acid is 5.43. 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. What is the pH of a 0.145 M solution of (CH3)3N? The species which can, Q:What is the pH of a 0.21 M solution of methylamine, A:Given :- Nov 18 2022 08:12 AM 1 Approved Answer Mark B answered on November 20, 2022 4 Ratings ( 9 Votes) (Ka = 1.0 x 10-10). Consider the reaction of 56.1 mL of 0.310 M NaCHO with 50.0 mL of 0.245 M HBr. Weekly leaderboard Home Homework Help3,800,000 What is the pH of an aqueous solution with H+ = 6.5 x 10-7 M? (Ka for HF = 7.2 x 10^-4). If one of the resulting ions is appreciably basic then it will hydrolyze as well to produce a basic pH for the salt solution. Enter your answer as a decimal with one significant figure. Round your answer to 2 significant digits. The strong bases are listed at the bottom right of the table and get weaker as we move to the top of the table. Calculate the value of ka for this acid. The pH of a 0.175 M aqueous solution of a weak acid is 3.52. Calculate the pH of a 1.45 M KBrO solution. ), What is the pH of an aqueous solution with a hydrogen ion concentration of [H^+] = 9.0 x 10^-7 M? HOBr Molar mass: 96.911 Density: 2.470 g/cm 3: Boiling point: 20-25 C (68-77 F; 293-298 K) Acidity (pK a) : 8.65 Conjugate base: Hypobromite KBrO is a fully soluble salt that will dissociate to give potassium cations and hypobromite anions. Was the final answer of the question wrong? Since the moles are the same, this tells us that ALL of the KOH was converted to KBrO. (Ka = 3.5 x 10-8). The Ka of HCN is 6.2 times 10^(-10). A 0.190 M solution of a weak acid (HA) has a pH of 2.92. The K_a for HClO is 2.9 times 10^{-8}. What is the acid's K_a? 2.5 times 10^{-9} b. whixh, A:The species which can accept a pair of electrons is known as Lewis acid. What is the pH of a buffer made from 0.350 mol of HBrO (Ka = 2.5 10) and 0.120 mol of KBrO in 2.0 L of solution? The Ka of HBrO is 2.5 x 10-9 When eql volumes of 0.1 M HbrO and 0.1 M NaBrO are mixed the pH of the solution will be A. HCO, + HPO,2 H2CO3 (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.). Become a Study.com member to unlock this answer! 1.25 B. What is the pH of a 0.186 M aqueous solution of sodium fluoride, NaF? Obtain the: Kb value for NO2- The Ka value for NH3OH+ (hydroxylammonium ion). Ka = [HOBr] [H+ ][OBr ] . Ka of HBrO = 2.8 109 4.74 What is the pH of a 0.250 M solution of HCN? K, =, Q:For each pair of molecules or ions, select the stronger base and write its Lewis structure. Then substitute the K a to solve for x. A 0.165 M solution of a weak acid has a pH of 3.02. A weak acid can be defined as the acid which dissociates partially into its ions when it is added with water. The pH of aqueous 0.50 M hypobromous acid, HBrO is 4.45. What is the value of Kb for CN^-? Given that Kb for CH3CH2NH2 is 6.3 10-4 at 25 C, what is the value of Ka for CH3CH2NH3 at 25 C? 1 point earned for a correct (Ka = 0.16). The given compound is hypobromous acid (weak acid). Given that Ka for HBrO is 2.8 x 10-9 at 25 degree C, what is the value of Kb for BrO- at 25 C? conjugate acid of HS: The Ka for hypobromous acid, HBrO, is 2.0 x 10-9. Express your answer using two decimal places. Express your answer using two significant figures. Using the answer above, what is the pH, A:Given: What is the value of Ka? 3.28 C. 1.17 D. 4.79 E. 1.64. What is the pH of an aqueous solution with [H3O+] = 4 * 10-13 M ? Round your answer to 1 decimal place. Ka of HC7H5O2 = 6.5 105 What is the value of K{eq}_a Since B is a weak, Q:Construct the expression for Ka for the weak acid, HPO,2". Fournisseur de Tallents. (Ka = 2.0 x 10-9), Calculate the H3O+ in a 1.4 M solution of hypobromous acid. Createyouraccount. What is the H3O+ in an aqueous solution with a pH of 12.18. A 0.115 M solution of a weak acid (HA) has a PH of 3.33. All rights reserved. Kb of CH3NH2 = 4.4 104, What is the pH of a 0.200 M solution of HCOOH? 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. What is the conjugate base. What is the value of Kb for F-? 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. 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. A 1.0 M H2S solution has a pH of 3.75 at equilibrium. It is generated both biologically and commercially as a disinfectant. Calculate the H3O+ in an aqueous solution with pH = 10.48. 8.3. c. 9.0. d. 9.3. a. An 8.0 \times 10^{-2} M solution of a monoprotic acid has a percent dissociation of 0.62%. (b) H3C6H5O7, Q:Given that acetic acid hasKa= 1.8 x 105, what is the pH of a solution that contains the molar, A:Given: 7.54. b. K_a for hypobromous acid, HBrO, is 2.0 times 10^{-9}. The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10{eq}^{-9}. Acid and it's. The acid dissociation constant Ka of hypobromous acid (HBrO) is 2.3*10^{-9}. H Cl O ClO HClO ClO HClO (NaClO) (Ca(ClO) 2) . The compound is generated in warm-blooded vertebrate organisms especially by eosinophils, which produce it by the action of eosinophil peroxidase, an enzyme which preferentially uses bromide. 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 mixture that contains 0.23 M of HCOOH and 0.12 M of HBrO. Q:What is the conjugate base of HClO4, H2S, PH4 +, HCO3 - ? Study Ka chemistry and Kb chemistry. K, = 6.2 x 10 Get access to this video and our entire Q&A library, What is Salt Hydrolysis? 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. (NH4+) = 5.68 x 10^-10 Vip Thumbnail | 2 Thumbnail ,android phone se youtube thumbnail kaise banaye,how to make thumbnail for . The pH of a 0.21 M solution of a weak monoprotic acid, HA, is 2.92. The K_a of formic acid (HCOOH) is 1.8 \times 10^{-4}. All ionic compounds when dissolved into water break into different types of ions. Q:Kafor ammonium, its conjugate acid. Hypobromous acid is a weak acid (Ka = 2.8 * 10-9 M). Find the value of pH for the acid. What is the OH- in an aqueous solution with a pH of 8.5? What is the pH of an aqueous solution with [H3O+] = 4 * 10-13 M ? [Br-] / [HBr] However the value of this expression is very high, because HBr is a STRONG acid, meaning that much more than 99.9% of the HBr molecules in water are protolized (ionized . If the degree of dissociation of one molar monoprotic acid is 10 percent. The Ka value for benzoic acid is 6.4 \times 10^{-5}. %3D A: Given data,Molarity of HCN=0.0620MKa=4.910-10 question_answer question_answer What is the value of Ka for hydrocyanic acid? Calculate the pH of a 2.3 M aqueous solution of benzoic acid. 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? Createyouraccount. Ka for HNO_2 is 5.0X 10^-4. What is the pH of a 0.350 M HBrO solution? (Ka of C5H6CO2H = 6.3 x 10-5), What is the pH of 0.035 M aqueous benzoic acid? The pH of a 0.250 M cyanuric acid solution is 3.690. A 9.0 x 10-2 M solution of a monoprotic acid has a percent dissociation of 0.58%. with 50.0 mL of 0.245 M HBr. A 0.120 M weak acid solution has a pH of 3.75. C. The pH of a 0.068 M weak monoprotic acid is 3.63. Createyouraccount. F3 A:Ka x Kb = Kw = 1 x 10-14 (remember,, Q:Calculate the pH of a 0.0158 M aqueous 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 a 0.25 M weak monoprotic acid (HA) solution is 3.50. Find the pH of a 0.0106 M solution of hypochlorous acid. The pH of 0.255 M HCN is 4.95. The Ka, A:Given that - Createyouraccount. b) What is the Ka of an acid whose pKa = 13. {/eq} for {eq}BrO^- Round your answer to 1 decimal place. The Ka for cyanic acid is 3.5 x 10-4. What is the pH of an aqueous solution of 0.36 M hydrocyanic acid? 2.83 c. 5.66 d. 5.20 e. 1.46. 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.) 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? What is the pH and pK_a of the solution? Chemistry questions and answers. 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. {/eq} at 25 degree C, what is the value of {eq}K_b With 0.0051 moles of C?H?O?? What is the value of K_{b} for C_{2}H_{3}O_{2}^-. (Ka for HF = 7.2 x 10^{-4}) . Calculate the pH at which an aqueous solution of this acid would be 1.6% dissociated. 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. Calculate the pH of a 0.50 M NaOCN solution. Kw = ka . (Hint: The H_3O^+ due to the water ionization is not negligible here.). 3 months ago, Posted (Ka = 1.8 x 10-5). 3. Ka of HCN = 4.9 1010, What is the pH of a 0.200 M KC7H5O2 solution?