An aqueous solution contains 0.132 mol L-1 of HCl and 0.717 mol L-1 of acetylsalicylic acid (Ka = 3.30×10-4). Determine the concentration of the conjugatebase of acetylsalicylic acid (i.e., acetylsalicylate).
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An aqueous solution contains 0.132 mol L-1 of HCl and 0.717 mol L-1 of acetylsalicylic acid (Ka = 3.30×10-4). Determine the concentration of the conjugatebase of acetylsalicylic acid (i.e., acetylsalicylate).
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- Calculate the percentages of dissociated and undissociated forms present in the following solutions: (a) 0.0010 M glycolic acid (HOCH2CO2H; pKa = 3.83) at pH = 4.50 (b) 0.0020 M propanoic acid (pKa = 4.87) at pH = 5.30The pka of acid HX is 6.02, and the pka of acid HY is 3.76. We can conclude that the Kp value of base X (the conjugate base of HX) should be HY). than the Kp value of base Y (the conjugate base of greater than equal to less than More information is needed to make judgment.The Kp of a solution can be determined from the pKp using the equation: K, = 10-PK, Where: K = base dissociation constant a Use the rules for logarithms and exponents to solve for pKp in terms of Kp. NOTE: Capitalization counts. pKp Submit
- [Review Topics] [References] Use the References to access important values if needed for this question. Consider the following equilibrium between 3-methylbenzoic acid (K,a-5.0x10) and its conjugate base: %3D CH3- CH3- H2O + H30* (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of 3-methylbenzoate ion to the concentration of 3-methylbenzoic acid at a pH of 1.59. ratio [conjugate base] / [acid] Submit Answer Retry Entire Group 9 more group attempts remainingThe pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.1/ 3. Calculate the pK, of hypochlorous acid from its K, value. (Refer to Appendix H.) J Ka 315x1078
- CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.acid, Ka = 7. The value of Ka for acetylsalicylic acid (aspirin) is 3.00x10-4. What is the value of Kb, for its conjugate base, C9H7O4?Which value of delta G would result in K eq =1 Give a delta G that would result in K eq<1
- A:(-) + H₂O(+). For the following named acids: 1a) Consider the reaction AH+ + H₂O a) draw the structure of the acid, b) give the approximate pKa of the conjugate acid in units of 5, c) give the name of the conjugate base, and d) draw the structure of the conjugate base p-Toluenesulfonic acid Conjugate base Dimethyl sulfoxide pka_ name acid pKa name Ethyl Acetate pKa name Benzamide pKa nameThe conjugate base that is produced after the first ionization step of carbonic acid when it has reacted with ethyl amine (CH3CH2NH2) would be _________. H2CO3 CH3CH2NH3+ HCO3- CO3-2 CH2CH2NH Given a Ksp of 4.96 X 10-9 for limestone (calcium carbonate), the calcium concentration in a limestone solution will be__________ the Ksp. greater than less than the same as cannot be determinedThe value of Ka for acetylsalicylic acid (aspirin) is 3.00×10-4. What is the value of Kb, for its conjugate base, C9H7O4-?