Calculate the percent dissociation of trimethylacetic acid (C,H,CO,H) in a 0.45 M aqueous solution of the stuff. You may find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. %
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- Calculate the percent dissociation of trimethylacetic acid (C,H,CO,H) in a 0.52 mM aqueous solution of the stuff. You may find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. | %O ACIDS AND BASES Calculating percent dissociation of a weak acid Calculate the percent dissociation of trimethylacetic acid (C4H,CO₂H) in a 0.26 mM aqueous solution of the stuff. You may find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. % Explanation Check 0 X » ZUZZ MILOTOW LLC. All Rights Reserved. Terms of Use | Privacy Center AcceIn a 0.73 mM aqueous solution of trimethylacetic acid (C₂H₂CO₂H), what is the percentage of trimethylacetic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. 1% 00 x10 X $
- Calculate the percent dissociation of trimethylacetic acid (C4H₂CO₂H) in a 0.57 mM aqueous solution of the stuff. You may find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. % OD 4An analytical chemist is titrating 187.6 mL of a 0.4000M solution of trimethylamine ((CH,) N) with a 0.7000M solution of 3 HNO3. The p K, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 19.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = ||4. Calculate the pH of a 0.100 M solution of alanine prepared from the form shown below. pKa (-COOH) = 2.344 and pKa (-NH;") = 9.868. H *H;N- C C O- CH3 pH = 6.106 5. Referring to Question 4, calculate the concentration of the fully protonated form of alanine in the solution described in Question 4. [H2A*] = 1.72*10-$ M
- Part A The chemical 5-amino-2,3-dihydro-1,4-phthalazinedione, better known as luminol, is used by forensic scientists in analyzing crime scenes for the presence of washed-away blood. Luminol is so sensitive that it can detect blood that has been diluted 10,000 times. A basic solution of luminol is often sprayed onto surfaces that are suspected of containing minute amounts of blood. The forensic technician at a crime scene has just prepared a luminol stock solution by adding 15.0 g of luminol into a total volume of 75.0 mL of H2O. What is the molarity of the stock solution of luminol? Express your answer with the appropriate units. Luminol has a molecular weight of 177 g/mol. • View Available Hint(s) HẢ molarity of luminol solution = Value Units Submit Part B Before investigating the scene, the technician must dilute the luminol solution to a concentration of 6.00x10-2 M. The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of…K Calculate the pH of a 0.295 M solution of ethylenediamine (H₂NCH₂CH₂NH₂). The pKa values for the acidic form of ethylenediamine (HFNCH₂CH₂NH3) are 6.848 (pKat) and 9.928 (pK₁2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H₂NCH₂CH₂NH₂] = [H₂NCH₂CH₂NH] = [HNCH₂CH₂NH3] = M M M- Calculate the pH of a 0.102 M solution of ethylenediamine (H, NCH₂CH₂NH₂). The pK, values for the acidic form of ethylenediamine (H; NCH₂CH₂NH) are 6.848 (pK₂1) and 9.928 (pK2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H₂NCH₂CH₂NH₂] = [H₂NCH₂CH₂NH] = [H; NCH₂CH₂NH] = M M M
- Calculate the pH of a 0.295 M solution of ethylenediamine (H₂NCH,CH,NH₂). The pKa values for the acidic form of ethylenediamine (HNCH,CH,NH) are 6.848 (pKa1) and 9.928 (pKa2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H2NCH2CH2NH₂] = [H2NCH,CH,NH] = [HNCH,CH,NH3] = M M MCalculate the pH of a 0.105 M solution of ethylenediamine (H,NCH,CH,NH,). The pKa values for the acidic form of ethylenediamine (H NCH,CH,NH}) are 6.848 (pKa1) and 9.928 (pK2). pH = Calculate the concentration of each form of ethylenediamine in this solution at equilibrium. [H,NCH,CH,NH,] = M [H,NCH,CH,NH] = М [H;NCH,CH,NH†] =Lysine (K) is a triprotic amino acid whose most protonated form has a charge of 2+. Its acid dissociation constants are pK31 = 1.77, pK32 = 9.07, and pkg3 = 10.82. For numbers 1 and 2 refer to the following choices. Write only the letter corresponding to your answer. a. H3K2+ b. H2K²* c. HK2+ d. H3K* e. H2K* f. HK* g. H3K h. H2K i. HK j. H2K- К. НК I. K- m. НК2- п. К2- о. КЗ- 1) At pH 7.47, the second most abundant species is 2) What is the third most abundant species at this pH? 3) At what pH is the concentration of the diprotic species equal to the concentration of the fully deprotonated species. (ANSWER FORMAT: If for example, the answer is 7.12, then c = 7, m =12) C = m =