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- What is the acid dissociation constant Ka for its conjugate acid? If the base dissociation constant Kb for hypochlorite ion is 3.3x10-7Dicarboxylic acids have two dissociation constants, one for the initial dissociation into a rnonoanion and one for the second dissociation into a dianion . For oxalic acid, HO,C-CO,H, the first ionization constant has pKaj = 1.2 and the second ionization constant has pKaz = 4.2. Why is the second carboxyl group so much less acidic than the first?At what pH will 50% of a compound with a pK₂ = 7.4 be in its basic form? Express your answer using one decimal place. pH = = ΠΫΠΙ ΑΣΦ ?
- 6. For the ionization of phenylacetic acid, C6H5CH₂CO₂H + H₂O = H3O+ + C6H5CH₂CO₂ K₂ = 49 × 10-5 (a) What is [C6H5CH₂CO₂] in 0.186 M C6H3CH₂CO₂H? (b) What is the pH of 0.121 M C6H3CH₂CO₂H?Which of the statements below are true? 1. When the NH¼NO3 compound is hydrolyzed in water, the solution becomes alkaline. 2. After the reaction of C-H502H + H2O → C-H502 + H3*, the pH of the solution becomes lower than 7. (pKA C7H502H)= 4.20 3. When the strengths of the conjugate bases that were derived from C2H5COOH and C2H5OH are compared, it is seen that C2H5O> C2H5CO0". 4. When the acid strengths of CH2CICOOH and CH,BRCOOH are compared, the CH2CICOOH is found more acidic than the CH,BRCOOH. O a. 2, 3, and 4 O b. 1, 2, and 4 O c. 2 and 3 O d. 1 and 3 O e. allCalculate the pH at 25 °C of a 0.32M solution of trimethylammonium chloride ((CH3)2NHCI). Note that trimethylamine ((CH3)3N) is N is a weak base with a pK of 4.19. Round your answer to 1 decimal place. = 0 pH =
- Calculate the pH for a mixture of one mole of benzoic acid andone mole of sodium benzoate. The pKa of benzoic acid is 4.2.Calculate the pH and the concentration of all the species present at equilibrium for a 1.0E-4 M asorbic acid H2C6H6O6 solution. pKa1 = 4.1; pKa2 11.8Calculate the pH of a 0.35 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).
- Calculate the concentration of the following weak acids. 2) a) ethanoic acid with pH 4.53 (Ka = 1.74 x 10° mol dm) b) pentanoic acid with pH 3.56 (pK, = 4.86) -58-39. (a) Write the chemical reactions whose equilibrium constants are K and K for imidazole and imidazole hydrochloride, respectively. (b) Calculate the pH of a solution prepared by mixing 1.00 g of imida- zole with 1.00 g of imidazole hydrochloride and diluting to 100.0 mL. (c) Calculate the pH of the solution if 2.30 mL of 1.07 M HC1O4 are added.1. What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Given:Ka of HC2H3O2 = 1.8 x 10-5