A beaker contains a total concentration of 0.33 molar of weak acetic acid with pKa=4.27 and pH=2.02. Calculate the molar concentration of the undissociated (AH) form.
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- Calculate the pKa of the weak acid HA, given that a solution that is 0.357 in HA and 1.24 in A- has pH = 5.32.Provide your answer rounded to 2 decimal digits.Determine the pKa of an acid; a 4e-3M solution of which has a pH of 2.4A weak acid solution with concentration 0.020 M has a pH of 3.7, what is the pKa of this acid?
- Consider a diprotic acid with pKa values of 1.60 and 4.50, that is colorless when fully protonated, deep blue when singly deprotonated, and bright red when doubly deprotonated. Assuming that both colored forms have large and approximately equal molar absorptivities, what can be inferred from a solution of the compound that has a faint blue color?What molar ratio of HPO42-to H3PO4- in solution would produce a pH of 7.0? Phosphoric acid (H3PO4 ), a triprotic acid, has three pKa values: 2.14, 6.86, and 12.4. Hint: Only one of the pKa values is relevant here.:::::(((((((( The PH of a 0.2 M solution of a monoprotic acid is 3.45. Calculate the pKa for this acid. What is the percent ionization of acid?
- The pH of a 0.12 M solution of acetic acid (HCH3CO2) is measured to be 2.83. Calculate the acid dissociation contant Ka of acetic acid.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.The conjugate acid of the base quinoline (1) has pKa = 4 .88.Estimate the pH and the fraction of molecules protonated in a 0.010 M aqueous solution of quinoline .
- Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM. This should include writing a balanced equation describing the acid-base reactions involved, calculation of the pKa for both, calculation of pH, and calculation of the percent dissociation of both.A solution was prepared at 25°C in which the ratio of methylamine (CH3NH2) to the salt methylammonium chloride (CH3NH3Cl) was two to one, and resulted in a pH = 11.00. Calculate Ka for the weak acid methylammonium (CH3NH3+) at 25°C.Identify the species represented by each curve in the fractional composition diagram of a triprotic acid (H3A) with pKa values of 3.00, 6.00 and 10.00.