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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionSolubility of gases in water increases with increasing mass. Explain? What is the relationship between the value of pKa and the strength of a weak acid?The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKa of the acid 5.74?
- (a) The PH of rain water collected from two cities A and B was found to be 6 and 5 respectively. Water of which city is more acidic? Find out the ratio of hydrogen ion concentration in the two samples of rain water?Three acids found in foods are lactic acid, LA, (in milk products), oxalic acid, OA, (in rhubarb), and malic acid, MA (in apples). The pKa values are LA =3.88, OA =1.23, and MA =3.40. Which list has the conjugate bases of these acids, lactate, oxalate, and malate, in order of decreasing strength? O lactate > malate > oxalate lactate > oxalate > malate malate > lactate > oxalate oxalate > malate > lactatePhenylacetic acid (C6H5CH2COOH, simplified here to HPAc is a monoprotic acid. It builds up in the blood of persons with phenylketonuria, that if untreated, causes mental retardation and death. A study of the acid shows that the pH of 0.120 M HPAc is 2.62. What are (a) the Ka and (b) pKa of phenylacetic acid?
- A 0.500M solution of a weak acid has a pH of 2.251. a. What is the pKa of the weak acid?d. During the fermentation of wine, a buffer system consisting of tartaric acid and potassium hydrogen tartrate is created as the result of a biochemical reaction. Assuming that at some point in the process, the concentrations of the two components are approximately equal, determine the pH of the wine. The pKa of tartaric acid is 2.96.COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…
- What is the pH of a solution containing 0.50 moles of benzoic acid and 0.75 moles of sodium benzoate if the pka is 4.19?Given the pKa of hypochlorous acid, HOCl, is 7.54. What is the pH of a solution which consists of 0.20 M HOCl and 0.70 M OCl-?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.
