Interpretation:
The
Concept introduction:
Acid–base reactions are the reactions in which the acid reacts with the base and tend to neutralize the effect of each other by producing a salt. In the esterification of 3-methylbutyl ethanoate from acetic acid and 3-methyl-1-butanol in the presence of a sulfuric acid catalyst, the ester portion remains in the organic layer on top, whereas water and alcohol constitute the aqueous inorganic layer below, because ester is less denser than water. The impurities, ethanoic acid, and sulfuric acid are removed by treating it with sodium bicarbonate whereas, alcohol is taken up by water.
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Organic Chemistry
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/Aarrow_forwardFind the value of Kb for the conjugate base of the following organic acids. (a) picric acid used in the manufacture of explosives; Ka = 0.16 (b) trichloroacetic acid used in the treatment of warts; Ka = 0.20arrow_forwardConsider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?arrow_forward
- The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107arrow_forwardWrite 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 ionarrow_forwardIonization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forward
- Both ions in the salt ammonium acetate (NH4C2H3O2) hydrolyze in aqueous solution. Explain why this hydrolysis produces a neutral solution rather than an acidic or basic solution.arrow_forwardFormic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.arrow_forwardReacting GeO2 with H2O forms the tetraprotic (four H+ ions) acid, H4GeO4. On a piece of paper, write down the chemical equations for the four acid dissociation equilibria. Match each chemical species below with its correct role in this polyprotic acid system. H4GeO4 H3GeO4 - H2GeO4 2- HGeO4 3- GeO4 4- [ Choose ] the conjugate base of H3GeO4 - the acid in the second H+ dissociation this species' conjugate acid is HGeO4 3- the conjugate base in the third H+ dissociation the conjugate acid of H3GeO4 -arrow_forward
- Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.arrow_forwardIn which direction would the reaction have to run in order to rebalance the ratios of CO2 and H2O to H+ and HCO3 − when CO2 levels are lower than normal?CO2+ H2O ⇌ H2CO3 ⇌ H++ HCO3−arrow_forwardFormic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. 4.Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. 5.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.arrow_forward
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