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LL ORG CHEM
- For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) H2S(aq) + CO32(aq) HS(aq) + HCO3(aq) (b) HCN(aq) + SO42(aq) CN(aq) + HSO4(aq) (c) SO42(aq) + CH3CO2H(aq) HSO4(aq) + CH3CO2(aq)arrow_forwardSodium benzoate is a salt of benzoic acid, C6H5COOH. A 0.15 M solution of this salt has a pOH a 5.31 at room temperature. A. Calculate the value for the equilibrium constant for the reaction: C6 H5COO- + H2O C6H5COOH + OH B. What is the Ka value for benzoic acid ? C. Benzoic acid has a low solubility in water. What is its molar solubility if a saturated solution has a pH of 2.83 at room temperature?arrow_forward1. For each acid-base reaction, label the acid, the base, the conjugate acid, and the conjugate base, and determine whether the equilibrium lies toward reactants (to the left) or toward products (to the right) ' a) b) d) H₂O OH + IZ Br Хон NH₂ H₂O OH HBr Xo NH3arrow_forward
- 2 What is the pH of a solution of 0.1M Acetic Acid with 0.01 M HCl added. The Ka for acetic acid is 1.8 x 10-5? What is the pH of a solution of 0.1M acetic acid with 0.01 M sodium acetate added. The Ka for acetic acid is 1.8 x 10-5arrow_forwardAbout this time, you may be wishing you had an aspirin. Aspirin is an organic acid with a Ka of 3.27 104 for the reaction. HC9H7O4(aq) + H2O() C9H7O4(aq) + H3O+(aq) If you have two tablets, each contains 0.325 g of aspirin (mixed with a neutral binder to hold the tablet together), and you dissolve then in a glass of water to give 225 mL of solution, what is the pH of the solution.arrow_forwardFor each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid? (a) Acetic add, Ka = 1.74 105 (b) Chloroacetic acid, Ka= 1.38 103arrow_forward
- What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. HC1O4+ H2O — NH/ + H2O -» HCOr + OH" —arrow_forward8-15 Write an equation for the reaction that takes place when each base is added to water. (a) LiOH (b) (CH3)2NH (c) Sr(OH)2 (d) CH3CH2NH2arrow_forwardWhich of the following will increase the percent of NH3 that is converted to the ammonium ion in water (Hint: Use LeChatelier’s principle.)? (a) addition of NaOH. (b) addition of HCl. (c) addition of NH4Clarrow_forward
- Barbituric acid, HC4H3N2O3, is used to prepare barbiturates, a class of drugs used as sedatives. Its Ka is 9.8105. Calculate [H+] in solutions prepared by adding enough water to the following to make 1.45 L. (a) 0.344 mol (b) 28.9 garrow_forwardCalculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H5NH+, in a 0.10-M aqueous solution of pyridine (Kb = 1.7 109).arrow_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
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