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Given
calculate K for the reaction
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Chemistry: Principles and Reactions
- . Write the conjugate base for each of the following acids. a. HBrO b. HNO2 c. HSO3 d. CH3NH3+arrow_forwardCalculate the pKa value for each of the following acids. a. Phosphoric acid (H3PO4), Ka = 7.5 103 b. Hydrofluoric acid (HF), Ka = 6.8 104 c. Hydrogen phosphate ion (HPO42), Ka = 4.2 1013 d. Propanoic acid (HC3H5O2), Ka = 1.3 105arrow_forwardWrite the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)arrow_forward
- Prove that Ka3 Kb1 = Kw for phosphoric acid, H3PO4, by adding the chemical equilibrium expressions that corresponds to the third ionization step of the acid in water with the first of the three successive steps of the reaction of phosphate ion, PO43, with water.arrow_forwardIn each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()arrow_forward25. Which of the following acids have relatively strong conjugate bases? a. HCN b. H2S c. HBrO4 d. HNO3arrow_forward
- Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?arrow_forwardDefine or illustrate the meaning of the following terms: a. Ka reaction b. Ka equilibrium constant c. Kb reaction d. Kb equilibrium constant e. conjugate acidbase pairarrow_forwardIdentify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted—Lowry base, and its conjugate acid in each of the following equations: (a) HNO3+H2OH3O++NO3 (b) CN+H2OHCN+OH (c) H2SO4+CIHCI+HSO4 (d) HSO4+OHSO42+H2O (e) O2+H2O2OH (f) [Cu( H 2 O)3(OH)]++[Al( H 2 O)6]3+[Cu( H 2 O)4]2++[Al( H 2 O)5(OH)]2+ (g) H2S+NH2HS+NH3arrow_forward
- Identify and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid in each of the following equations: (a) NO2+H2OHNO2+OH (b) HBR+H2OH3O++Br (c) HS-+H2OH2S+OH (d) H2PO4+OHHPO42+H2O (e) H2PO4+HClH3PO4+Cl (f) [Fe( H 2 O)5(OH)]2++[Al( H 2 O)6]3+[Fe( H 2 O)6]3++[Al( H 2 O)5(OH)]2+ (g) CH3OH+HCH3O+H2arrow_forwardWhat is the ionization constant at 25 C for the weak acid CH3 NH3+, the conjugate acid of the weak base CH3NH2, Kb=4.4104.arrow_forwardIn each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()arrow_forward
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