The equilibrium constant expression for the base-ionization reaction of SO42 would be O [HSO4][OH-] [SO42] [SO42-] [HSO4][OH-] [SO₁²-] [HSO4 [H3O+ O [HSO₁¯] [H3O+] [SO₁₂-]
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- Determine the principal species at the following pH levels for Nitrilotriacetic acid. The most protonated form is C6H10NO6+. pH= 1,2,3,4,10. pK1 = 1.0, pK2 = 1.81, pK3 = 2.52, pK4 = 9.46.Write the equilibrium-constant expressions and obtain numerical values for each constant in the basic dissociation of aniline, C6H5NH2. the acidic dissociation of hypochlorous acid, HClO.Consider the molecule, pentanoic acid which has a pKa of 4.81: H3C OH At each of the following pH values, will the structure be charged or uncharged? i. 11.75 ii. 4.81 iii. 2.95 2
- What is the acid dissociation constant Ka for its conjugate acid? If the base dissociation constant Kb for hypochlorite ion is 3.3x10-7(a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+. (b) Give the conjugate acidof the following Brønsted–Lowry bases: (i) O2-, (ii) H2PO4-.Acidified potassium bromate(V), KBrO3, reacts with hydrogen sulfide, H2S, to give a yellow solid and an orange solution. On shaking the solution with trichloroethane, the trichloroethane layer turned orange-red. (a) Suggest the identity of yellow solid and the orange solution. Describe the type of reaction taking place. (b) Construct a balanced equation for the reaction between KBrO3 and H2S. (C) BrO3- is the conjugate base of HBrO3. Draw the dot and cross structure of HBrO3. (d) HBr is a stronger acid than HCl. However, HBrO3 is a weaker acid than HCIO3. Explain the difference in acidities.
- At 25°C, the Ka of pentafluorobenzoic acid (C6F5COOH) is 0.033. Suppose 0.100 mol of pentafluorobenzoic acid is dissolved in 1.00 L of water. What is the pH of this solution?Identify all of the bases in this equation: PO₄³⁻ + HNO₃ <--> NO³⁻ + HPO₄²⁻ Based on your knowledge of acid/base strength: Which direction will this reaction proceed?Calculate the hydrogen-ion concentration and the pH of a solution of 0.0001M H2CO3, and also calculate what fraction of the H2CO3 has been dissociated. Compare this fraction with the fraction dissociated when the concentration is 0.01M (given that the pH is 4.2 in a 0.01M solution). What generalization can you make regarding the effect of dilution on the degree of dissociation?