Find the pH for the following solutions if it contains: [d] 0.105 M urea, Ka = 0.67 [e] 0.027 M lactic acid, Ka = 1.38 x 10 - 4 [f] 0.105 M aniline, pKa = 4.60 [g] 0.10 M ascorbic acid, pKa = 4.10

A solution contains 0.321 M potassium fluoride and 0.165 M hydrofluoric acid (K₁ = 7.20 × 10-¹). The pH of this solution is A solution contains 0.157 M potassium acetate and 0.167 M acetic acid (Ka = 1.80 × 10-5). The pH of this solution is A solution contains 0.485 M sodium acetate and 0.0779 M acetic acid (Ka = 1.80 × 10-5). The pH of this solution is

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 concentration of CO32– in a 0.030 M solution of carbonic acid, H2CO3? For carbonic acid, Ka1 = 4.2  10–7and Ka2 = 4.8  10–11.