A. Ka and pka for some acids Acid name Phosphoric acid Dihydrogen phosphate Carbonic acid Acetic acid formula H₂PO4 3 H₂PO H, CO, 2 3 Dack and CH₂COOH out Dissociation reaction H₂PO4 →→ H² + H₂PO н Ka 7.08x10 -3 6.31x106 pka 6.35 4.76
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- Calculate the pH at25°C of a 0.65M solution of potassium acetate KCH3CO2. Note that acetic acid HCH3CO2 is a weak acid with a pKa of4.76. Round your answer to 1 decimal place.Phosphoric acid (H3PO4) is tribasic, with pKa's of 2.14, 6.86, and 12.4. The charge of the ionic form of the conjugate base that predominates at pH 8 is _______ .Some H2PO4- and HPO42- are added to water such that the concentration of each is the same value, 5.25 mmol L-1 (pKa = 2.1, 6.8, 12.4). The water was initially at pH 6.55 and 25.0 °C. Calculate ΔGrxn in kJ mol-1. (R = 8.3145 J mol-1 K-1)
- A solution consisting of 1.14e-4 M H2S was found to be 2.78196 % ionized. What is the Ka? See reaction belowH2S(aq) + H2O ↔HS- + H3O+ 9.100e-8 3.180e-6 0.02782 1.833e-7(b) Calculate the pH of 0.0005 mol dm-3 ethanoic acid when its pKa = 4.75 and explain the assumptions made in the calculations CH3COOH(aq) à CH3COO-(aq) + H+(aq) Ka = pH = 3.1 (a) Define and write the expression of Kw for the dissociation of water (H2O). Kw is the ____________________ _____________ of _________________ Kw = (b) Calculate the pH of 0.1 mol dm-3 potassium hydroxide (KOH(aq)) pH = 10. Explain briefly the effect of temperature on Kw.Ethanoic acid is a weak acid pka value 4.74 at 298K. Calculate the pH value at 298K of: a 0.1M solution of ethanoic acid. a mixture of equal volumes of 0.1M solution of ethanoic acid and sodium ethanoate.
- An aqueous solution contains 0.132 mol L-1 of HCl and 0.717 mol L-1 of acetylsalicylic acid (Ka = 3.30×10-4). Determine the concentration of the conjugatebase of acetylsalicylic acid (i.e., acetylsalicylate).Give typed explanation not written Consider the following Ka values for phosphoric acid, H3PO4.Ka1 = 7.1 x 10-3Ka2 = 6.3 x 10-8Ka3 = 4.2 x 10-13a.) What is the pH of a 4.0 M solution of H3PO4? b.) Determine the effectiveness of H2PO4acting as a base by calculating its Kb. c.) What is the pH of a 4.0 M solution of Na3PO4 (not H3PO4)?A diprotic acid, H2A, has values of Ka1 = 1.0×10–5 and Ka2 = 1.0×10–10 at 25 ºC. In a 0.10 M aqueoussolution of H2A, what is the concentration of the anion A2– ?
- Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H The −CO2H functional group is still present but it’s acidity isreduced to Ka = 3.0 × 10^-4. What is the pH of a solution of acetylsalicylic acid with the concentration of 2.502?4 b) At pH 1.58, calculate the free [PO43-] when [PO43-]t = 22 mM. You can either solve 4 simultaneous equations to solve this problem for [H3PO4], [H2PO4-], [HPO42-] and [PO43-], or simply calculate the ratio of the two highest concentration species at the pH of the solution, and then calculate [PO43-] from those values. What are the two highest concentration species at pH 1.58?pH = 10.31 Use the following table to predict the best acid/ base pair for the desired pH/pOH values below (hint: remember buffer range = ± 1 pKa unit). Acid Base Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38