Calculate the pH of a .5M solution of the amino acid, aspargine, that was prepared from the form of asparganine that has a net -1 charge. Ka(-COOH) = 6.92x10^-3 and Ka(-NH3+)=1.86x10^-9 A. 4.52 B. 1.23 C. 5.45 D. 11.22 E. 7.93 F. 10.42
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Calculate the pH of a .5M solution of the amino acid, aspargine, that was prepared from the form of asparganine that has a net -1 charge. Ka(-COOH) = 6.92x10^-3 and Ka(-NH3+)=1.86x10^-9
A. 4.52
B. 1.23
C. 5.45
D. 11.22
E. 7.93
F. 10.42
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- 10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.Benzoic acid, HC7H5O2, and its salts are used as food preservatives. Ka for benzoic acid is 6,3 x 10–5. A solution of sodium benzoate, NaC7H5O2, in water has a concentration of 0,015 mol.dm–3. What is the pH of this solution?
- The amino acid asparagine has ionization constants Kal = 6.92 x 10-3 and K ₁2 = 6.92 x 10-3 and K₁2 = 1.86 x 10-9, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.170 M asparagine (HN) solution. pH =3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.5. a. Write an equation to show that HPo, (aq) can act as a Brønsted base in water. b. Label the species in (a) as acid, base, conjugate a cid and conjugate base respectively c. For the following equilibrium at 298 K, the equilibrium constant К- 2.84 х 10 2 М. Ag PO45) + H,O() = 3Agʻ(aq) + HPO, (aq) + OH (aq) Calculate the concentration of Ag in 0.10 M HPO. solution at pH 10.
- The base protonation constant K of morpholine (CH₂ONH) is 2.14 × 10¯6. Calculate the pH of a 0.41 M solution of morpholine at 25 °C. Round your answer to 1 decimal place. pH = 0 × Ś ?Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula C;H,N |1.7 × 10~9 4 hydrofluoric acid HF 6.8 × 10 pyridine 10 4.9 x 10 alo 4 hydrocyanic acid НCN ethylamine C2H,NH, | 6.4 × 10 Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the sofution t will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C2H5NH3B choose one 0.1 M C5H5NHCI choose one v 0.1 М KI choose one v 0.1 M KF choose oneIn the laboratory, a general chemistry student measured the pH of a 0.527 M aqueous solution of methylamine, CH3NH₂ to be 12.159. Use the information she obtained to determine the Kb for this base. Kb (experiment) = Show Transcribed Text In the laboratory, a general chemistry student measured the pH of a 0.524 M aqueous solution of pyridine, C,HSN to be 9.461. Use the information she obtained to determine the K, for this base. Kb (experiment) =
- Calculate the pH of a 0.12 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).Abbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2 in each of the following solutions: (a) 0.100 M H2M; (b) 0.100 M NaHM; (c) 0.100 M Na2M. For (b), use the approximation 3HM24 < 0.100 M.Use the References to access Im The pOH of an aqueous solution of 0.418 M quinoline (a weak base with the formula C₂ H7N) is (Assume that Kb (CH7N) = 6.30 × 10-¹⁰.) Submit Answer Retry Entire Group 9 more group attempts remaining