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Ethylamine, CH3CH2NH2, is an organic base with pKb = 3.367 at 298 K. In an experiment, a 40.0 mL sample of 0.105 mol L?1 CH3CH2NH2 (aq) is titrated with 0.150 mol L?1 HI(aq) solution at 298 K. (1a) Write a balanced chemical equation for the neutralization reaction upon which this titration is based, and indicate clearly which atom is being protonated. Then, calculate the equilibrium constant for the neutralization reaction. (Hint: To calculate the equilibrium constant, you may find it helpful to represent the neutralization reaction as the sum of two separate reactions.) (1b) Calculate the pH, [CH3CH2NH2], and [CH3CH2NH3+] at the following stages of the titration. i) before the addition of any HI solution. ii) after the addition of 20.0 mL of HI solution. iii) at the equivalence point. iv) after the addition of 60.0 mL of HI solution.
Calculate the partial pressures of CO2 and CO at equilibrium if 5.0 g of CO2 are introduced into a 10.0 L container and heated to 1200 K in the presence of 1.50 g of graphite (C (s)).
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Equilibrium constant from standard potential data, Calculate the equilibrium constants of the following reactions at 25°C from standard potential data
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Which of the following elements will have the same number of core electrons as P?
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Provide a structure for the following compound: C9H10O3; IR: 2400-3200, 1700, 1630 cm-1; 1H NMR: ? 1.53 (3H, t, J = 8 Hz); ? 4.32 (2H, q, J = 8 Hz); ? 7.08, ? 8.13 (4H, pair of leaning doublets, J = 10 Hz); ? 10 (1H, broad, disappears with D2O sha..
A solution is made by adding 0.51 mol of lithium hydroxide (LiOH) in enough water to form 5 L of solution. Calculate the pH.
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