The pH of a 0.170 mM solution of the alkaloid quinine is 9.25.
Determine Kb for quinine from these data. (Assume Kw =
1.01 ✕ 10−14.)
C20H24N2O2(aq) + H2O(l) equilibrium reaction arrow HC20H24N2O2+(aq)
+ OH −(aq)
The pH of a 0.170 mM solution of the alkaloid quinine is 9.25. Determine Kb for...
The pH of a 0.135 mM solution of the alkaloid emetine is 9.24. Determine Kb for emetine from these data. (Assume Kw = 1.01 ✕ 10−14.) C29H40N2O4(aq) + H2O(l) HC29H40N2O4+(aq) + OH−(aq)
Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pKb1 = 5.1 and pKb2 = 9.7 (pKb = −log(Kb)). Only 1.0 g of quinine will dissolve in 1900.0 mL of water. Calculate the pH of saturated aqueous solution of quinine. Consider only the reaction Q + H2O equilibrium reaction arrow QH + + OH − described by pKb1, where Q = quinine.
Quinine (C20H24N2O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pKb1 = 5.1 and pKb2 = 9.7 (pKb = −log(Kb)). Only 1.0 g of quinine will dissolve in 1900.0 mL of water. Calculate the pH of saturated aqueous solution of quinine. Consider only the reaction Q + H2O equilibrium reaction arrow QH + + OH − described by pKb1, where Q = quinine.
The pH of a 0.145 mM solution of the alkaloid papaverine is 8.27. Determine K for papaverine from these data. (Assume Kw 1.01x10-14.) 20214 20 214
Quinine (C2H2N,O,) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine pk. = 5.1 and PK 1900.0 mL of water. Calculate the pH of saturated aqueous solution of quinine. Consider only the reaction Q + H,0 = QH+ + OH- described by = 9.7 (pKb = -log(K)). Only 1.0 g of quinine will dissolve in here Q = quinine.
QUESTION 10 What is the pH of a 0.30 M pyridine solution that has a Kb = 1.9 x 10-97 The equation for the dissociation of pyridine is CsH5N(aq) + H2O(1 =C5H5NH+ (aq) + OH" (aq). Kw = 1.0 x 10-14 10.38 4.62 9.38 8.72
In aqueous solution, the azide ion, N3−, is a weak base that accepts a proton from water to form the hydroxide ion, OH −, and hydrazoic acid, HN3, according to the following equation. N3−(aq) + H2O(l) equilibrium reaction arrow OH −(aq) + HN3(aq) The base-dissociation constant (Kb) for this base is 4.04 ✕ 10−10. If a 0.082 M solution of azide ions is prepared, what is the final pH of the solution? (Assume that the temperature is 25°C.)
This question pertains to the pH of a weak acid/weak base salt combo. For an aq solution of NH4NO2, these are the combinations of reactions that are possible. (1) NH4+(aq) + NO21-(aq) ⇆ NH3(aq) + HNO2(aq)____________K1 = ? (2) NH4+(aq) + H2O(l) ⇆ H3O+(aq) + NH3(aq)_______________Ka = 5.6 x 10-10 (3) NO21- + H2O(l) ⇆ HNO2(aq) + OH-(aq)_________________Kb = 2.2 x 10-11 (4) 2H2O(l) ⇆ H3O+(aq) + OH-(aq)_________________________Kw =1.0 x 10-14 Write the symbolic expression for the equilibrium constants...
Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below: Determine the ammonia concentration of an aqueous solution that has a pH of 11.30. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below: a)9.0 × 10-3 mol L-1 b)2.7 mol L-1 c)0.22 mol L-1 d)2.0 × 10-3 mol L-1 NH3(aq) + H20(1) = NH4+(aq) + OH-(aq) NH3(aq)...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...