Strychnince is a weak base with KB=1.6x10-6. The equilibrium for KB can be represented as below (where B stands for neutral molecules of strychnine). What is the OH- concentration in .090 M strychnin?
B(aq) + H2O <----> BH+(aq) + OH-(aq)
Strychnince is a weak base with KB=1.6x10-6. The equilibrium for KB can be represented as below...
The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent ionization....
codeine is a drug used in painkillers and is a weak
base with kb 1.6X10-6. calculate the ph of a 2.2X10-3M solution of
codeine. calculate % dissociation of codeine.
Question 1: Codeine (CiaH21 NO:) is a drug used in painkillers and is a weak base with a Kb value 1.6 x 106 1 solution of codeine (3 points) b) Calculate the % dissociation of codeine (2 points).
Model 2: A weak base increases the hydroxide concentration of a solution, but the amount of reaction is small. Na OH 圖B molecule ON BH+ ion H20 molecules are not shown H20 molecules are not shown A solution of a strong base, NaOH A solution of a weak base, B Critical Thinking Questions 7. How was the species BH produced in Model 2? 8. Complete and balance the following reaction equation for the weak base pyridine: CsH5N(aq) + H20(I) =...
Methylamine, CH3NH4, is a weak base. A 0.504 M solution of methylamine has equilibrium concentrations of both CH3NH3^+ and OH^- equal to 0.0150 M. What is the Kb of the base? CH3NH2(aq) + H2O(l) <> CH3NH3^+(aq) + OH^-(aq)
The base ionization constant Kb describes which of the following reactions for a weak base, B, in aqueous solution? OB(aq)+H*(aq) 5 BH*(24) B(aq) + H, 0*(aq) SBH*(aq) + H,00) B(aq)+ H,00) S BH(aq) + OH(aq) OB(aq) + OH"(aq) 5 BH"(aq) +0*- (aq) OBH*(aq) + OH"(aq) B(aq) + H20(1)
The weak base methylamine, CH3NH2, has Kb= 4.2x10^-4. CH3NH2 + H2O -> CH3NH3+ + OH- Calculate the equilibrium hydroxide ion concentration in a 0.95 M solution of the base. [OH-] = What are the pH and pOH of the solution?
(Set 2) Practice Problems in Equilibrium All weak acids use this generic equation: HA(aq)+ H2O() A (aq) + H30*(aq) And all weak bases use this one: B(aq)+ H2O(I) = BH*(aq)+ OH'(aq) Part A: Finding K, or Kb 3.012? What is the value of Ka for a weak acid if a 1.44 M solution has a pH 1. 2. A weak acid is 0.00987 M, but is found to be 25.5 % ionized. What is the pH? 3. The pH for...
a) If the Kb of a weak base is 4.8×10−6, what is the pH of a 0.46 M solution of this base? b)A certain weak base has a Kb of 8.90×10−7. What concentration of this base will produce a pH of 10.35?
Need Help on 1-6 please
1. Mercury ions exit as the mercurous dimer Hg22+ and Hgt. If Hg22+ is in contact with liquid mercury, Hg (1), the following equilibrium is established: Hgt(aq) → Hg22+(aq) + Hg(1) K= 2.24x10-5 If a 0.15 M solution of Hgt is put in contact with liquid mercury, what will be the resulting equilibrium concentration of Hg22+? Show work a. 3.36 x 10-6 M b. 1.83 x 10-3 M c. 1.14 x 10-2 M d. 0.83...
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What is the pH of a 0.128 M solution of the weak base B if AH° = -28.0 kJ and AS° = -175 J/K for the following equilibrium reaction at 25°C? B(aq) + H2O(1) 5 BH(aq) + OH (aq) pH =