Determine the pK b for the base B given that the equilibrium concentrations are [B]=2.64 M , [ HB + ]=1.5 M , and [ OH − ]=1.2 M .
Determine the pK b for the base B given that the equilibrium concentrations are [B]=2.64 M...
Determine the pKb for the base B given that the equilibrium concentrations are [B]=1.5 M, [HB+]=0.87 M, and [OH−]=0.75 M. Report your answer with two decimal places.
Determine the equilibrium concentration of the base C5H5N given that pKb=8.77 and the equilibrium concentrations of OH− and C5H5NH+ are 0.0032 M, and 4.9×10^−6 M respectively. Report your answer with two significant figures.
Determine the equilibrium concentration of the base NH3 given that pKb=4.76 and the equilibrium concentrations of OH− and NH+4 are 6.5×10−5 M, and 0.42 M respectively. Report your answer with two significant figures.
Determine the equilibrium concentration of the base HS− given that Kb=1.0×10−7 and the equilibrium concentrations of OH− and H2S are 6.0×10−4 M, and 4.4×10−7 M respectively.
A hypothetical weak base has Kg = 5.0 x 108. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB]= mol/L [OH-] = pH = Submit Show Approach Show Tutor Steps Submit Answer Try Another Version 10 item attempts remaining
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)
When dealing with buffer systems, we often use the acid reaction to determine the equilibrium and set up the ICE table. The most common experimental method used to study acid-base systems is titration, which studies the stoichiometric addition of the acid to a base solution or the base to an acid solution to determine the value of K, or K, The value of the pK, or pK, is essential to the understanding of the buffer system, where pK, = -log...
5) Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [NO2]eq = 0.85 M and [NO]eq=0.38 M. 2 NO2(g) - N2048) A) 2.2 B) 1.9 C) 0.022 D) 0.22 E) 0.53 6) Which of the following statements is true? A) If Q=K, it means the reaction is not at equilibrium. B) If Q<K, it means the forward reaction will proceed to the right) to form more reactants. C) IFO <K, it means the...
Consider the reaction and the associated equilibrium constant. Determine the equilibrium concentrations of A and B. Assume the initial concentration of A = 1.0 M and that no B is present at the beginning of the reaction, since B is the product. A(g) ⇌ B(g) Kc = 4.0 Group of answer choices A [A] = 0.2 M; [B] = 0.8 M B [A] = 0.4 M; [B] = 0.1 M C [A] = 1. M; [B] = 4. M D [A]...
Question 15 1 pts Given equilibrium concentrations of A = 0.138 M; B = 0.154 M and C = 0.071 M at 308 K, calculate AGºrxn for the following reaction in kj. Enter the result to 2 decimal places and no units. 2A + 1B → 2C