The hydroxide ion concentration, [OH-], of an aqueous solution of 0.463 M methylamine (a weak base with the formula CH3NH2)
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The hydronium ion concentration of an aqueous solution of 0.538 M methylamine (a weak base with the formula CH3NH2) is [H3O+] = ________ M
The weak base methylamine, CH3NH2, has Kb = 4.2 ×10−4. It reacts with water according to the equation.
CH3NH2 (aq) + H2O (l) ⇌ CH3NH3+ (aq) + OH− (aq)
Calculate the equilibrium hydroxide ion concentration in a 0.25 M solution of the base. What are the pH and pOH of the solution?
1. A buffer solution contains 0.393 M CH3NH3Br and 0.463 M CH3NH2 (methylamine). Determine the pH change when 0.095 mol HNO3 is added to 1.00 L of the buffer. pH after addition â pH before addition = pH change =
2. An aqueous solution contains 0.346 M nitrous acid. How many mL of 0.318 M potassium hydroxide would have to be added to 125 mL of this solution in order to prepare a buffer with a pH of 3.160?