1. Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5
(a) 5.137 (b) 4.367 (c) 9.633 (d) 8.781 (e) 8.863
2. A 0.1 M solution of which of the following willl have the highest pH?
(a) KCN, Ka of HCN = 4.0x10-10
(b) NH4NO3, Kb of NH3 = 1.8x10-5
(c) NaOAc, Ka of HOAc = 1.8x10-5
(d) NaClO, Ka of HClO = 3.2x10-8
(e) NaSH, Kb of SH1- = 1.8x10-7
please help me answer both questions. show work and explanation. thank you!
1. Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350...
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What is the pH of a solution which is prepared by dissolving .85 mol of NH3 and .30 mol of NH4CL in water to yield 1.00 L of solution? (The Kb is 1.77x10^-5)
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