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Methylaime, CH3NH2. If a 0.100

Methylaime, CH3NH2.If a 0.100 mol/L solution of methyamine has a pH of 11.80, calculate the ionization constant for the weak
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2. asked by Lena
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What ratio [CH3NH3+]/[CH3NH2] is needed to prepare a buffer solution with a pH of 8.60 from methylamine, CH3NH2, and
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2. asked by Kasey
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Solve an equilibrium problem (using an ICE table) to calculate the pH.a solution that is 0.205 M in CH3NH2 and 0.110 M in
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2. asked by Kyle
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Find the pH of a buffer that consists of 0.82 M methylamin (CH3NH2) and 0.71 M CH3NH3Cl (pKb of methylamine (CH3NH2) = 3.35.)I
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2. asked by Edward
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At 298k the base dissociating constant Kb of CH3NH2 is 4.5×10mol/dmWrite an expression for the kb of CH3NH2
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2. asked by Esther
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Suppose that 50.0 mL of 0.25 M CH3NH2(aq) is titrated with 0.35 M HCl(aq).(a) What is the initial pH of the 0.25 M CH3NH2(aq)?
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2. asked by Dana
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Determine pH of each solution:b) 0.20 M CH3NH3I I did.... CH3NH3^+ +H2O -> CH3NH2 + H3O^+ 0.20 ---------------0--------------0
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2. asked by ALISON
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What will the pH be if 15 mL of 0.1 M HCl are added to the buffer obtained by mixing 70 mL of 0.5 M CH3NH2 and 30 mL of 1.0 M
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2. asked by Maria
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I'm trying do this question:0.10 mol/L hydrochloric acid is titrated with 0.10 mol/L methylamine, CH3NH2. Calculate the pH of
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2. asked by a Canadian
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In one experiment, 50.0ml of 0.10M CH3NH2, is mixed with 20.00ml of 0.10 M CH3NH3Cl. The kb of CH3NH2 is 3.70*10^-4.a) write the
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2. asked by James
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