mixture of amine and its salt act as basic buffer
pOH = pKb + log [CH3NH3+] / [CH3NH2]
pKb = - log Kb = - log [4.4 x 10-4] = 3.36
pH = 10.00
pOH = 14 - 10.00
pOH = 4.00
4.00 = 3.36 + log [CH3NH3+] / [CH3NH2]
log [CH3NH3+] / [CH3NH2] = 0.64
[CH3NH3+] / [CH3NH2] = 4.36
[CH3NH2] / [CH3NH3+] = 0.23
What ratio of CH3NH2 to CH3NH3* is needed to prepare a pH 10.00 buffer? (Kb for...
answer is 3.70
What concentration ratio of acid to base, [CH3NH3*]/[CH3NH2], would be needed to make a buffer with a pH 10.00? Kb for CH3NH2 is 3.7x 104
Calculate the PH and concentrations of CH3NH2 and CH3NH3+ in a
0.0445M Methylamine (CH3NH2)
Calculate the pH and concentrations of CH3NH2 and CH3NH3 in a 0.0445 M methylamine (CH3NH2) solution. The Kb of CH3NH2-4.47 x10 Number pH11.520 Number CH,NH0.0409 Number CH, NH, |-| | 0.00446
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?
What is the pH of a 0.200 M CH3NH2 solution? (Kb for CH3NH2 = 4.4 x 10-4) 2.03 11.97 9.33 8.79
Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. Calculate the pH of a 1.40 M CH3NH3Cl solution. Kb for methylamine, CH3NH2, is 4.4 × 10-4. 1.61 8.75 5.25 12.39
What is the pH of a solution of 0.400 M CH3NH2 containing 0.180 M CH3NH31? (Kb of CH3NH2 is 4.4 x 10-4)
A) Calculate the pH of a 0.0116 M aqueous solution of methylamine (CH3NH2, Kb = 4.2×10-4) and the equilibrium concentrations of the weak base and its conjugate acid. pH = ? [CH3NH2]equilibrium = ? M [CH3NH3+ ]equilibrium = ? M B)Calculate the pH of a 0.0115 M aqueous solution of nitrous acid (HNO2, Ka= 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = ? [HNO2]equilibrium = ? M [NO2- ]equilibrium = ? M C)...
> Click Submit to complete this assessment. Question 22 Calculate the ratio of CH3NH2 to CH3NH3Cl concentration required to create a buffer with pH of 10.24. Kb (CH3NH2) = 4.4 x 10-4 OA 0.40 08.16 Oc.0.39 Oolo O E 0.96 > Click Submit to complete this assessment.
Consider a buffer solution which consists of methyl amine (CH3NH2) and methyl ammonium chloride (CH3NH3Cl). At what pH is this buffer solution most effective? (Kb = 4.4⋅10−4 for methyl amine)
Question 7 of 9 How many moles of CH3NH3Cl need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for CH3NH2 is 4.4 * 10-4) to make a buffer with a pH of 11.60? mol C +/- 0 x 100