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)
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
Determine the pH of a 0.10 M CH3NH3Cl solution. (Kb (CH3NH2) = 4.4 x 10-4) 2.18 11.82 5.82 8.17 3.36
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
a.Determine the pH of a 0.20 M CH3NH3Cl solution. (Kb (CH3NH2) = 4.4 x 10-4) b. Determine what products are expected to be produced (a) at the cathode and (b) at the anode as a result of electrolysis of an aqueous solution of MgI2 with inert electrodes. The standard electrode potentials are: O2(g) + 4 H+(aq) + 4 e-→ 2 H2O(l) E° = +1.23 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V 2 H2O(l) + 2 e-...
Consider the titration of a 25.0 mL sample of 0.180 molL−1 CH3NH2 (Kb=4.4×10−4) with 0.155 molL−1 HBr. Determine the pH at 5.0 mL of added acid
0.082 L of 0.200 M HCl(aq) is combined with 0.0600 L of 0.400 M CH3NH2(aq). What is the pH of the resulting mixture? CH3NH2 has a Kb of 4.4 x 10-4. Enter your answer to 2 decimal places.
Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.250 M solution of methylamine?
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)...
What is the pH of a 0.650 M solution of methylamine (CH3NH2)? Kb=4.4x10-4
Determine the pH of a 0.35 M aqueous solution of CH3NH2 (methylamine). The Kb of methylamine is 4.4 × 10−4. can you please show your work and explain the steps on how you get 12.09 as the answer