Calculate the pH of a 25.2 mM solution of methylamine. Please show steps and explain thank...
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
Calculate pH of a weak base solution. Please box answers! Thank you! Close Problem Tutored Practice Problem 16.4.6 cm STOWARRANTIE Calculate the pH of a weak base solution (quadratic equation). Calculate the pH of a 0.0304 M aqueous solution of methylamine (CHANH. K. - 4.2x10*) and the equilibrium concentrations of the weak base and its conjugate acid PH [CH3NH2lequilibrium [CH3NH3 Jequilibrium - Check & Submnt Answer Show Approach
What is the pH of a 0.10M solution of methylamine (:NH2CH3) From Table 15.8, Kb = 4.4 x 10-4. Please show me how to work it out, thank you!
Please show all work. Thank you. Calculate the pH of a 0.10 M solution of sodium acetate NaC_2H_3O_2.
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
please help with these questions ! 2. Show how methylamine, CH,NH2 dissociates in solution and calculate the pH of a 0.25 M aqueous solution of the substance. Kb for CH,NH, is 1.8 x 10-4 3. Write a balanced equation to show how the following ions hydrolyze in water and write the acid or base dissociation constant for each: b) Al3 d0 HCO a) CN CH,СО, c) CO22 d)
please explain your answer 3. An aqueous solution of 0.204 M methylamine, CH3NH2, is hydrochloric acid, HCL. The base ionization constant for methylamine is 4.4 x 10-1. What is the pH of the mixture when 12.50 ml of the methylamine solution has been delivered by the buret? added by buret to 25.00 mL of 0.102 M 50 grade paints] SHOW YOUR WORK AND/OR REASONING
please explain If the a mixture of methylamine in water produces a pH of 11.2, what is the concentration of methylamine in the solution? HOC-NH2 + HO Hoc Noth methenemine methylumine) methylammonium ion pk, 10.7 O A 5x10-3M o B 2.5x 10-3M O C 1210-2M O 5x10 M
please show steps 16.36 Calculate the pH of an aqueous solution at 25°C that is (a) 0.12 M in HCI, (b) 2.4 M in HNO3, and (c) 3.2 X 10 M in HCIO4 16.54 Calculate the pH of an aqueous solution at 25°C that is 0.34 M in phenol (CH5OH). (K, for phenol - 1.3 x 1010 The pH of an aqueous acid solution is 6.20 at 25°C. Calculate the K, for the acid. The initial acid 16.60 concentration is...
Enter your answer in the provided box. Calculate the pH of a 0.25 M methylamine solution. pH =