4. What is the pH of a 0.0442 M solution of methylamine if enough hydrochloric acid is added to bring the chloride concentration to 0.0442? pKb = 3.19
4. What is the pH of a 0.0442 M solution of methylamine if enough hydrochloric acid...
1. What is the pH of a 0.0442 M solution of methylamine if enough hydrochloric acid is added to bring the chloride concentration to 0.0442? 2. What is the Ka value if a 0.0350M solution of an unknown weak acid yields a pH of 5.34?
If the a mixture of methylamine (CH3NH2, pkb = 3.32) in water produces a pH of 11.2, what is the initial molar concentration of methylamine in the solution? O A 5.2x10-3M O B 2.5x10-3M O C 1.3x10-2M O D 5.6x10 M Unanswered Submit Initial Concentration C Homework Unanswered What is the initial molar concentration of a solution of hydrochloric acid (HCI) with a pH = 1.92
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine, CH3NH2, with 25.00 mL of 0.10 M methylammonium chloride, CH3NH3C1? Assume that the volume of the solutions are additive and that Kb = 3.70 times 10-4 for methylamine. 10.27 10.57 10.87 11.78 Which statement about buffers is true? Buffers have a pH = 7. Buffers consist of a strong acid and its conjugate base. A buffer does not change pH on addition of a...
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
An aqueous solution contains 0.380 M methylamine (CH3NH2). How many mL of 0.211 M hydrochloric acid would have to be added to 250 mL of this solution in order to prepare a buffer with a pH of 10.800. mL -------------
What is the pH of a 0.14 M solution of methylammonium chloride, CH NH, CI? What is the concentration of methylamine in the solution? Ks (methylamine) - 4.4 x 10-4 pH- Concentration =
Post Lab Activity Acids, Bases, pH, and Buffers 1. Calculate the pH of a 0.08 M NaOH solution. 2. Hydrochloric acid is a strong acid and dissociate almost 100% in aqueous solution. If two drops (0.1 mL) of 1.0 MHCI are added to pure water to make 1.0 L solution. What is the pH of this solution? 3. M. What will be the A dilute solution of hydrochloric acid (HCI) has a concentration of 0.1 pH of this solution? 4....
A 22.8 mL sample of 0.218 M methylamine, CH3NH2, is titrated with 0.393 M hydrochloric acid. After adding 4.64 mL of hydrochloric acid, the pH is .
what is the pH of 0.36M methylamine solution? pH of 0.36 M methylamine sol. (Kb = 4.4 * 10^-4)
2) What is the effect on the solution pH when 2.00 mL 1.00 M hydrochloric acid is added to 250.0 mL of 0.0500 M sodium acetate/acetic acid buffer pH 4.01? Note: acetic acid K, is 1.8 x105.