12. Calculating pH of a buffer. a) A solution is prepared that is initially 0.44M in...
13. Calculating the composition of a buffer of a given pH. a) Kb=5.4*10-4 125mL of 0.90M (CH3)2NH Calculate the mass of (CH3)2NH2Br should the student dissolve in the (CH3)2NH solution to turn into a buffer with pH=10.70. MW-125.9956g/mol b) Ka=4.5*10-4 125mL of 1.40M HNO2 solution Calculate the mass of KNO2 should the student dissolve in the HNO2 solution to turn into a buffer with pH=3.30
Can anyone help me with this question? Calculate the pH of a buffer solution of a .050M nitrous acid (HNO2, Ka = 4.5x10-4) and .1M KNO2.
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 Kb for methylamine, CH3NH2, if a solution prepared by dissolved 0.82 mol of methylamine in 425 mL of H2O has a pH of 12.46? (Ans: 4.4 x 10-4) A 0.100 M solution of formic acid, HCOOH, is 4.0% dissociated. Calculate Ka for formic acid. (Ans: 1.7 x 10-4)
Post-Lab Assignment: pH and Buffers 1. A buffer is prepared from a weak acid with a Ka - 7.1 x 104 and its conjugate base. a. What pH would provide maximum buffer capacity? b. What would be the buffer range for this acid? (Your answer should show the lowest and the highest pH that would provide a reasonably effective buffer.) 2. If you were provided with a 0.1 M solution of an unknown weak acid and a 0.1 M solution...
The following shows a list of weak acids and bases with their Ka and Kb values. Substances Ka Substances Kb Cyanic acid (HCN) 4.9 x 10-10 Ammonia (NH3) 1.8 x 10-5 Nitrous acid (HNO2) 4.5 x 10-4 Aniline (C6H5NH2) 4.3 x 10-10 Hydrofluoric acid (HF) 6.8 x 10-4 Pyridine (C5H5N) 1.7 x 10-9 Acetic acid (CH3COOH) 1.8 x 10-5 Methylamine (CH3NH2) 4.4 x 10-4 If you want to make a pH 8.0 buffer solution, which of the following acids or...
Rank the following solutions in order of increasing pH. Consider the following data on some weak acids and weak bases: - Ka Ko acid name formula nitrous acid HNO2 4.5*10-4 base name formula methylamine CH3NH2 4.4 x 10-4 acetic acid HCH,CO2 1.8 x 10-5 aniline CH3NH2 4.3 * 10-10 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the so the solution that will have the next lowest...
What is the pH of a 0.180 M aqueous solution of potassium nitrite, KNO2 at 25 °C? (Ka for HNO2 = 4.5×10-4)
What is the pH of a buffer solution containing 0.13 M HF and 5.0×10−2 M NaF? What is the pH of a buffer solution containing 1.0×10−2 M HF and 0.16 M NaF? Using the table given below for Ka values, compare the pH of an HF buffer that contains 0.13 MHF and 5.0x10-2 M NaF with another HF buffer that contains 1.0x10-2 MHF and 0.16 M NaF. Ka and K b values for selected weak acids and bases HF Acid...
Be sure to answer all parts. What is the [H3O+] and the pH of a buffer that consists of 0.54 M HNO2 and 0.74 M KNO2? (Ka of HNO2 = 7.1 × 10−4)