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4. Calculate the pH of a solution with 2.5 x 103 mol CsHsN and 1.2 x 10-mol HCl in 100 mL. The Kb for pyridine is 1...
A 250.0 mL solution contains two weak bases, pyridine (Kb = 1.7 x 10^-9) and caffeine (Kb = 4.1 x 10^-4). This solution contains 1.00 x 10^-3 mol of each of the bases. What's the pH of this solution?
Calculate the pH of a 0.20 M solution of the weak base pyridine. (C5H5N; Kb = 1.7 x 10-9). What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 ´ 10–5]
35. What is the pH for a 0.80M HCSH5NCI solution? Kb for CsHsN is 1.7 x 10 Fnd ka SN 36, What is the pH for a 0.050 M Sodium Benzoate (NaCHsO2) solution? Ka for HC7H502 is 6.4 x 10 weat /st
1. A hydrogen atom in the organic base pyridine, CsHsN, can be substituted by various atoms or groups to give XCsH4N, where X is an atom such as Cl or a group such as CH3. The following table gives K, values for the conjugate acids of a variety of substituted pyridines. Atom or Group X (aq) + HCl(aq) → (aq) + Cl-(aq) NO K, of Conjugate Acid 5.9 x 10-2 1.5 x 10-4 6.8 x 10-6 1.0 x 10-6 н....
16 What is the pH of a 1.63 M solution of pyridine (C5H5N; Kb = 1.7 x 10-9)? [ (4 Puan) 9.72 10.07 9.07 5.23 8.77
Pyridine is a weak base with a Kb=1.7 x 10^-9. If 0.300 moles of pyridine is added to 1.00 L of water, what will be the equilibrium concentrations of the species below? a. [Pyridine] b.[Pyridine-H+] (the Pyridium ion) c.[OH-] 2. what is the pH of the solution in problem 4 above?
You have a 0.776 M solution of the base pyridine. Kb = 1.7 x 10" Find the pH of the pyridine solution. Round your answer to two places past the decimal. Type your answer...
Calculate the pH and pOH of 1.2 x 10-3 M HCl solution. Calculate pH, pOH and [OH-] of 0.1 M HNO3 solution. If a solution X has pH = 5, which of the following is true: Solution X is neutral. H3O+ ion concentration is higher than OH- concentration. c. OH- ion concentration is higher than H3O+ concentration.
Calculate the pH of a solution containing 2.5 x 10– 2 mol of nicotinic acid (a monoprotic acid) dissolved in 350 mL of water. ( Ka = 1.1 x 10- 5). The answer is 3.05. Please Help
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...