Given the mixture hydrazine is a weak base as it's Kb is very small and a strong acid HCl .First we have to calculate the number of moles of both weak base and strong acid .We see that the moles of acid is equals to moles of base hence we conclude that the there will be formation of salt as both acid and base are consume in equal amount. Therefore salt form undergo equilibrium with hydrazine and proton form. So we have to find the concentration of salt as we have 0.05 moles and total volume 200 mL.Then we consider let 'x' moles of salt dissociates at equilibrium to give x moles of proton and x moles of hydrazine. We use the Ka (7.7 *10-9 from literature)value for salt (i.e is a weak acid type) and solve the equation to have x .We assume that x is very very small than the initial concentration of acid and ignore it.Then after calculating x we have concentration of proton and crossponding pH. So the pH calculated is less than 7.Therefore B is the correct option
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Hydrazine (NH2NH2) has a Kb = 3.0 x 10-6. If 100.0 mL of a 0.5000 M...
1. The weak base hydrazine, N2H4, has a Kb = 1.7 x 10-6. What is the percent ionization of a 0.15 M solution? 2. Hydrofluoric Acid has a Ka of 6.8 x 10-4. Calculate the [H+] in 0.25 M HF: 3. What is the pH of a 0.050 M solution of Acetic Acid, HC2H3O2? 4. A solution has a pOH of 10.25. Calculate the [H+].
You are charged to perform a titration with 20 mL of 1.0 M hydrazine (KB = 1.7x10-6) as analyte and 0.5 M HBr as titrant. What is the initial pH of the solution? pH = At what volume would you reach the stoichiometric point? stoichiometric point = mL At what volume would pH = pka? pH = pka @ ml What is the pH at the stoichiometric point? pH @ stoichiometric point =
(1) Given the following information: hydrocyanic acid HCN Ka = 4.0×10-10 diethylamine (C2H5)2NH Kb = 6.9×10-4 (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium will the reactants or products be favored? (3) Will the pH of the resulting solution be greater than, less than, or roughly equal to 7?...
NEED HELP ASAP Hydrazine, N2H4, has Kb = 1.3E-6. Calculate the pH of a 0.236 M solution of N2H4.
Consider the titration of 100.0 mL of 0.200 M acetic acid ( Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a 0.0 mL pH= 50.0 mL pH = C 100.0 mL pH = 140.0 mL pH= C 200.0 mL pH = f 240.0 mL pH=
Rolerences Consider the titration of 100.0 mL of 0.200 M acetic acid K = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL pH = b. 50.0 mL pH = c. 100.0 mL pH = d. 130.0 mL pH = e. 200.0 mL pH = f. 210.0 mL pH = Submit Answer TEY Another Version 6 ltem attempts remaining.
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
If 20.9 mL of 0.071 M hydrochloric acid (HCI) solution is added to 21 mL of 0.132 M ammonia (NH3) solution, what is the pH value of the mixed solution at 25°C? (Kb for NH3 = 1.8 x 10-5); Please keep your answer to two decimal place x.xx.
You have 15.00 mL of a 0.100 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
You have 25.00 mL of a 0.100 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...