A weak base, ammonia, is to be titrated with hydrochloric acid. A volume of 30.0 mL of the 0.75 M NH3 (weak base) whose Kb = 5.25 x10^-6 is titrated with 0.96 M HCl (strong monoprotic acid). Assuming that the stoichiometry for this neutralization titration is 1:1 , calculate the ff: A. pH of the resulting solution when the volume of the added strong acid titrant neutralizes 70% of the analyte. B. pH of the resulting solution at the equivalence point. C. pH of the resulting solution at 5.0 ml added titrant beyond the equivalence point.

Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.

Calculate the pH for each of the cases in the titration of 25.0 mL of 1.50 M pyridine, C5H5N(aq) with 0.500 M HBr(aq) at 25°C. The Kb of pyridine is 1.7×10−9. Report all your answers to 2 decimal places. Record the bold and underlined values to the empty spaces in your handout. Before the addition of any HBr: Question Blank 1 of 5 After the addition of 10.0 mL of HBr: Question Blank 2 of 5 After the addition of 37.5 mL of HBr: Question Blank 3 of 5 After the addition of 75.0 mL of HBr: Question Blank 4 of 5 After the addition of 85.0 mL of HBr: Question Blank 5 of 5

Twenty millimeters of 0.50N HOAc is diluted with water to 100mL, and the resulting solution is titrated with 0.50N HOAc. Calculate the pH value (a) at the start, (b) when 0.8 ml of the NaOH has been added, (c) at the equivalence point (when 20mL of NaOH has been added, (d) when 30mL of the NaOH has been added. Ka=1.8x10^-5

in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.

A solution is prepared that is initially 0.26M in hydrofluoric acid (HF) and 0.25M in potassium fluoride (KF). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O*]. You can leave out the M symbol for molarity. initial change final [HF] 0 П [F] 0 0 0 [H₂O*] 0 0 0 X

Near the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.

A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? 227 g/mol 82.5 g/mol 371 g/mol 124 g/mol 186 g/mol

Please don't provide handwritten solution ....

What is the approximate pH at the equivalence point of a weak base-strong acid titration if 50.00 mL of aqueous ammonia (NH3) requires 37.10 mL of 0.1087 mol L-1 HCI? pK₁ =4.75 for ammonia. Report your answer in 2 decimal places.