250.0 M acetic acid and 0.250 M in sodium acetate. What is the initial pH of this solution? What is the PH after the addition of 0.005 mol of HCI ?

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If 0.10 M Acetic acid + 0.10 M sodium acetate at a final volume of 50 ml was prepared? what is the theoretical pH of the solution? The Ka for acetic acid is 1.8 * 10^-5. What would be the theoretical pH after adding 1ml of 1M HCl to the above solution?

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.

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

A solution is prepared that is initially 0.13M in acetic acid (HCH3CO₂) and 0.24M in potassium acetate (KCH3CO₂). 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 initial change final [HCH,CO₂] 0 [H₂0]. You can leave out the M symbol for molarity. [cH,co,] 0 L [H₂O] 0 0 0 plo X G

A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of propanoic acid (HPr, K«= 1.3 x 105). Assume the volume of the solution to be 1.0 L. a) Write the chemical equation for the acid hydrolysis reaction. | b) What is the acid-base conjugate pair that governs the pH of the buffer? c) Calculate the pH of the buffer. Be sure to justify and validate any approximations used.

An aqueous solution contains 0.302 M ammonia (NH3). How many mL of 0.393 M perchloric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 9.240? mL

If 4.5 moles of nitric acid falls into 8000 L of pure water, what will be the change of the pH of the solution? (Note that nitric acid dissociates completely and puts in one hydrogen ion for each molecule of nitric acid)

Calculate the pH for each of the cases in the titration of 35.0 mL of 0.240 M KOH(aq) with 0.240 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCl: after addition of 13.5 mL HCl: after addition of 21.5 mL HCl: after addition of 35.0 mL HCl: after addition of 41.5 mL HCl: after addition of 50.0 mL HCl: