Given aqueous solutions of 0.1 M weak acetic acid (CH3COOH, pKa=4.72) and 0.1 M sodium acetate (NaC2H3O2), calculate the volumes of acid and acetate to be mixed, in order to make 50mL of a buffer solution with pH=5.2.

One liter of buffer is made by dissolving 103.2 grams of acetic acid, HC₂H3O2, and 103.2 grams of sodium acetate, NaC₂H3O2, in enough water to make one liter. What is the pH of this solution? For acetic acid, HC2H3O2, K₂ = 1.8 x 105.

An aqueous solution contains 0.329 M methylamine (CH3NH2).How many mL of 0.305 M perchloric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.700.

A buffer solution contains 0.405 M NaHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide are added to 150. mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide) pH =

1.56 g of sodium acetate, NaCH;CO, has been 0.20 M ammonia, NH3, and 0.20 M ammonium 4. What is the pH of 0.15 M acetic acid to which 3. What is the pH of a solution that consists of aqueous solution of NH3? the same when you (c) add solid NaCl to a dilute aqueous solution of (b) add solid sodium acetate to a dilute a (a) add solid ammonium chloride to a dilute 1. Does the pH of the solution increase, decrease, or 17.1 and 17.2.) stay solution of acetic acid? aqueous NaOH? 2 Does the pH of the solution increase, decrease, or stay the same when you (a) add solid sodium oxalate, Na,C,O4, to 50.0 mL of 0.015 M oxalic acid, H,C,O4? (b) add solid ammonium chloride to 75 mL of 0.016 M HCl? (c) add 20.0 acetate, NaCH;CO2? of NaCl to 1.0 L of 0.10 M sodium *What is the pH of a solution that consists of chloride, NH4CI? added?

A 1.48 L buffer solution consists of 0.332 M propanoic acid and 0.178 M sodium propanoate. Calculate the pH of the solution following the addition of 0.062 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The ?a of propanoic acid is 1.34×10−5. PH =  A buffer with a pH of 4.22 contains 0.27 M of sodium benzoate and 0.26 M of benzoic acid. What is the concentration of [H3O+] in the solution after the addition of 0.056 mol HCl to a final volume of 1.6 L? Assume that any contribution of HCl to the volume is negligible. H3O+ =  (these are on the same slide on the homework)

buffer consists of 0.500 M acetic acid and 0.500 M sodium acetate. What is the pH if 0.100 mol ofKOH is added to 1.00 L of the buffer solution? Ka(HC2H3O2)=1.8×10−5

what is the pH of a buffer solution containing 0.100 M acetic and 0.050 M sodium acetate. The Ka for acetic acid is  1.82×10^-5:

Aspirin, or acetylsalicylic acid (CH3COC6H4CO2H; molar mass = 164.15 g/mol) has Ka= 3.0 x 10–4. If saturated solution of aspirin has pH = 2.68. Determine the solubility of aspirin in mol/L and in g/L

What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.