28. 25.00 mL of a solution of a weak monoprotic acid, HX, was titrated with a 0.0640 M solution of NaOH, requiring 18.22 mL to neutralize the acid. If the Ka for the acid is 3.60*10-6, calculate the number of moles of a salt, NaX, that must be added to produce a pH of 6.00 in 150.00 mL of the original solution. You may assume that the temperature is 25 °C. It is impossible for a solution with this composition to have a pH of 6.00 0.00117 mol 0.0252 mol 0.0466 mol O 1.17 mol

An analytical chemist is titrating 243.8 mL of a 0.7000 M solution of butanoic acid (HC3H,CO2) with a 0.3800 M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 278.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH ☐ olo Ar

1 L buffer containing 0.75 M formic acid ( HCOOH) and 0.25 M sodium formate ( HCOONa) was prepared . pka of formic acid is 3.75. Calculate the pH of the buffer when (a) when 40 mL 5 M HCI was added to the buffer (b) when 40 mL 5 M NaOH was added to the buffer

Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 2.34? Group of answer choices HClO2, Ka = 1.1 × 10-2 HIO, Ka = 2.3 × 10-10 HCN, Ka = 4.9 × 10-10 C6H5OH, Ka = 1.3 × 10-10 HN3, Ka = 2.5 × 10-5

Suppose you have an alkaline buffer consisting of 0.20 M aqueous ammonia (NHs) and 0.10 M ammonium chloride (NH4CI). What is the pH of the solution? 5 Calculate the pH of a 0.350 M solution of potassium phenolate, KC6H5O. Ka for phenol (CH5OH) is 1.0 x 10-10. How do the concentration/volumes of the buffer affect the buffer capacity? E.g., 50.0 mL of 0.10 M acetic acid solution with 50.0 mL of 0.10 M sodium acetate solution vs. the buffer you made in the lab (25.0 mL of 0.10 M acetic acid solution with 25.0 mL of 0.10 M sodium acetate solution).

When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 19.1 mL of barium hydroxide have been added?

How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.396 M hypobromous acid, HBrO, to form a buffer solution of pH 8.95? The Ka of HOBr is 2.0 × 10–9. Express your answer in moles using at least three significant figures. Do not use scientific notation.

When a 20.1 mL sample of a 0.367 M aqueous hydrocyanic acid solution is titrated with a 0.492 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 11.2 mL of barium hydroxide have been added?

-2 A chemistry graduate student is given 100. mL of a 0.80M chlorous acid (HCIO,) solution. Chlorous acid is a weak acid with K,=1.1 × 10 ´. What mass of KCIO, should the student dissolve in the HCIO, solution to turn it into a buffer with pH = 1.37? You may assume that the volume of the solution doesn't change when the KC10, is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10

(a) Calculate the pH of a 0.500 L buffer solution composed of 0.700 M formic acid (HCOOH, Ka = 1.77 x 10-4) and 0.500 M sodium formate (HCOONa). (b) Calculate the pH after adding 50.0 mL of a 1.00 M NaOH solution.