500ml of 2M Tris-HCl buffer pH 8.9. Tris base MW is 121.14 g/mol. Please describe the preparation procedure for the desired Tris buffer and list the materials needed.

What is the pH of a buffer prepared by combining 0.461 moles of  HC2H3O2 with 0.486 moles of NaC2H3O2  in 531 mL of solution?

Be sure to answer all parts. Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 30.00 mL pH = (b) 39.40 mL pH = (c) 55.00 mL pH =

A buffer is created by mixing 600 mL solution of acid HA (0.500 M) with 700 mL of conjugate base A- (0.800M). acid HA has the acid dissociation constant of 9.20 x 10-5 Determine the pH of the mixture

A)What is the pH of a buffer prepared by adding 0.506 molmol of the weak acid HAHA to 0.507 molmol of NaANaA in 2.00 LL of solution? The dissociation constant KaKa of HAHAis 5.66×10−75.66×10−7. b)What is the pHpH after 0.150 molmol of HClHCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. c).What is the pHpH after 0.195 molmol of NaOHNaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.

14- Triethylammonium chloride (22.00g, (C2H5);NHCI, 137.65 g/mol) is added to water to make 1.75 L of solution. (Hint: (C2H5);NH* is the conjugate acid of the weak base triethylamine, (C2H5);N, pKs = 4.19). A buffer is prepared by mixing 25.00 mL of the previous solution with 25.00 mL of 0.0750 M sodium hydroxide. Determine the pH of the resulting buffer. 15- A buffer is prepared using 0.180 mol of dihydrogenphosphate ions and 0.120 mol of hydrogenphosphate ions in 250.0 mL volumetric flask. a- Calculate the pH of the prepared buffer.

What is the pH of a buffer solution made by mixing 50.0 ml of 0.100M potassium hydrogen phthalate with 13.6 ml of 0.100 M NaOH and diuting the miture to 100.0 ml, with water? The Kaz for hydrogen phthalate is 3.1 10-6. O 3.25 O 5.08 O 5.51 O 5.94

Solution X is a 400 mL benzoate/benzoic acid buffer solution with a pH of 3.49. If the concentration of benzoic acid present in solution X is 0.3 mol L–1, calculate the concentration of sodium benzoate (in mol L–1) present in solution X at 25 °C. The Ka of benzoic acid is 6.5E-5.

When 25.00 ml of an unknown monoprotic weak acid was titrated with 0.856 M NaOH, the following series of pH measurements in the region of the equivalence point were collected. Based on the data provided. calculate the concentration, in M, of the weak acid: Report the answer to three places after the decimal. Do not include units pH Titration Data Near Equivalence Point Volume of Solution Added from Buret (mL) pH 10.26 10.78 11.32 11.86 12.37 12.89 6.22 664 10.32 10.97 11:22 11,36