Estimate the volume of a solution of 4.5 M NaOH that must be added to adjust the pH from 4.0 to 9.0 in 51 ml of a 99 mM solution of phosphoric acid.

Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.

Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)

Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2

1. Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine is 1.8 x 10-9. The answer must be given with the correct number of significant figures. 2. How many grams of NaF must be added to 60.0 mL of 0.500 M HF(aq) to adjust the pH to 3.40? Assume no volume change. The pKa of HF is 3.14.

Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?

A chemistry graduate student is given 125. mL of a 0.80M ammonia (NH3) solution. Ammonia is a weak base with K₂ = 1.8 × 10. What mass of NHÂBr should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.55? 4 You may assume that the volume of the solution doesn't change when the NH Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 × S

What is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 ✕ 10−14.)

Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.

The acidity of a solution is measured by its pH. If HT| represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log H+ Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 37.93% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 4.36, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number - (Report to the nearest 0.01)