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

24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?

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 10.0 mL sample of 0.20 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0700 mol/L NaOH(aq) and then diluted to a final volume of 100. mL. Calculate the concentration of OH- ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.

A) Determine the pH of the solution that results from the mixing of 60.0 mL of 0.100 M NaOH, 94.0 mL of 0.0500 M KOH, 62.5 mL of 0.075 M HCl, 37.0 mL of 0.065 M HNO3, and 3.00 quarts of distilled water.   B)     Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points: a. Before any NaOH is added.      b. After 18.7 mL of NaOH are added.   c. After 25.00 mL of NaOH are added.   d. After 50.00 mL of NaOH are added.   e. After 53.00 mL of NaOH are added.   C) What is the pKa of the acid (show calculation)?

A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the KB of NH3 is 1.86 × 10^⁻5, determine the pH of the resultant solution. (You may assume the volume is unchanged.)