A 10.00 mL solution of 0.1900 M NH4Cl is titrated with 0.1300 M NaOH to the equivalence point. Volume of NaOH = 14.62mL Calculate the pH of the solution at the equivalence point. Calculate the pH of a simple 0.0772 M aqueous solution of ammonia.

A 0.150 M solution of potassium citrate commonly used to treat kidney stone condition called renal tubercular acidosis and to prevent kidney stones that may occur with gout is prepared by dissolving in water. A 50.0 mL sample of this potassium citrate solution is titrated with a 0.150 M hydroboric acid at 25°C. What is the pH of the solution at the equivalence point of the titration? Potassium citrate is a basic salt with the formula K3C6H5O7. The Acid Ionization constant of its conjugate, citric acid is 7.1x10^-4 at 25°C. Please answer very soon will give rating surely

When 32.3 mL of 0.100 M Ba(OH)2 is mixed with 197.2 mL of 0.200 M HCl, the reaction goes to completion. Calculate the pH of the solution.

consider the titration of 50.0 mL of 0.10 M acetic acid with NaOH. drag and drop each amount of NaOH added (to the acetic acid) Into the appropriate resulting pH. In other words, determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solutions be acidic, basic, or neutral? Consider the stration of 50.0 ml of 0.10 M acetic acid (HC₂H₂O₂. K, -18 x 10) with NaOH. Drag and drop each amount of NaOH added to the acetic acid) into the appropriate resulting pH. In other words determine the pH of the final solution after each volume of NaOH has been added. Will the resulting solution be acidic, basic, or neutra? Acidic Neutral Basic Drag and drop your selection from the following list to complete the answer 25.0 mL (total) of 0.10 M NaOH has been added (the halfway point) 50.0 mL. (total) of 0.10 M NaOH has been added (the equivalence point) 10.0 mL (total) of 0.10 M NaOH has been added 60.0 mL (total) of 0.10 M NaOll has been added No NaOH has been…