An aqueous solution of barium hydroxide is standardized by titration with a 0.180 M solution of perchloric acid. If 26.1 mL of base are required to neutralize 15.7 mL of the acid, what is the molarity of the barium hydroxide solution? ________M barium hydroxide

Determine the concentration of nitric acid if 26.5 mL of nitric acid is titrated with 16.0 mL of 0.30 M sodium hydroxide.

1. If 10. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =   mL? 2. A 7.52-g sample of a diprotic acid requires 179.0 mL of a 0.750 M NaOH solution for complete neutralization. Determine the molar mass of the acid.  g/mol?

None

An aqueous solution of sodium hydroxide is standardized by titration with a 0.156 M solution of nitric acid. If 12.4 mL of base are required to neutralize 22.4 mL of the acid, what is the molarity of the sodium hydroxide solution?_____M sodium hydroxide

A student is asked to standardize a solution of calcium hydroxide. He weighs out 0.945 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 27.4 mL of calcium hydroxide to reach the endpoint. A. What is the molarity of the calcium hydroxide solution? M This calcium hydroxide solution is then used to titrate an unknown solution of hydrochloric acid. B. If 12.3 mL of the calcium hydroxide solution is required to neutralize 29.7 mL of hydrochloric acid, what is the molarity of the hydrochloric acid solution? M

__________  is the solvent in an aqueous solution of sodium sulfate and barium nitrate.     barium nitrate                   sodium sulfate                     water     barium sulfate                    sodium nitrate

Upon adding 275 mL of water to 275 mL of a 0.310 M aqueous solution of NaOH, the concentration of NaOH in the new solution will be ___________ that of the original solution.

1. Original volume of unknown NaCl solution = _______99.481______ mL   2. The concentration of Ag + within the 10 mL unknown NaCl solution after AgCl is added         [Ag+] = _______1.97412 x 10^(-10)_______________   3. Calculate the concentration of Cl- in the 10mL unknown NaCl solution. The Ksp for Silver Chloride is: 1.83 x 10-10.    Show your work below. AgCl(s)⇌Ag+(aq)+Cl−(aq)  Ksp=[Ag+][Cl−]       4. Calculate the mass of NaCl in the 10 mL unknown solution. Show your work. Hint:  mole = molarity x L; mass = mole x molar mass     5. Calculate the mass of NaCl in the original unknown solution. Show your work. mass of NaCl in the original unknown solution =             mass of NaCl in the 10 mL unknown solution x  ((?? ?? ???????? ?????? ?? ??????? ???? ????????) /10 ??)