To 2.12L of 0.473M NaOH, you add 3.52L of a second NaOH solution of an unknown concentration. The resulting solution is titrated and determined to be 1.170M. Assuming the volumes are additive, calculate the molarity of the second NaOH solution.

Write a balanced equation for the precipitation titration of the "iron chloride" and sodium hydroxide. Include physical states. balanced equation:

True or false: the determination of a molar mass of a compound by the titration method used today depends on having a pure sample of the unknown compound? Explain.

A 0.8159 g sample of HCl was placed into a 50 mL volumetric flask and the sample was thoroughly dissolved in water to make 50 mL of solution. It required 22.07 mL of NaOH to reach the endpoint in the titration. What is the molarity of the NaOH solution? I mg IHE/ 2.022 4 mol 0.81599 Hcl 36.4bg.

Sonomic acid is a monoprotic acid developed in the chemistry department of Sacramento state University. The storeroom staff successfully obtained a sample of sonomic acid and made a solution. They made the solution by adding 302.4 g of sonomic acid and diluting it to a volume of 10.00 L with water. Unfortunately, the stockroom attendant, Steven , does not know the molar mass of sonomic acid so he could not calculate the molarity of the solution he prepared. It would be great if you could help him.

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1166 M standard sodium hydroxide solution. He takes a 25.00mL sample of the original acid solution and diluted it to a 250.0mL. Then, he takes a 10.00mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.52mL of the standard solution. What is the concentration of the original sulfuric acid solution?  concentration:_____M

A solution was made by adding water to 0.293 g of H2ZH2Z until the volume totaled 25.00 mL. Subsequent titration required 40.50 mL of 0.093 M sodium hydroxide. Calculate the molar mass of H2ZH2Z (in g/mol).

The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail

3) When excess sliver nitrate was added to 25.00 ml of barium chloride, a precipitate of sliver chloride formed at the bottom of the beaker. If the mass of the precipitate was 4.30g, calculate the initial concentration of barium chloride.

A 25.0 mL sample of solution of unknown acid, HX, is titrated with 2.11 M KOH. If 67 mL of KOH was required to neutralize the sample, find the molarity of the original HX solution. Only enter your numerical answer. Do not enter units.