An unknown concentration of sodium thiosulfate, Na2S2O3,Na2S2O3, is used to titrate a standardized solution of KIO3KIO3 with excess KIKI present. Suppose 16.05 mL16.05 mL of the Na2S2O3Na2S2O3 solution is required to titrate the iodine formed from 21.60 mL21.60 mL of 0.0115 M KIO3.0.0115 M KIO3. What is the molarity of the Na2S2O3Na2S2O3 solution?

A 0.200 M K2SO3 solution is produced by A) diluting 250.0 mL of a 1.00M K2SO3 solution to 1.00 L B) diluting 100.0 mL of a 2.50 M K2SO3 solution to 250.0 mL C) diluting 20.0 mL of a 5.00 M K2SO3 solution to 500.0 mL D) diluting 1.00 mL of a 250M K2SO3 solution to 1.00 L O B C OD O A

A 2.1182.118 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/molMM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/molMM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.1030.10 mL of a 0.7570.757 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture.

An aqueous solution of methanol (455. mL) was diluted to a volume of 3.50 L giving a concentration of 0.0875 M. What was the concentration of the original solution ?

A stock solution of potassium permanganate (KMnO4) was prepared by dissolving 17.1 g  KMnO4 with DI H2Oin a 100.00-mL volumetric flask and diluting to the calibration mark. Determine the molarity of the solution.

Calculate the final molarity of H2O2H2⁢O2 if 5.2 mL5.2 mL of a 3.0% w/w H2O23.0% w/w H2⁢O2 solution, which has a density of 1.0 g/mL,1.0 g/mL, is added to 5.2 mL5.2 mL of a starch-iodide solution.

1.50 mL of 0.15M Fe2(SO4)3 is diluted with deionized water to 25.00 mL in a volumetric flask. What is the concentration (molarity) of iron (not Fe2(SO4)3) in the diluted sample?

How would you prepare: a. 5.00 L of 1.50 M KMnO4 from solid reagent. b. 400.0 mL of a solution that is 0.0500 M I- starting with MgI2. c. 4.00 L of 0.175 M HCIO4, starting with an 8.00 M solution of the reagent.

You are the public health officer in the water treatment facility for a city of 50,000 people. A concentration of 1.0 ppm fluride in the drinking water is sufficient for the purpoise of helping to prevent tooth decay. The compound normally chosen for fluoridation is the same as is found in some toothpastes, sodium fluoride (NaF). Calculate how many kilograms of sodium fluride you will need to purchase in order to fluoridate the city's water supply for one year, based upong your estimate that the average daily consumption of water is 150 gallons per person   You will find the following information helping in solving the problem below. Sodium fluride, NaF, is 45.0% fluride by mass.  1 ppm means "one part per million" by mass, e.g. 1 g of fluoride peron million grams of water 1 gallon = 3.79 L 1 year = 365 days 1 ton = 2000lb 1 lb = 453.6 g  Density of water = 1.0 g/mL