Blue #1 is an FDA approved dye with the formula C37H34N2Na2O9S3. A stock solution is prepared by adding 75.0 mg of Blue #1 to enough water to prepare 250.0 ml of solution. A working solution is prepared by diluting 25.0 ml of the stock solution to a final volume of 500.0 ml. Calculate the concentration of the working solution in mol/L.

Calculate the molarity of NaOH solution prepared by mixing 25 mL of 0.60 M NaOH with 250 mL H2O.

Calculate the % by mass Sr(OH)2 , M, N, m, mf H2 O of a Sr(OH)2 solution that contains 107.2 g Sr(OH)2 dissolved in enough H2O to make 3.000 L of solution. The density of the solution is 1.14 g/mL.

A student is asked to standardize a solution of calcium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 37.2 mL of calcium hydroxide to reach the endpoint. A. What is the molarity of the calcium hydroxide solution? This calcium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 18.1 mL of the calcium hydroxide solution is required to neutralize 24.6 mL of hydrobromic acid, what is the molarity of the hydrobromic acid solution? M M

What is the concentration in each of the following solutions?   240 ml of 0.200 M KNO3 is added to 160 ML of water.   2.25 g of NaCl is dissolved in 250 ml of water

2. a) 25mL of water is added to 125mL of 1 0.15mol/L NaOH solution, what is the concentration of the diluted solution? b) What volume of 0.05mol/L HCl solution is made by diluting 250mL of 10.0mol/L HOCI?

The maximum contaminant level of cyanide (CN) in drinking water as set by the the Environmental Protection Agency (EPA) is 0.00020 g · L. Express this concentration in parts per million (ppm). Assume the density of water is 1.00 g/mL. concentration: Ppm

Consider a 1.000-L stock solution of 9.69 M Na3PO4. A 2.000-mL aliquot is taken from this stock solution and diluted to a final volume of 1.000 L. A 5.000-mL aliquot is then taken from this new solution and further diluted to make a new solution with a final volume of 750.0 mL.   Calculate Na+ in the final solution.

2.000 g TUMS tablet (CaCO3 and Binder) was analyzed in a lab. 11.42 mL of 0.871 M HCI was needed to dissolve the CaCO3 (active ingredient) of TUMS Tablet. Find the mass and % by mass of CaCO3 in TUMS Tablets. ( 459.00 mg O 75% 50% 605.00 mg 30% O 25% O 400.00 mg O 500,00 mg

A researcher has a sample of potassium chloride that is contaminated with magnesium chloride. They weigh 5.00 g of the sample, dissolve it in 1.00 L of water, and determine the chloride ion concentration to be 0.0708 M. What mass (in g) of the 5.00 g sample was magnesium chloride?