Solid sodium sulfide is slowly added to 150 mL of a 0.454 M manganese(II) nitrate solution until the concentration of sulfide ion is 0.0268 M. The mass of manganese(II) ion remaining in solution is  grams.

M Complete and balance the chemical equation associated with the neutralization of aqueous sodium hydroxide with aqueous boric acid. If it takes 20.45 ml of a 0.1026 M standard sodium hydroxide solution to titrate 25.00 ml of an unknown boric acid solution, what was the original concentration of the unknown boric acid solution?

You have 559 ml of 3.29 M HCl.  Using a volumetric pipet, you take 297 ml of that solution and dilute it to 612 ml in a volumetric flask.  Now you take 100.00 ml of that solution and dilute it to 176 ml in a volumetric flask.  What is the concentration of hydrochloric acid in the final solution?

Enter your answer in the box provided. A 2250 mL sample of 2.50 M HCl solution is treated with 4.14 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged. M HCI ences

A sodium sulfate solution is added to a 25.0 mL sample of a solution containing Ba2+ ions until no more precipitate formed.  The precipitate (BaSO4) is collected, dried, and weighed.  If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0 mL sample? Your answer should have 3 sig. figs. Molar Masses:  (Na2SO4: 142.05 g/mol)  (Ba2+: 137.3 g/mol) (BaSO4: 233.37 g/mol)

14.00 mL of deionized water is added to 35.00 mL 0.250 M hydrochloric acid. Calculate the molarity of the resulting solution.

A standard solution of 0.2436 M NaOH was used to determine the concentration of a hydrochloric acid solution. If 46.33 mL of NaOH is needed to neutralize 10.00 mL of the acid, what is the molar concentration of the acid in the original solution?

8. A chemist wants to make 100 of a 0.15 M AlCl 3 (aq) solution. How many grams of aluminum chloride should the chemist use?

A student soaks willow bark (a natural source of salicylic acid) in ethanol. After a few minutes, the student has 12.5 mL of salicylic acid. The student determines the concentration of salicylic acid is 0.30 M. Calculate the amount, in grams, of acetylsalicylic acid that can be produced when the salicylic acid is reacted with excess acetic acid.

In the laboratory, a student dilutes 11.9 mL of a 6.96 M hydroiodic acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution? M Concentration =