Question

1a. You need to make an aqueous solution of 0.180 M sodium fluoride for an experiment in lab, using a 300 mL volumetric flask. How much solid sodium fluoride should you add?

1b. How many milliliters of an aqueous solution of 0.215 M ammonium bromide is needed to obtain 9.82 grams of the salt?

1c. In the laboratory you dissolve 24.0 g of iron(III) fluoride in a volumetric flask and add water to a total volume of 125 . mL.

2. In the laboratory you dissolve 18.0 g of sodium fluoride in a volumetric flask and add water to a total volume of 375 mL.

What is the molarity of the solution? ___ M.

What is the concentration of the sodium cation? ____ M.

What is the concentration of the fluoride anion? ____ M.

3a. You wish to make a 0.325 M hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution?

3b. In the laboratory you dilute 3.68 mL of a concentrated 12.0 M hydroiodic acid solution to a total volume of 50.0 mL. What is the concentration of the dilute solution?

3c. In the laboratory you dilute 2.35 mL of a concentrated 6.00 M hydrobromic acid solution to a total volume of 175 mL. What is the concentration of the dilute solution?

4a. How many grams of Cu(OH)₂ will precipitate when excess KOH solution is added to 49.0 mL of 0.640 M CuI₂ solution?

CuI₂(aq) + 2KOH(aq) ---> Cu(OH)₂(s) + 2KI(aq)

4b. How many mL of 0.763 M HBr are needed to dissolve 7.67 g of BaCO₃?

2HBr(aq) + BaCO₃(s) ----> BaBr₂(aq) + H₂O(l) + CO₂(g)

5. What volume of a 0.389 M hydrochloric acid solution is required to neutralize 24.1 mL of a 0.113 M calcium hydroxide solution?
_________ mL hydrochloric acid

6. An aqueous solution of hydrochloric acid is standardized by titration with a 0.113 M solution of barium hydroxide.
If 24.1 mL of base are required to neutralize 29.3 mL of the acid, what is the molarity of the hydrochloric acid solution?

______________ M hydrochloric acid

7.
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the unwieldy formula of KHC₈H₄O₄. This is often written in shorthand notation as KHP.

If 29.3 mL of a potassium hydroxide solution are needed to neutralize 1.23 grams of KHP, what is the molarity of the potassium hydroxide solution?
________ M

8a. The concentration of H₃AsO₃ in a solution is determined by titrating it with a 0.1464 M Ce⁴⁺ solution. The balanced net ionic equation for the reaction is:

2Ce⁴⁺(aq) + H₃AsO₃(aq) + 5H₂O(l) -----> 2Ce³⁺(aq) + H₃AsO₄(aq) + 2H₃O⁺(aq)

In one experiment, 21.33 mL of the 0.1464 M Ce⁴⁺ solution is required to react completely with 20.00 mL of the H₃AsO₃ solution. Calculate the concentration of the H₃AsO₃ solution.

8b. A Ce⁴⁺ solution is standardized by titrating it with a 0.1733 M hydrogen peroxide solution. The balanced net ionic equation for the reaction is:

2Ce⁴⁺(aq) + H₂O₂(aq)+2H₂O(l) ------> 2Ce³⁺(aq) + O₂(g)+2H₃O⁺(aq)

If 19.34 mL of the 0.1733 M hydrogen peroxide solution is required to react completely with 40.00 mL of the Ce⁴⁺ solution, calculate the concentration of the Ce⁴⁺ solution.