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It was found that a 20.00 mL portion of a solution of oxalicacid, H2C2O4, requires 7.08 mL of0.200 M K2Cr2O7 forcomplete reaction in an acidic solution. In the reaction, theoxidation product is CO2 and the reduction product isCr3+. How many milliliters of 0.450 M NaOH arerequired to completely neutralize theH2C2O4 in a separate 20.00 mLsample of the same oxalic acid solution?

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Patrina SchowalterLv2
28 Sep 2019
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Related questions

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1) A 24.00 รขยˆย’mL sample of an unknown HClO4 solution requires titration with 22.82 mL of 0.1900 M NaOH to reach the equivalence point.
What is the concentration of the unknown HClO4 solution? The neutralization reaction is:
HClO4(aq)+NaOH(aq)รขย†ย’H2O(l)+NaClO4(aq)

2) A 25.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.33 mL of NaOH solution is added.
What is the concentration of the unknown H3PO4 solution?

3) An acid solution is 0.100 M in HCl and 0.200 M in H2SO4.
What volume of a 0.140 M KOH solution would have to be added to 550.0 mL of the acidic solution to neutralize completely all of the acid?

4) A tanker truck carrying 2.01รƒย—103 kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuric acid solution is 95.0% H2SO4 by mass and has a density of 1.84 g/mL.
Sodium carbonate (Na2CO3) is used to neutralize the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 2.01รƒย—103 kg of sulfuric acid solution?

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.

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