Question

You will be standardizing a .8 M NaOH solution using oxalic acid di-hydrate. You want to...

You will be standardizing a .8 M NaOH solution using oxalic acid di-hydrate. You want to use about 15 mls per titration of NaOH. What should the molarity of your oxalic acid be?

0 0
Add a comment Improve this question Transcribed image text
Know the answer?
Add Answer to:
You will be standardizing a .8 M NaOH solution using oxalic acid di-hydrate. You want to...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Sample Data Sheet: TITRATION AND MOLARITY Part I: Preparing the Oxalic Acid solution 1.         Mass of...

    Sample Data Sheet: TITRATION AND MOLARITY Part I: Preparing the Oxalic Acid solution 1.         Mass of oxalic acid + weighing paper.                     _____1.5765_____________ g 2.         Mass of weighing paper.                                            _____n/a_____________ g 3.         Volume of oxalic acid solution.                                                 250       mL 4.         Concentration of oxalic acid=___________        (show calculation above) Part III: Completing the Neutralization    Trial #1 Trial #2 Trial #3 Volume of Oxalic Acid 15ml 15ml 15ml Final Buret Reading of NaOH (mL)           15.87 15.74 19.43 Initial...

  • You want to determine the concentration of acid in a particular solution. To this end, you...

    You want to determine the concentration of acid in a particular solution. To this end, you decide to titrate the acid with a standardized sodium hydroxide solution. You quickly throw together an approximately 0.1 M NaOH solution, and then you realize you need to know the exact concentration of this solution before you can use it for anything meaningful. 1. Using an acid-base titration, 30.65 mL of your NaOH solution were needed to neutralize 0.6923 g of KHP (potassium hydrogen...

  • You titrated a 22.00 mL solution of 0.0300 M oxalic acid with freshly prepared solution of...

    You titrated a 22.00 mL solution of 0.0300 M oxalic acid with freshly prepared solution of KMnO4. If it took 48.99 mL of this solution, what is the molarity of the KMnO4? 0.022 L of 0.300 M oxalic acid (0.022)(0.03) = 0.00066 mol oxalic acid 0.0006 mol oxalic acid x (2 mol KMnO4)/(5 mol oxalic acid)= 0.000264 mol KMnO4 0.000264 mol/0.04899 L = 0.05388855 M KMnO4 = 0.005388 M KMnO4 where did I go wrong? Question 7 0.1 / 1...

  • - What is a primary standard? You have weighed out precisely 2.471 g of oxalic acid...

    - What is a primary standard? You have weighed out precisely 2.471 g of oxalic acid dihydrate, and diluted it to 250,0 mL. What is its molarity? (Hint: Example 12.1) What is a secondary standard? You have diluted 9 mL of roughly 6 M NaOH to 500 mL. What is the approximate molarity of the base? (Pay attention to significant figures) (Hint: Example 12.2) What is the name of the indicator you are to use and what color does it...

  • Data Table 1 Mass of flask and oxalic acid (g) 117.43 Mass of empty flask (g)...

    Data Table 1 Mass of flask and oxalic acid (g) 117.43 Mass of empty flask (g) 116.93 Mass of oxalic acid (g) 0.5 Moles of oxalic acid (mol) Final volume of NaOH (mL) 17 Initial volume of NaOH (mL) 5 Volume of NaOH used (mL) 12 Moles of NaOH (mol) Molarity of NaOH (M) Data Table 2 Mass of flask and vinegar (g) 126.61 Mass of empty flask (g) 121.63 Mass of vinegar (g) 4.98 Final volume of NaOH (mL)...

  • A 0.100 M oxalic acid, HO2CCO2H, solution is titrated with 0.100 M KOH

    A 0.100 M oxalic acid, HO2CCO2H, solution is titrated with 0.100 M KOH. Calculate the pHs when 25.00 mL of oxalic acid solution is titrated with 10, 15, 20, 25, 35, 40, 45, 50 and 55 mL of NaOH. Kal = 5.4 x 10-2 and Ka2 = 5.42 x 10-5 for oxalic acid. Show all your work and make a graph of pH versus Vb

  • Trial one Trial two Trial three Volume of oxalic acid (mL) 10.1 mL 10.2 mL 10.1...

    Trial one Trial two Trial three Volume of oxalic acid (mL) 10.1 mL 10.2 mL 10.1 mL Moles of oxalic acid (moles) Initial volume of NaOH (mL) 18.7 mL 26.5 mL 34.6 mL Final volume of NaOH (mL) 26.5 mL 34.6 mL 42.6 mL Delivered volume of NaOH (moles) 7.8 mL 8.1 mL 8 mL Moles of NaOH (moles) Molarity of NaOH (M) Average Molarity NaOH (M) Concentration of oxalic acid (M) = 0.2567 Trial one Trial two Trial three...

  • 4. Calculate the mass of Oxalic acid (H2C2O4*2H2O) required to neutralize 20.0 ml of 0.10 M...

    4. Calculate the mass of Oxalic acid (H2C2O4*2H2O) required to neutralize 20.0 ml of 0.10 M NaOH solution using the balanced chemical equation for this reaction. 5. A 0.120 g sample of pure oxalic acid (H2C2O2*2H2O) was dissolved in water and neutralized with 21.0 ml of NaOH. Calculate the molarity of NaOH. Do not use scientific notation, but do use the proper number of significant digits and units.

  • 25.00 mL of a sulfuric acid solution was standardized by titration with 0.2500 M NaOH using...

    25.00 mL of a sulfuric acid solution was standardized by titration with 0.2500 M NaOH using phenolpthalein indicator. 30.52 ml of the NaOH was required. Find the molarity of the sulfuric acid. H2SO4 (aq) + 2NaOH (aq) ----> Na2SO4 (aq) + 2H2O (l)

  • You titrated a 25.00 mL solution of 0.02 M oxalic acid with a freshly prepared solution...

    You titrated a 25.00 mL solution of 0.02 M oxalic acid with a freshly prepared solution of KMnO4. If it took 41.81 mL of this solution to reach the endpoint, what was the molarity of the KMnO4? 0.0119 is wrong +/- 3 sig figs.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT