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(a) A student prepares a solution by obtaining 168 mL from 0.100 M of NaOH and diluting it to a total volume of 634 mL. What is the concentration of the solution prepared by the student? (b) How many milliliters of 9.500 M perchloric acid solution should be used to prepare 0.2890 L of 0.7000 M of perchloric acid? A student adds 28.7 mL of water to 89.9 mL of a 5.10 M glucose solution. (i) Will this solution be concentrated or dilute? -concentrated -dilute (ii) What is the concentration of the solution? SHOW CORRECT UNITS!

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Related questions

What would be the final concentration of a sodium hydroxide solution prepared by diluting 5.00 mL of concentrated NaOH (19.3 M) to 74.63 mL?

What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by diluting 40 mL of concentrated (11.6 M) HCl to a final volume of 500 mL?

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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