CHEM 104 Quiz: Titration/Buffers Quiz

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violetoyster294

30 Oct 2014

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Which of the following pairs of reagents, if reacted in 1. 0l of water, would result in a ph < 7? (select all that apply) This is a strong acid and a weak base, therefore the ph would be less than 7. Give the total volume of the solution in ml. Write your answer using one decimal places, even if this is not the correct number of significant figures. You must include a leading zero in your answer if appropriate (e. g. , 0. 7). You may want to use the following acid/base table to answer the question below. For more help, you may also want to go through the buffers module of the online acids and bases tutorial. You should review section 17. 1 from your text. phbuffercalc. Calculate the ph of a buffer solution made by mixing 213 ml of a 1. 84m trimethylamine (ch3)3n solution with 229 ml of a 1. 63m trimethylammonium chloride, (ch3)3nhcl solution.

Related Questions

1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titrations are correct

Drag items A-F to: Before equivalence point, At equivalence point, After equivalence point

A.) The pH of the solution is close to 2

B.) The pH of the solution is close to 12

C.) The pH of the solution is 7

D.) The color of the solution is pink

E.) The color of the solution is blue

F.) The pH changes most rapidly

2.) Consider the balanced equation for the titration of an acid, HCl, with a base, NaOH:

HCl(aq)+NaOH(aq)âNaCl(aq)+H2O(aq)

According to the balanced equation, to neutralize one mole of the acid (HCl) you will have to add one mole of the base (NaOH). Based on the number of moles of HCl and NaOH at a particular stage of titration, the progress of the reaction with respect to the equivalence point can be decided, as shown in the following table:

You can use the following equation to determine the number of moles in a given solution or volume of titrant: number of moles=molarity (mol/L)Ãvolume (in liters)

A volume of 100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point.

Drag items A-F to Before equivalence point, At equivalence point, After equivalence point

A.) 50.0 mL of 1.00 M NaOH

B.) 150 mL of 1.00 M NaOH

C.) 200 mL of 1.00 M NaOH

D.) 10.0 mL of 1.00 M NaOH

E.) 5.00 mL of 1.00 M NaOH

F.) 100 mL of 1.00 M NaOH

1. In a problem involving the mixing of a weak acid solution with a strong base solution (such as the titration of a weak acid with a strong base), before attempting to calculate the pH of the resulting solution, you must ___.

		A.) Determine which (the weak acid or strong base) is present in excess
		B.) Determine the pH of the weak acid solution.
		C.) determine th pH of the strong base solution
		D.) Determine the difference in volume of the acid and base solutions.

2.) Consider a weak acid , HA, for which the pKa is 5.826. The pH of a 0.28 M solution of this weak is is ___ at 25 oC. (Answer to three decimal places.)

3.) What is the pH of the solution resulting from mixing 33.07 mL of 0.183 M HA (pK_a = 4.876) with 14.82 mL of 0.100 M KOH? (answer to three decimal places)

pH = ___

4.)

What is the pH of a solution created by mixing 32.19 mL of 0.200 M HA (K_a = 1.81 x 10^-5 M) with 32.19 mL of 0.200 M KOH? (Answer to three decimal places)

pH = ___

5.)

What is the pH of a solution created by mixing 18.52 mL of 0.129 M HA (pK_a = 4.877) with 73.61 mL of 0.100 M KOH? (Answer to three decimal places)

pH = ___

CHEM 104 Quiz: Titration/Buffers Quiz

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