Question

In: Chemistry

Outline how you would prepare a 0.1 M buffer solution of pH 11. b) add 5.0...

Outline how you would prepare a 0.1 M buffer solution of pH 11.

b) add 5.0 mL of 10 mM HCl to 500 mL of your buffer, calculate the pH after this addition

Solutions

Expert Solution

To prepare a buffer solution of pH 11, take a weak base of concentration 0.1M and the solution of its conjugate base of concentration 0.1M with equal volumes of acid and the salt.

A slightly different path to the [OH¯]

pH = 11, so pOH = 14 - pH = 14.00 - 11 = 3

[OH¯] = 10¯pOH = 10¯3= 0.001 M

[HB+] = [OH¯] =0.001 M

[B] = 0.1

Kb = [( 10¯3) ( 10¯3)] / 0.1

Kb = 1.0 x 10-5

such type of weak base must be selected whose Kb value is 1.0 x 10-5 .


Related Solutions

What should be the ph of a solution of 5.0 ml of 0.1 M acetic acid...
What should be the ph of a solution of 5.0 ml of 0.1 M acetic acid and 5.0ml of 0.1M sodium acetate and 40.0ml h20? please show steps
Need to prepare an acetate buffer solution: 25.00 mL of 0.1 M acetic acid and 0.1...
Need to prepare an acetate buffer solution: 25.00 mL of 0.1 M acetic acid and 0.1 M sodium acetate. The stock acetic acid is 6.0 M. The instructions involve the preparation of a (10-fold) intermediate acetic acid solution. Ka = 1.75 x 10-5 (pKa = 4.76). What are the values for the: * volume of acetic acid * grams of sodium acetate (since it's a solid) * volume of DI water needed * calculated pH Thanks.
Given a 0.1 M NH4Cl solution: a) Which is the pH of this solution? b) If...
Given a 0.1 M NH4Cl solution: a) Which is the pH of this solution? b) If 100 mL of 0.1 M HCl solution are added to 100 mL of the original solution, which is the pH? c) And if 100 mL of 0.1 M NH3 are added to 100 mL of the original solution? Data: kb(NH3 ) = 1.8 10^-5 .
How you would prepare a 500 mL solution of 0.1M "tris" buffer at pH of 7.5...
How you would prepare a 500 mL solution of 0.1M "tris" buffer at pH of 7.5 starting with solid tris free base. The free base has a chemical forumla of (HOCH2)3-C-NH2 and a MW of 121.1 g/mol. The protonated amine form, tris-chloride, has a pKa of 8.10. To prepare the solution, 1.0M HCl will be used.
How can you prepare 100.0 mL of acetic buffer solution (0.100 M) with pH = 5.10...
How can you prepare 100.0 mL of acetic buffer solution (0.100 M) with pH = 5.10 by using a solution of acetic acid (25% w/w, density = 1.05 g/cm3 ) and pure sodium acetate. (pKa = 4.76; M. W. = 60.05 g/mol for HAc and 82.03 for NaAc).
Show how would you prepare a solution of 500 ml of a 0.15 M acetate buffer....
Show how would you prepare a solution of 500 ml of a 0.15 M acetate buffer. You have available the following: 6M HCl, 4 M acetic, solid sodium acetate, solid sodium hydroxide
a) What happens when you add acid to a solution of 0.1 M HNO2 and 0.1...
a) What happens when you add acid to a solution of 0.1 M HNO2 and 0.1 M KNO2? Write a chemical equation if relevant. b) Why doesnt the same kind of reaction occur when you add acid to a solution of 0.1 M HNO3 and 0.1 M KNO3?
You need to prepare 100.0 mL of a pH = 4.00 buffer solution using 0.100 M...
You need to prepare 100.0 mL of a pH = 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and 0.200 M sodium benzoate. How much of each solution should be mixed to prepare this buffer?
Assume that you have a solution of 0.1 M glucose 6-phosphate. To this solution, you add...
Assume that you have a solution of 0.1 M glucose 6-phosphate. To this solution, you add the enzyme Phosphoglucomutase, which catalyzes the following reaction: The ΔG0’ for the reaction is +1.8 kcal mol-1. (a) Does the reaction proceed as written? If so, what are the final concentrations of glucose 6-phosphate and glucose 1-phosphate?
What would be the pH of a 0.1 M aqueous solution of the phenolate ion, C6H5O�?...
What would be the pH of a 0.1 M aqueous solution of the phenolate ion, C6H5O�? (Ka for phenol, C6H5OH, is 1.3 x 10�10) I don't understand the steps to get this anwser
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT