Question

In: Chemistry

A pH 3.30 buffer is prepared from iodoacetic acid ICH2COOH (pKa = 3.175), and sodium iodoacetate,...

A pH 3.30 buffer is prepared from iodoacetic acid ICH₂COOH (pK_a = 3.175), and sodium iodoacetate, ICH₂COO^-Na⁺ . If ionic strength of the buffer solution must not exceed 0.200 M, what are the maximum concentrations of the two components that could be used?

What volume of KOH (conc = 1.850 M), could be added to 50.00 mL of the buffer solution of part (a), before the pH would increase to 4.000?

Expert Solution

ICH2COONa + ICH2COOH = 0.200 M

pH = pKa + log [salt/acid]

3.30 = 3.175 + log (ICH2COONa/ICH2COOH)

1.33 = ICH2COONa / ICH2COOH

ICH2COONa + ICH2COOH = 0.200 M

1.33 ICH2COOH + ICH2COOH = 0.200

2.33 ICH2COOH = 0.200

[ICH2COOH] = 0.0858 M

ICH2COONa = 1.33 ICH2COOH = 1.33 x 0.0858

= 0.114 M

[ICH2COONa] = 0.114 M

ICH2COOH + KOH -------------------> ICH2COOK + H2O

0.0858 x 50 1.850 V 0 0

4.29 - 1.850 V 0 1.850 V 1.850V

here salt and acid remaining so it forms acidic buffer.

pH = pKa + log [salt / acid]

4.00 = 3.175 + log [1.850V / 4.29 - 1.850V]

6.68 = [1.850V / 4.29 - 1.850V]

V = 2.02 mL

volume of KOH added = 2.02 mL

queen_honey_blossom answered 11 months ago

1. Calculate the pH of the buffer of a solution of 0.02M acetic acid (pKa =...

1. Calculate the pH of the buffer of a solution of 0.02M acetic acid (pKa = 4.76) and 0.04 M acetate 2. Based on your answer to the previous question, how much of a 0.5 M solution of HCl must be added to 200 mL of the above mentioned solution to lower the pH to 2.50? Ignore volume changes.

500ml of an HTS/TS- buffer (pKa = 5.25) at pH 4 was prepared. Unfortunately, the student...

500ml of an HTS/TS- buffer (pKa = 5.25) at pH 4 was prepared. Unfortunately, the student who had prepared the buffer forgot how many moles of HTS and TS- he had added. Although HTS does not fluoresce, TS- does fluoresce. (If = 1000CTS). The intensity of the fluorescence signal from the buffer is 10. How many moles of HTS and TS- were used to prepare 500ml of the pH 4 buffer?

Preparation of the acetic acid-sodium acetate buffer: Calculate the theoretical pH of this buffer solution. 3.504...

Preparation of the acetic acid-sodium acetate buffer: Calculate the theoretical pH of this buffer solution. 3.504 grams of NaC2H3O2*3H2O with 8.8 mL of 3.0 M acetic acid and 55.6 mL of distilled water. Experimental pH of buffer solution: 4.8

calculate the ph of a mixture of 0.26M acetic acid (pKa 4.76) and 0.23 M sodium...

calculate the ph of a mixture of 0.26M acetic acid (pKa 4.76) and 0.23 M sodium acetate.

A buffer was prepared by adding 1.00 mol of formic acid and 1.00 mol of sodium...

A buffer was prepared by adding 1.00 mol of formic acid and 1.00 mol of sodium formate to 1.00 L of distilled water. A 100.0 mL aliquot of 1.00 M HCl is then added. What is the pH of the resulting buffer solution? (Formic acid pKa=3.74)

An acetic acid-sodium acetate buffer can be prepared by adding sodium acetate to HCl(aq). a) Write...

An acetic acid-sodium acetate buffer can be prepared by adding sodium acetate to HCl(aq). a) Write an equation for the reaction that occurs when sodium acetate is added to HCl(aq) b) If 10.0g of CH3COON is added to 275 mL of 0.225 M HCl(aq), what is the pH of the resulting buffer? c) What is the pH of the solution in part b after the addition of 1.26g of solid NaOH?

What is the pH of a buffer containing 20.53g benzoic acid and 17.23g sodium benzoate in...

What is the pH of a buffer containing 20.53g benzoic acid and 17.23g sodium benzoate in 500mL of solution?

Prepare 1 L of an acetic acid sodium acetate buffer with a pH of 5.00 and...

Prepare 1 L of an acetic acid sodium acetate buffer with a pH of 5.00 and a buffer concentration of 100 mM. Besides water you only have a 500g bottle of sodium acetate trihydrate, 1L of 1.00 hydrochloric acid, and 1L of 1.00 M sodium hydroxide. A. Identify the reagents needed and calculate all amounts needed. B. Calculate the change in pH of a 250 mL portion of the buffer that has 1 mL of 1.00 M NaOH added to...

A buffer contains 0.150M acetic acid and 0.105M in sodium acetate. a) Calculate the pH of...

A buffer contains 0.150M acetic acid and 0.105M in sodium acetate. a) Calculate the pH of the buffer. b) What is the volume of 6.0M NaOH must be added to raise the pH of 100.0 mL of the buffer by 1.5 pH units? c) Calculate the pH when 2.0 mL of 6.0M is added to 100.0 mL to the buffer. please show work. question is due before 11PM

What is the pH of a buffer solution that contains 0.350M pyruvic acid and 0.150M sodium...

What is the pH of a buffer solution that contains 0.350M pyruvic acid and 0.150M sodium pyruvate? Ka = 4.1x10^-3 Select one: A. 4.72 B. 2.82 C. 2.02 D. 2.76 What is the pH of a 100.0mL buffer solution that contains 0.215M acetic acid and 0.255M sodium acetate after 0.055 mmol HCl is added. Assume no volume change. Ka = 1.8x10^-5. Select one: A. 4.61 B. 4.87 C. 5.03 D. 5.48 Calculate the change in pH after 0.010 mole HCl...