1. Calculate the buffer capacity for 100 mL of buffer if 12.02 mL of 0.09978 M...

1. Calculate the buffer capacity for 100 mL of buffer if 12.02 mL of 0.09978 M NaOH was used to change the pH by 0.54 units.

a. 0.022 b. 0.00022 c.12.22 d.0.22

2. Calculate the pH of a buffer with 0.10 M benzoic acid and 0.10 M sodium benzoate. Use activity coefficient table 8-1 in the (9th edition) textbook to determine the activities for the ions (benzoate ion =C₆H₅CO₂¯). The pKa of benzoic acid is 4.20.

a. 4.20 b. 4.28 c.4.10 d.4.35

3. Suppose you have a solution of benzoic acid and sodium benzoate with an ionic strength of 0.19 M. Calculate the activity coefficient for the benzoate ion. The benzoate ion has an ion size of 600 pm.

a.-0.46 b.0.83 c.3.26 d. 0.34 e.0.75

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Calculate the weight of buffer needed to make 100 mL of a 0.1 M buffer of...

Calculate the weight of buffer needed to make 100 mL of a 0.1 M buffer of acetate (MW=136.1g/mol)

calculate the pH of 100 mL of a buffer that is .080 M NH4Cl and .105...

calculate the pH of 100 mL of a buffer that is .080 M NH4Cl and .105 M NH3 before and after the addition of 1.00mL of 6.05 M HNO3

A 100. mL buffer solution is 0.300 M in HAc and 0.150 M in NaAc. Calculate...

A 100. mL buffer solution is 0.300 M in HAc and 0.150 M in NaAc. Calculate the pH of the solution after the addition of 35.0 mL of 0.20 M HCl. The Ka for HAc is 1.8 × 10-5.

Buffer 1) 100 mL of 0.50 M sodium phosphate buffer, pH 7.0 MW; 137.99

What is the buffer capacity for a solution that requires 3.35 mL of 0.10 M HCl...

What is the buffer capacity for a solution that requires 3.35 mL of 0.10 M HCl to change the pH by 1 unit?

Calculate the pH of 100.0 mL of a buffer that is 0.0700 M NH4Cl and 0.115 M...

Calculate the pH of 100.0 mL of a buffer that is 0.0700 M NH4Cl and 0.115 M NH3 before and after the addition of 1.00 mL of 5.10 M HNO3. Before= After=

Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl and 0.180...

Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl and 0.180 M NH3 before and after the addition of 1.00 mL of 5.50 M HNO3. Can you please do a step-by-step of how to solve this, paying special attention to how to get the Ka in the Henderson Hasselbalch Equation? That's the part I'm not understanding.

Question