QUESTION 3 What is the pH of a buffer solution composed of HA and A (Ka...

Question

Question

science chemistry

Answer 1

Answer #1

According to Henderson-Hasselbalch equation

pH = pKa +log ([Base]/[Acid])

pKa = -logKa = -log(1.38 x 10-4) = 4- log(1.38) = 4 - 0.1398 = 3.860

pH = 3.86 + log (0.65/0.62) = 3.86 + log (1.048) = 3.86 + 0.02 = 3.88

pH = 3.88

Note : Please give your feedback

Answer 2

Similar Homework Help Questions

1. What is the pH of a buffer solution that is composed of a weak acid,...

1. What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=7.2×10–8), and the conjugate base, A–, after 2.81 mL of 0.122 M HCl solution is added. The initial concentrations of the 183 mL buffer solution are [HA]=0.67 M and [A–]=0.65 M. Enter your value to two (2) decimal places. 2. What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=7.37×10–4), and the conjugate base, A–, after...
What is the pH of a buffer solution that is composed of a weak acid, HA...

What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.45×10–8), and the conjugate base, A–, after 2.71 mL of 0.135 M HCl solution is added. The initial concentrations of the 142 mL buffer solution are [HA]=0.7 M and [A–]=0.37 M. Enter your value to two (2) decimal places.
What is the pH of a buffer solution that is composed of a weak acid, HA...

What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=2.58×10–5), and the conjugate base, A–, after 1.83 mL of 0.094 M HCl solution is added. The initial concentrations of the 133 mL buffer solution are [HA]=0.38 M and [A–]=0.67 M. Enter your value to two (2) decimal places.

What is the pH of a buffer solution that is composed of a weak acid, HA...

What is the pH of a buffer solution that is composed of a weak acid, HA (Ka=5.01×10–9), and the conjugate base, A–, after 1.75 mL of 0.122 M HCl solution is added. The initial concentrations of the 86 mL buffer solution are [HA]=0.42 M and [A–]=0.45 M. Enter your value to two (2) decimal places.
Consider a buffer composed of aqueous HA and A.The Ka for HA is 3.7 x 109....

Consider a buffer composed of aqueous HA and A.The Ka for HA is 3.7 x 109. The concentration of HA (aq) and A (aq) would be equal in a buffer solution with a pH equal to O A. 9.28 B. 7.00 C. 6.63 OD. 4.75 E.8.43 Reset Selection
Consider a buffer composed of aqueous HA and A- . The Ka for HA is 3.7...

Consider a buffer composed of aqueous HA and A- . The Ka for HA is 3.7 x 10-9 . Which of the following combinations of reagents will produce an HA / A- buffer with pH 8.13? A. 0.80 mol of HA and 0.40 mol of A - B. 0.80 mol of HCl and 1.20 mol of A - C. none of these D. 1.20 mol of HA and 0.40 mol of NaOH E. all of these

1. Determine the pH of a buffer solution prepared by mixing 25.3mL of 0.35M HA (Ka=...

1. Determine the pH of a buffer solution prepared by mixing 25.3mL of 0.35M HA (Ka= 1.6x10-5) with 15.3mL of 0.45M NaA. 2.100 mL of buffer solution that is 0.15M HA (Ka= 6.8x10-5) and 0.20M NaA is mixed with 17.3mL of 0.25M HCl. What is the pH of the resulting solution? 3. Calculate the pH of a solution made by mixing 75.0mL of 0.15M HA (Ka= 2.5x10-5) with 7.5mL of 0.75M NaOH 4. 100 mL of buffer solution that is...
A buffer solution is composed of 0.380 M HA, a weak monoprotic acid, and 0.760 M...

A buffer solution is composed of 0.380 M HA, a weak monoprotic acid, and 0.760 M NaA, the sodium salt of the acid. The solution has a pH of 4.10. What is the Ka of the weak acid, HA? tks!!!!!!!!!!!!!
You wish to make a buffer solution using an acid (HA) with a Ka of 8.90 x 10-6 and a salt of its conjugate base (Na...

You wish to make a buffer solution using an acid (HA) with a Ka of 8.90 x 10-6 and a salt of its conjugate base (NaA). If you start with 1.50 MHA and 2.25 M NaA: what is the hydronium concentration at equilibrium? concentration: what is the pH? pH:

You wish to make a buffer solution at a pH 9.56 with the weak acid HCN...

You wish to make a buffer solution at a pH 9.56 with the weak acid HCN (Ka = 6.9 x 10-10 ) and its salt, NaCN..What ratio of the concentration of conjugate base to the acid: ([A- ]:[HA]) is required to attain the desired pH? a. [A- ] is 2.5 × that of [HA] b. [A- ] is 5 × that of [HA] c. [A- ] is 1 × that of [HA] d. [A- ] is ½ × that of...