Question

33 . Strong base is dissolved in 565 L of 0.600 M weak acid (?a=3.30×10−5 M)(Ka=3.30×10−5...

33 . Strong base is dissolved in 565 L of 0.600 M weak acid (?a=3.30×10−5 M)(Ka=3.30×10−5 M) to make a buffer with a pH of 4.08. Assume that the volume remains constant when the base is added.

HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)

Calculate the pKa value of the acid and determine the number of moles of acid initially present.

When the reaction is complete, what is the concentration ratio of conjugate base to acid? How many moles of strong base were initially added?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. Strong base is dissolved in 565 mL of 0.400 M weak acid (Ka = 3.85...
1. Strong base is dissolved in 565 mL of 0.400 M weak acid (Ka = 3.85 × 10-5) to make a buffer with a pH of 4.07. Assume that the volume remains constant when the base is added. a. Calculate the pKa value of the scid and determine the number of moles of acid initially present. b. When the reaction is complete, what is the concentration ratio of conjugate base to acid? c. How many moles of strong base were...
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 ×...
Strong base is dissolved in 645 mL of 0.400 M weak acid (Ka = 4.91 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. Calculate the pKa value of the acid and determine the number of moles of acid initially present. When the reaction is complete, what is the concentration ratio of conjugate base to acid? How many moles of strong base were initially added?
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 ×...
Strong base is dissolved in 545 mL of 0.200 M weak acid (Ka = 4.02 × 10-5) to make a buffer with a pH of 4.11. Assume that the volume remains constant when the base is added. a) Calculate the pKa value of the acid and determine the number of moles of acid initially present. b) When the reaction is complete, what is the concentration ratio of conjugate base to acid? c) How many moles of strong base were initially...
You are given a buffer that contains a weak base whose concentration is 0.600 M and...
You are given a buffer that contains a weak base whose concentration is 0.600 M and its conjugate weak acid whose concentration is 0.260 M. The volume of this solution is 0.375 L. If 0.080 L of an HCl solution with a concentration of 1.10 M is added to this solution, what will the pH of the combined solution be? The pKa of the weak acid is 4.67.
When a solution contains a weak acid and its conjugate base or a weak base and...
When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base is...
500 mL OF 0.120 M NaOH IS ADDED TO 605 mL OF .200 M WEAK ACID...
500 mL OF 0.120 M NaOH IS ADDED TO 605 mL OF .200 M WEAK ACID (Ka= 4.39X10-5). WHAT IS THE PH OF THE RESULTING BUFFER. HA(aq) + OH-(aq) -------> H2O (L) + A-
You are titrating 0.200 L of a 0.400M monoprotic weak acid with a strong base that...
You are titrating 0.200 L of a 0.400M monoprotic weak acid with a strong base that is 0.800 M. Ka= 4.8x10^-6 a) At first, there is 0.200 L of 0.400M acid and no strong base. What is the pH? b) After 35.0 mL of 0.800 M strong base is added, what is the pH? c) How many mL of 0.800 M strong base must be added to reach the half equivalence point? d) What is the pH of the equivalence...
Given that Ka for the weak acid HA is 3.46 × 10–8, calculate K for the...
Given that Ka for the weak acid HA is 3.46 × 10–8, calculate K for the reaction of HA with OH–. HA(aq) + OH−(aq) ↔ A−(aq) + H2O(l)
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base...
± pH Changes in Buffers When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A−) is represented as HA(aq)⇌H+(aq)+A−(aq) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the addedH+, forming more...
If a buffer solution is 0.160 M in a weak acid (Ka = 3.4 × 10-5)...
If a buffer solution is 0.160 M in a weak acid (Ka = 3.4 × 10-5) and 0.510 M in its conjugate base, what is the pH? If a buffer solution is 0.260 M in a weak base (Kb = 6.9 × 10-5) and 0.550 M in its conjugate acid, what is the pH? Please show work that way it's actually learning and not just giving an answer. Thank you!