Question

Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of...

Using a 0.25 M phosphate buffer with a pH of 6.2, you add 0.70 mL of 0.50 M HCl to 49 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Ph= PKa+log[ concentration of buffer/ concentration of acid]

6.2 =6.86+ log[phsophate/ acid]

6.2-6.86= log [0.25/acid]

-0.66 =log [0.25/acid]

0.25/acid=10^(-0.66)

acid =0.25/0.218= 1.146M

moles of buffer in 49 ml = 0.25*49/1000 = 0.01225

moles of acid added = 0.5*49/1000 =0.0245

volume of the mixture= 49+0.7 =49.7 ml

Concentration of buffer = 0.01225/(49.7/1000)= 0.246278M

Concentration of acid = 0.0245*1000/49.7= 0.4929 M

Now pH= pka+ log [ 0.24627/0.4929]

pH= 6.86-0.30138=6,55

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. Using a 0.25 M phosphate buffer with a pH of 6.8, you add 0.79 mL...
1. Using a 0.25 M phosphate buffer with a pH of 6.8, you add 0.79 mL of 0.49 M HCl to 44 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) ________ 2. Using a 0.25 M phosphate buffer with a pH of 6.8, you add 0.79 mL of 0.49 M NaOH to 44 mL of the buffer. What is the new pH of the solution? (Enter your answer to...
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.8, you add 0.72 mL of 0.50 M HCl to 53 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.30 M phosphate buffer with a pH of 6.4, you add 0.75 mL of...
Using a 0.30 M phosphate buffer with a pH of 6.4, you add 0.75 mL of 0.49 M HCl to 46 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) WebAssign will check your answer for the correct number of significant figures. Incorrect: Your answer is incorrect. Using a 0.30 M phosphate buffer with a pH of 6.4, you add 0.75 mL of 0.49 M NaOH to 46 mL of...
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.80 mL of...
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.80 mL of 0.50 M NaOH to 60. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of 0.46 M HCl to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.71 mL of...
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.71 mL of 0.51 M HCl to 50. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of...
Using a 0.20 M phosphate buffer with a pH of 7.6, you add 0.72 mL of 0.46 M NaOH to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
A) Need to prepare 100 ml of a 0.10 M phosphate buffer with a pH of...
A) Need to prepare 100 ml of a 0.10 M phosphate buffer with a pH of 6.2. Calculate the amounts of 1.0 M NaH2PO4 and 1.0 M K2HPO4 solutions which will give the required pH of 6.2.Use the Henderson-Hasselbalch equation ( pH = pKa + log (base/acid) B) Need to prepare 100 ml of a solution containing 0.025 M NaHCO3 and 0.12 M NaHCO3 and 0.12 M NaCl From stock solutions of 0.05 M NaHCO3 and 0.24 M NaCl from...
2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without...
2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without a significant pH change. It is governed by the concentrations of the conjugate acid and base forms of the buffer. A 0.5 M buffer will require five times as much acid or base as a 0.1 M buffer for given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity...
How would you prepare 1 L of a 0.100 M phosphate buffer at pH 7.02 using...
How would you prepare 1 L of a 0.100 M phosphate buffer at pH 7.02 using crystalline Na2HPO4 and a solution of 1.0 M HCl?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT