# Henderson-Hasselbalch

posted by .

If the same volume (130-mL) of the buffer were 0.265 M in NH3 and 0.400 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?

I used the henderson-hasselbalch equation to solve this. i set it up as 9=9.24551+log((0.03445-x)/(0.052+x))

0.03445= moles of NH3
0.052= moles of NH4Br

I calculated the grams to be .11 g but it was wrong. Did i set up my H-H equation wrong?

• Chemistry -

Assistance needed.

Please type your subject in the School Subject box. Any other words, including obscure abbreviations, are likely to delay responses from a teacher who knows that subject well.

• Henderson-Hasselbalch -

See above for my response.

• Henderson-Hasselbalch -

The x is small approximation doesn't work for this problem, so you have to set up an ICE table to solve for the amount of HCl, you can't use the H-H

## Similar Questions

1. ### Science- Chemistry

How many grams of sodium acetate( molar mass 82.03 g/mol) must me added to 1.00L of a 0.200M acetic acid solution to form a buffer of 4.20?
2. ### Chemistry

If the same volume (130-mL) of the buffer were 0.265 M in NH3 and 0.400 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
3. ### chem

A 120.0 mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4Br, What mass of HCl could this buffer neutralize before the pH fell below 9.00?
4. ### Chemistry

A beaker with 200 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 6.40 mL of a 0.400 \it M \rm HCl solution to the beaker. …
5. ### Chemistry

How many grams of glycine amide (FM 74.08) should be used with 1.0 gram of glycine amide HCl (FM 110.54, pKa=8.20) to give 100 mL at pH 8.0?
6. ### chemistry

A 130.0 mL buffer solution is 0.100 M in NH3 amd 0.135 M in NH3 and 0.135 M in NH4Br. What mass of HCI could this buffer neutralize before the pH fell below 9.00?
7. ### chemistry

use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution prepared by mixing equal volumes of 0.20 M NaHCO3 and 0.10M Na2CO3.(Ka=5.6x10^-11). how would you prepare NaHCO3-Na2CO3 buffer solution that has the pH …
8. ### chem

calculate the pH in a solution prepared by dissolving .10 mol of solid NH4Cl in .500 L of .40 M NH3. Assuming no volume change. Without the use of Henderson-hasselbalch
9. ### Chemistry

Four sets of conjugate acid/base pairs and Ka of the acid are given. Which pair would be the best to form a buffer at pH = 9.2?
10. ### chemistry

anyone know how to do this and which choice is correct?

More Similar Questions