A buffer solution contains 0.259 M NaHSO3 and 0.459 M Na2SO3. If 0.0149 moles of hydrochloric...

A buffer solution contains 0.259 M NaHSO₃ and 0.459 M Na₂SO₃.

If 0.0149 moles of hydrochloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ?
(Assume that the volume does not change upon adding hydrochloric acid)

What is the pH?

No pKa was given

Please include work as well!

Expert Solution

queen_honey_blossom answered 10 months ago

A buffer solution contains 0.350 M NaHSO3 and 0.387 M Na2SO3. Determine the pH change when...

A buffer solution contains 0.350 M NaHSO3 and 0.387 M Na2SO3. Determine the pH change when 0.104 mol HNO3 is added to 1.00 L of the buffer. pH change = This is all the info that was given

A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia. If 0.0488 moles of...

A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia. If 0.0488 moles of nitric acid are added to 225 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding nitric acid.) pH =

A buffer solution contains 0.249 M ammonium bromide and 0.410 M ammonia. If 0.0196 moles of...

A buffer solution contains 0.249 M ammonium bromide and 0.410 M ammonia. If 0.0196 moles of nitric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding nitric acid) pH =

1. A buffer solution contains 0.257 M NaHCO3 and 0.498 M K2CO3. If 0.0231 moles of...

1. A buffer solution contains 0.257 M NaHCO3 and 0.498 M K2CO3. If 0.0231 moles of hydrochloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrochloric acid) pH = 1A. A buffer solution contains 0.303 M NaH2PO4 and 0.307 M Na2HPO4. If 0.0440 moles of potassium hydroxide are added to 250. mL of this buffer, what is the pH of...

A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia. If 0.0297 moles of...

A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia. If 0.0297 moles of potassium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding potassium hydroxide) pH = A buffer solution contains 0.382 M nitrous acid and 0.466 M potassium nitrite. If 0.0176 moles of hydrobromic acid are added to 150. mL of this buffer, what is the pH...

1) A buffer solution contains 0.356 M ammonium chloride and 0.396 M ammonia. If 0.0550 moles...

1) A buffer solution contains 0.356 M ammonium chloride and 0.396 M ammonia. If 0.0550 moles of hydroiodic acid are added to 250 ml of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding hydroiodic acid) pH=____ 2) A buffer solution contains 0.354 M NaH2PO4 and 0.393 M K2HPO4. If 0.0412 moles of sodium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting...

A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M...

A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M NH4Cl. (a) Write the net ionic equations to show how this buffer solution neutralizes the added H + and OH- . (b) Calculate the pH of this buffer solution.

A) A buffer solution contains 0.484 M KHCO3 and 0.314 M K2CO3. Determine the pH change...

A) A buffer solution contains 0.484 M KHCO3 and 0.314 M K2CO3. Determine the pH change when 0.126 mol NaOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = B) A buffer solution contains 0.335 M NH4Br and 0.313 M NH3 (ammonia). Determine the pH change when 0.072 mol KOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = C)...

a. A buffer solution contains 0.274 M NH4Br and 0.379 M NH3 (ammonia). Determine the pH...

a. A buffer solution contains 0.274 M NH4Br and 0.379 M NH3 (ammonia). Determine the pH change when 0.103 mol HBr is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = b. A buffer solution contains 0.432 M NaH2PO4 and 0.209 M K2HPO4. Determine the pH change when 0.113 mol KOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change =

0.5 L of a buffer solution contains 0.44 M acetic acid and 0.44 M NaCH3COO, and...

0.5 L of a buffer solution contains 0.44 M acetic acid and 0.44 M NaCH3COO, and has a pH of 4.74. What will the pH be if 0.20 mol of HCL is added to the solution?

Question