What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250...

What is the pH of the buffer solution that contains 2.2 g of NH4Cl in 250 mL of 0.12 NH3? Is the final pH lower than the pH of the 0.12 M ammonia solution?

Expert Solution

Calculate the concentration of NH4Cl in 250 ml solution ={2.2g *1000}/{53.5 *250} = 0.165 M

According to Henderson equation pOH = -logKb +log[conju.acid] / [base]

where Kb of ammonia solution = 1.8*10^-5

pOH = - log (1.8*10^-5 ) + log [0.165] /[0.12]

= 4.7448 + 0.1409= 4.88

∴pH = 14 - pOH

= 14 - 4.88

= 9.12

The pH of the solution at initial concentration pOH =√Kb * C

= √1.8*10^-5 * 0.12

= 1.469*10^-2

∴ pH = 14 -0.01469 = 13.985

Hence the final pH is lower than the original pH of the ammonia solution

queen_honey_blossom answered 2 years ago

What is the pH of a buffer solution that contains 0.350M pyruvic acid and 0.150M sodium...

What is the pH of a buffer solution that contains 0.350M pyruvic acid and 0.150M sodium pyruvate? Ka = 4.1x10^-3 Select one: A. 4.72 B. 2.82 C. 2.02 D. 2.76 What is the pH of a 100.0mL buffer solution that contains 0.215M acetic acid and 0.255M sodium acetate after 0.055 mmol HCl is added. Assume no volume change. Ka = 1.8x10^-5. Select one: A. 4.61 B. 4.87 C. 5.03 D. 5.48 Calculate the change in pH after 0.010 mole HCl...

A buffer is 0.10 M in NH3 and 0.10 M in NH4Cl. What is the pH...

A buffer is 0.10 M in NH3 and 0.10 M in NH4Cl. What is the pH of the solution after the addition of 10.0 mL of 0.20 M of HCl to 100.0 mL of the buffer?

a. Calculate the pH of a buffer that is prepared by completely dissolving 0.0401 g of NH4Cl in exactly 25.0 ml of a 0.020 Molar aqueous NH3 solution.

a. Calculate the pH of a buffer that is prepared by completely dissolving 0.0401 g of NH4Cl in exactly 25.0 ml of a 0.020 Molar aqueous NH3 solution.b. What is the pH after 5.0 mL of 0.020 M NaOH solution is added to 0.020 L of this buffer?

prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH ,...

prepare a 100 ml of pH 10 Buffer solution using NH4Cl (s) and concentrated NH4OH , the NH4OH molartiy is 18.1 M ? NH4OH is equal to NH3 (aq)

What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide...

What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide to 5.00 L of 0.200 M ammonia? Ka of ammonium is 5.8 x 10^-10 2) What is the pH of the buffer after 90.0mL of 2.00 M HCl are added? 3) What is the pH of the buffer if 15.00 g of NaOH is added to the original buffer solution?

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate...

What is the pH of a buffer solution made by dissolving 10 g of sodium acetate in 200 ml of 1M acetic acid? The Ka for acetic acid id 1.7*10-5. B. Calculate the pH of the solution if 10 ml of 0.100M HCl is added to the solution. C. What will the pH be if 5.00 ml of 0.150M NaOH was added to solution in B? D. Write the equation when an acid and a base are added to the...

Calculate the pH of the 0.250 M NH3/0.5 M NH4Cl buffer system. What is the pH...

Calculate the pH of the 0.250 M NH3/0.5 M NH4Cl buffer system. What is the pH after the addition of 2.0 mL of 0.250 M NaOH to 18.0 mL of the buffer solution? After adding 10 more mL of 0.25 M NaOH what is the pH?

What is the pH of buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00...

What is the pH of buffer system prepared by dissolving 10.70 grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make 1.000 L of solution? Kb = 1.80 x 10^-5 for NH3 Calculate the change in pH after addition of 50.0 mL of 0.15 M NaOH.

Calculate the pH of a solution that contains .03 g of NaH2PO4*H2O and .01 g of...

Calculate the pH of a solution that contains .03 g of NaH2PO4*H2O and .01 g of Na2HPO4*7H2O in 10 mLs.

Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl and 0.180...

Calculate the pH of 100.0 mL of a buffer that is 0.0850 M NH4Cl and 0.180 M NH3 before and after the addition of 1.00 mL of 5.50 M HNO3. Can you please do a step-by-step of how to solve this, paying special attention to how to get the Ka in the Henderson Hasselbalch Equation? That's the part I'm not understanding.

Question