Calculate the pH of 0.100 L of the buffer 0.110 M CH3COONa/0.130 M CH3COOH before and...

Calculate the pH of 0.100 L of the buffer 0.110 M CH3COONa/0.130 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.)

(a) pH of the starting buffer:

(b) pH after addition of 0.0030 mol HCl:

(c) pH after addition of 0.0040 mol NaOH (added to a fresh solution of the starting buffer):

Expert Solution

no of moles of CH3COONa = molarity * volume in L
                           = 0.11*0.1 = 0.011moles
no of moles of CH3COOH   = molarity * volume in L
                           = 0.13*0.1 = 0.013 moles
   PKa = 4.75 for CH3COOH
    PH = PKa + log[CH3COONa]/[CH3COOH]
        = 4.75+ log0.011/0.013
         = 4.75-0.0725 = 4.6775
b. no of moles of CH3COONa after addition of 0.003 moles of HCl = 0.011-0.003 = 0.008mole
   no of moles of CH3COOH after addtion of 0.003 moles of HCl   = 0.013+ 0.003 = 0.016moles
PH = Pka + log[CH3COONa]/[CH3COOH]
      = 4.75+ log0.008/0.016
      = 4.75-0.3010 = 4.449
c. no of moles of CH3COONa after addition of 0.004 moles of NaOH = 0.011+0.004 = 0.015mole
   no of moles of CH3COOH after addtion of 0.004 moles of NaOH   = 0.013- 0.004 = 0.009moles
PH = Pka + log[CH3COONa]/[CH3COOH]
      = 4.75+ log0.015/0.009
      = 4.75+0.2218 = 4.9718

queen_honey_blossom answered 2 years ago

Calculate the pH of 1.00 L of a buffer 0.98 M CH3COONa/0.92 M CH3COOH before and...

Calculate the pH of 1.00 L of a buffer 0.98 M CH3COONa/0.92 M CH3COOH before and after the addition of the following species A. pH of starting buffer: B. pH after addition if 0.040 mol NaOH: C. pH after further addition if 0.101 mol HCl

Calculate the pH of 1.00 L of the buffer 1.06 M CH3COONa/1.09 M CH3COOH before and...

Calculate the pH of 1.00 L of the buffer 1.06 M CH3COONa/1.09 M CH3COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.060 mol NaOH: (c) pH after further addition of 0.109 mol HCl:

Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa. a)...

Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa. a) Using the Henderson-Hasselbalch equation b) Making no assumptions about quantities (use the quadratic equation) c) Compare and explain your results in a) and b) d) What is the pH of a buffer system after the addition of 0.10 moles of gaseous HCl to a 1.0 L of the solution? Assume that the volume of the solution does not change when the HCl is added....

Calculate the theoretical buffer capability of 0.1 M CH3COOH/CH3COONa buffer at pH=4.74 and pH=6 (I don't...

Calculate the theoretical buffer capability of 0.1 M CH3COOH/CH3COONa buffer at pH=4.74 and pH=6 (I don't know does the pH value affect so I provide it anyway) pKa of acetic acid is 4.74 To calculate the buffer capability, meansure the change by adding 0.5mL of 1.0M HCl and by adding 0.5mL NaOH to 10 mL of buffer, the capability is then the determined as the molarity of the HCl or NaOH added to the buffer divided by the change of...

Calculate the PH of 1.00 L of a buffer that is 0.130 M HNO2 and 0.170...

Calculate the PH of 1.00 L of a buffer that is 0.130 M HNO2 and 0.170 M NaNO2. What is the PH of the same buffer after the addition of 1.00 mL of 12.0 M HCl. (pKa of HNO2 = 3.40). Original Buffer: After HCl is added:

Part A Calculate the pH of 0.100 L of a buffer solution that is 0.27 M...

Part A Calculate the pH of 0.100 L of a buffer solution that is 0.27 M in HF and 0.47 M in NaF. Express your answer using three significant figures. pH = SubmitMy AnswersGive Up Part B Calculate pH of the solution on addition of the following. 0.004 mol of HNO3 Express your answer using three significant figures. pH = SubmitMy AnswersGive Up Part C Calculate pH of the solution on addition of the following. 0.005 mol of KOH Express...

What is the pH change of a buffer that has 0.100 mol HC2H3O2 and 0.130 mol...

What is the pH change of a buffer that has 0.100 mol HC2H3O2 and 0.130 mol NaC2H3O2 in 1.00 L after 0.010 mol HCl added to it? pKa = 4.74

A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.130 M in NH4Br. Part...

A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.130 M in NH4Br. Part A : What mass of HCl can this buffer neutralize before the pH falls below 9.00? Part B: If the same volume of the buffer were 0.255 M in NH3 and 0.400 M in NH4Br, what mass of HCl could be handled before the pH falls below 9.00?

Consider the titration of a 25.0 mL sample of 0.100 M CH3COOH (Ka= 1.8e-5) with 0.130...

Consider the titration of a 25.0 mL sample of 0.100 M CH3COOH (Ka= 1.8e-5) with 0.130 M NaOH. Determine the pH after adding 4.0 mL of base beyond the equivalence point.

calculate the ph of 1.0 l of a buffer that is .01 m of HNO2 and...

calculate the ph of 1.0 l of a buffer that is .01 m of HNO2 and .15 m NaO2. what is the ph of the same buffer and after the additon of 1.0 l of 12m hcl (pka of HNO2 is 3.4)

Question