$referrer_host = www.google.com. Buffer Solutions Practice Problems - Chemistry Steps

General Chemistry

This is a summary practice problem set on buffer solutions aimed to help identify buffers, calculating the pH of a buffer solution prepared from a weak acid and its conjugate base or vice versa.

The links to the corresponding topics are given below:

Practice

1.

Which of the following solutions can be classified as buffer solutions?

(a) NaBr + HBr, (b) NaHSO4 + H2SO4, (c) HCl + HOCl (d) Na2HPO4 + NaH2PO4, (e) CH3CH2NH2 + CH3CH2NH3+ (f) NaNO2 + HNO2, (g) KCN + HCN, (h) Na2SO4 + NaHSO4, (i) NH3 + NH4ClO3, (j) CH3CO2H + NaOH.

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2.

Addition of which salt will suppress the ionization of HOCl?

  1. Na2SO4
  2. KNO3
  3. NaOCl
  4. NaNO2
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3.

A solution of ammonia and ammonium chloride is a common buffer system. Write the corresponding reactions to show how it resists a pH change when an acid or a base is added to it.

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4.

Calculate the pH of the buffer solution consisting of 0.75 M NH3 and 0.95 M NH4Cl. Kb (NH3) = 1.8 x 10-5.

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5.

Calculate the pH of the buffer solution which is 1.4 M CH3COONa and 1.8 M CH3COOH. Ka (CH3CO2H) = 1.7 x 10-5

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6.

Calculate the pH of the buffer solution that is 0.70 M NaCN and 0.55 M HCN. Ka (HCN) = 4.9 x 10-10

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7.

Calculate the pH of the buffer solution that is 0.60 M propionic acid (CH3CH2CO2H) and 0.75 M sodium propionate. Ka (CH3CH2CO2H) = 1.32 x 10-5

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8.

What is the pH of a buffer solution that is 0.85 M pyridine (C5H5N) and 1.3 M pyridinium chloride (C5H5NHCl)? Kb (C5H5N) = 1.7 x 10-9 16.82

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9.

Calculate the pH of a solution that is 0.8 M HF and 2.0 M NaF. Ka (HF) = 6.6 x 10-4

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10.

Calculate the ratio of NaNO2 to HNO2 required to create a buffer with pH = 4.00. Ka (HNO2 = 7.2 x 10-4)

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11.

Assuming no volume change, how many grams of sodium benzoate (C7H5O2Na) needs to be added to 250.0 mL of a 0.25 M benzoic acid (C7H5O2H) solution to prepare a buffer with a pH of 4.60? Ka = 6.46 x 10-5

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12.

How many mL of 0.60 M HF and 0.70 M NaF must be mixed to prepare 1.00 L of a buffer solution at pH of 4.2? pKa HF = 3.8

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13.

What is the concentration of C6H5NH3Cl in the buffer solution with a pH of 4.3 containing 0.50 M C6H5NH2? Kb (C6H5NH2) 3.8 x 10-10

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14.

Which of the following pairs is the best choice to prepare a buffer with pH = 3.2 ?

In what mass ratio would you add the components to prepare the buffer.

a) CH3COOH and CH3COONa b) HNO2 and KNO2 c) NH3 and NH4Cl d) C5H5N and C5H5NHCl.

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15.

What would be the pH of a buffer solution composed of 0.60 M NH3/0.45 M NH4Cl after 0.010 mole of gaseous HCl is added to a 400.0 mL solution?

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16.

Calculate the pH after 20.0 g NaOH(s) is added to 1.0 L of a buffer solution containing 1.80 M acetic acid and 1.50 M sodium acetate at pH 4.0.

 

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