Reactivity 3.1.17—The pH of a buffer solution depends on both: • the pKa or pKb of its acid or base • the ratio of the concentration of acid or base to the concentration of the conjugate base or acid. Solve problems involving the composition and pH of a buffer solution, using the equilibrium constant.
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[N/A]Directly related questions
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EXM.1A.HL.TZ0.9:
Which of the following statements is correct when a 1.0 M NH4+/NH3 buffer (pH = 9.2) is diluted to 0.5 M with water?
I. The ability of the buffer to resist changes in pH when acids are added will decrease.
II. The ability of the buffer to resist changes in pH when bases are added will decrease.
III. The pH of the buffer will be equal to 7.
A. I and II onlyB. I and III only
C. II and III only
D. I, II and III
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EXM.1A.HL.TZ0.9:
Which of the following statements is correct when a 1.0 M NH4+/NH3 buffer (pH = 9.2) is diluted to 0.5 M with water?
I. The ability of the buffer to resist changes in pH when acids are added will decrease.
II. The ability of the buffer to resist changes in pH when bases are added will decrease.
III. The pH of the buffer will be equal to 7.
A. I and II onlyB. I and III only
C. II and III only
D. I, II and III
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EXM.2.HL.TZ0.2a:
Determine the ratio in which 0.1 mol dm–3 NaH2PO4 and 0.1 mol dm–3 Na2HPO4 should be mixed to obtain a buffer with pH= 7.8.
pKa NaH2PO4 = 7.20
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EXM.2.HL.TZ0.2a:
Determine the ratio in which 0.1 mol dm–3 NaH2PO4 and 0.1 mol dm–3 Na2HPO4 should be mixed to obtain a buffer with pH= 7.8.
pKa NaH2PO4 = 7.20
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EXM.2.HL.TZ0.a:
Determine the ratio in which 0.1 mol dm–3 NaH2PO4 and 0.1 mol dm–3 Na2HPO4 should be mixed to obtain a buffer with pH= 7.8.
pKa NaH2PO4 = 7.20
- EXM.2.HL.TZ0.2b: Suggest, giving your reasons, the effect of diluting the buffer 1/100 with water on its pH and...
- EXM.2.HL.TZ0.2b: Suggest, giving your reasons, the effect of diluting the buffer 1/100 with water on its pH and...
- EXM.2.HL.TZ0.b: Suggest, giving your reasons, the effect of diluting the buffer 1/100 with water on its pH and...
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19M.2.HL.TZ1.12b:
Enzymatic activity is studied in buffered aqueous solutions.
Calculate the ratio in which 0.1 mol dm−3 NaH2PO4 (aq) and 0.1 mol dm−3 Na2HPO4 (aq) should be mixed to obtain a buffer with pH = 6.10. Use section 1 of the data booklet.
pKa (NaH2PO4) = 7.20
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19M.2.HL.TZ1.b:
Enzymatic activity is studied in buffered aqueous solutions.
Calculate the ratio in which 0.1 mol dm−3 NaH2PO4 (aq) and 0.1 mol dm−3 Na2HPO4 (aq) should be mixed to obtain a buffer with pH = 6.10. Use section 1 of the data booklet.
pKa (NaH2PO4) = 7.20
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19M.2.HL.TZ1.12b:
Enzymatic activity is studied in buffered aqueous solutions.
Calculate the ratio in which 0.1 mol dm−3 NaH2PO4 (aq) and 0.1 mol dm−3 Na2HPO4 (aq) should be mixed to obtain a buffer with pH = 6.10. Use section 1 of the data booklet.
pKa (NaH2PO4) = 7.20
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19M.2.HL.TZ1.b:
Enzymatic activity is studied in buffered aqueous solutions.
Calculate the ratio in which 0.1 mol dm−3 NaH2PO4 (aq) and 0.1 mol dm−3 Na2HPO4 (aq) should be mixed to obtain a buffer with pH = 6.10. Use section 1 of the data booklet.
pKa (NaH2PO4) = 7.20
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19M.2.HL.TZ2.23b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.23b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.16b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.16b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
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19M.2.HL.TZ2.b:
Some antacids contain carbonates.
Determine the pH of a buffer solution which contains 0.160 mol dm−3 CO32− and 0.200 mol dm−3 HCO3−, using section 1 of the data booklet.
pKa (HCO3−) = 10.32
- 21M.1A.HL.TZ1.27: Which combination will produce an alkaline buffer in water? A. 0.10 mol NH3 and 0.05 mol...
- 21M.1A.HL.TZ1.27: Which combination will produce an alkaline buffer in water? A. 0.10 mol NH3 and 0.05 mol...
- 21M.1A.HL.TZ1.27: Which combination will produce an alkaline buffer in water? A. 0.10 mol NH3 and 0.05 mol...
- 21M.1A.HL.TZ1.27: Which combination will produce an alkaline buffer in water? A. 0.10 mol NH3 and 0.05 mol...
- 22M.2.HL.TZ2.7a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...
- 22M.2.HL.TZ2.7a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...
- 22M.2.HL.TZ2.a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...
- 22M.2.HL.TZ2.7a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...
- 22M.2.HL.TZ2.7a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...
- 22M.2.HL.TZ2.a(iii): Justify whether a 1.0 dm3 solution made from 0.10 mol NH3 and 0.20 mol HCl will form a buffer...