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Concept explainers
(a)
Interpretation:
The acid-base pair to form a buffer solution of pH 4.0 needs to be determined.
Concept introduction:
A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example, the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation
Also known as Henderson-Hasselbalch equation.
(b)
Interpretation:
The acid-base pair to form a buffer solution of pH 9.2 needs to be determined.
Concept introduction:
A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example, the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation
Also known as Henderson-Hasselbalch equation.
(c)
Interpretation:
The acid-base pair to form a buffer solution of pH 11 needs to be determined.
Concept introduction:
A buffer is a solution which resists change in pH on addition of small amount of acid or base. A buffer is prepared by mixing a weak acid with its conjugate base ion or a weak base and its conjugate acid ion.
For example, the mixture of acetic acid and its conjugate base acetate ion will form a buffer solution.
The pH of a buffer solution is determined with the following equation
Also known as Henderson-Hasselbalch equation.
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Chapter 14 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?arrow_forwardConsider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+ X2(aq)Ka2=9.7 10 8 Calculate the pH of the solution and estimate [HX-] and [X2-].arrow_forwardCalculate the hydrogen ion concentration in mol/l for solutions with the following ph values: (a) 2.42 (b) 11.21 (c) 6.96 (d) 15.00arrow_forward
- (a) 33. Which one of the following statements regarding acid-base property is NOT correct? pH + pOH = 14, for all aqueous solutions The pH of 108 (M) HCl solution is 8 The conjugate base of H₂PO4 is HPO4 ²- H₂SO4 is a strong acid in aqueous solution (b) (c) (d)arrow_forwardCalculate the molar H3O+ion concentration of a solution that has a pH of (A) 4.31 (B) 13.89 (C) 5.32 (D) 4.48arrow_forwardAcidity of a solution is determined by the concentration H of hydrogen ions in the solution (measured in moles per liter of solution). Chemists use the negative of the logarithm of the concentration of hydrogen ions to define the pH scale, as shown in the following formula. pH = -log (H) Lower pH values indicate a more acidic solution. (a) Normal rain has a pH value of 5.6. Rain in the eastern United States often has a pH level of 3.8. How much more acidic is this than normal rain? (Round your answer to two decimal places.) 63.10 times as acidic as normal rain (b) If the pH of water in a lake falls below a value of 5, fish often fail to reproduce. How much more acidic is this than normal water with a pH of 5.6? (Round your answer to two decimal places.) * times as acidic as normal waterarrow_forward
- The pH scale for acidity is defined by pH – log10 H*| where |H*| is the concentration of hydrogen ions measured in moles per liter (M). (A) The pH of Drano is 13.3. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = M (B) The pH of rain water is 5.5. Calculate the concentration of hydrogen ions in moles per liter (M). [H*] = Marrow_forward83. Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 = 4.2 (b) pOH (c) POH = 1.7 (d) pOH = 7.0arrow_forwardThe pH of a chemical solution is given by theformula pH = - log10 [H+ ] where [H+ ] is the concentration of hydrogen ions in molesper liter. Values of pH range from 0 (acidic) to 14 (alkaline).(a) What is the pH of a solution for which [H+ ] is 0.1?(b) What is the pH of a solution for which [H+ ] is 0.01?(c) What is the pH of a solution for which [H+ ] is 0.001?(d) What happens to pH as the hydrogen ion concentration decreases?(e) Determine the hydrogen ion concentration of an orange (pH = 3.5).(f) Determine the hydrogen ion concentration of human blood (pH = 7.4).arrow_forward
- 6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.arrow_forwardWhich of the following reactions is an acid-base reaction? A) AGNO:(aq) + KF(aq) → AgF(s) + KNO:(aq) B) NH:(aq) + HF(aq) → NH:"(aq) + -F(aq) C) NO: (aq) + AI(s) → NH3(g) + AIO: (aq) D) CH:(g) + 202(g) - 2H:O(g) + CO:(g)arrow_forwardWhat is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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