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- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/14%3A_Ionic_Equilibria_in_Aqueous_Solutions/14.08%3A_Buffer_SolutionsBuffers allow chemists to maintain a specific pH range for a reaction. Buffers utilize conjugate acid-base pairs to function. Read on to learn more about the specifics and calculations of buffers.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_331_-_Organic_Chemistry_(Lund)/09%3A_Introduction_to_Acid-base_Reactions/9.02%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Courses/Smith_College/CHM_222_Chemistry_II%3A_Organic_Chemistry_(2025)/11%3A_Carboxylic_Acids_and_Nitriles/11.04%3A_Biological_Acids_and_the_Henderson-Hasselbalch_Equation_(reference_only)use the Henderson-Hasselbalch equation to calculate the percentages of dissociated and undissociated acids [A − ] and [HA] in a solution, given the pK a value of the acid and the pH of the solution. A...use the Henderson-Hasselbalch equation to calculate the percentages of dissociated and undissociated acids [A − ] and [HA] in a solution, given the pK a value of the acid and the pH of the solution. Also, the Henderson-Hasselbalch allows for the pH of the solution to be calculated when the pK a of the acid is known along with the concentrations of the carboxylic acid and carboxylate are known.
- https://chem.libretexts.org/Courses/Stanford_Online_High_School/TEN2A-Acids/03%3A_Buffers/3.01%3A_Buffered_SolutionsBuffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (HA) and its conjugate weak base (A−). Adding a strong electrolyte that contains o...Buffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (HA) and its conjugate weak base (A−). Adding a strong electrolyte that contains one ion in common with a reaction system that is at equilibrium shifts the equilibrium in such a way as to reduce the concentration of the common ion. Buffers are characterized by their pH range and buffer capacity.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_(Morsch_et_al.)/24%3A_Amines_and_Heterocycles/24.05%3A_Biological_Amines_and_the_Henderson-Hasselbalch_EquationThe Henderson-Hasselbalch equation is very useful relating the pKa of a buffered solution to the relative amounts of an acid and its conjugate base.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_332_--_Organic_Chemistry_II_(Lund)/7%3A_Acid-base_Reactions/7.2%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_333_-_Organic_Chemistry_III_(Lund)/New_Page/7%3A_Acid-base_Reactions/7.2%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Courses/SUNY_Oneonta/Organic_Chemistry_with_a_Biological_Emphasis_(SUNY_Oneonta)/07%3A_Acid-base_Reactions/7.03%3A_The_Acidity_ConstantYou are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a comm...You are no doubt aware that some acids are stronger than others. The relative acidity of different compounds or functional groups – in other words, their relative capacity to donate a proton to a common base under identical conditions – is quantified by a number called the acidity constant, abbreviated K
- https://chem.libretexts.org/Workbench/LCDS_Organic_Chemistry_OER_Textbook_-_Todd_Trout/24%3A_Amines_and_Heterocycles/24.06%3A_Biological_Amines_and_the_Henderson-Hasselbalch_EquationWe saw in Section 20.3 that the extent of dissociation of a carboxylic acid HA in an aqueous solution buffered to a given pH can be calculated with the Henderson–Hasselbalch equation. [RNH 2 ] = (4 .6...We saw in Section 20.3 that the extent of dissociation of a carboxylic acid HA in an aqueous solution buffered to a given pH can be calculated with the Henderson–Hasselbalch equation. [RNH 2 ] = (4 .6 × 10 –4 )[RNH 3 + ] l og [RNH 2 ] [RNH 3 + ] = pH – p K a = 7 .3 – 10 .64 = –3 .34 [RNH 2 ] [RNH 3 + ] = antilog(–3 .34) = 4 .6 × 10 –4 In other words, at a physiological pH of 7.3, essentially 100% of the methylamine in a 0.0010 M solution exists in its protonated form as methylammonium ion.
- https://chem.libretexts.org/Courses/Thompson_Rivers_University/TRU%3A_Fundamentals_and_Principles_of_Chemistry_(CHEM_1510_and_CHEM_1520)/07%3A_Buffers_Titrations_and_Solubility_Equilibria/7.02%3A_Practical_Aspects_of_BuffersBuffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (HA) and its conjugate weak base (A−). Adding a strong electrolyte that contains o...Buffers are solutions that resist a change in pH after adding an acid or a base. Buffers contain a weak acid (HA) and its conjugate weak base (A−). Adding a strong electrolyte that contains one ion in common with a reaction system that is at equilibrium shifts the equilibrium in such a way as to reduce the concentration of the common ion. Buffers are characterized by their pH range and buffer capacity.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_III_(Morsch_et_al.)/24%3A_Amines_and_Heterocycles/24.05%3A_Biological_Amines_and_the_Henderson-Hasselbalch_Equationuse the Henderson‑Hasselbalch equation to calculate the percentage of a base that is protonated in a solution, given the pK a value of the associated ion and the pH of the solution. The values in the ...use the Henderson‑Hasselbalch equation to calculate the percentage of a base that is protonated in a solution, given the pK a value of the associated ion and the pH of the solution. The values in the Henderson-Hasselbalch can be used for an amine with the ammonium salt written as, HA = RNH 3 + , and the amine as being, A - = RNH 2 . With an approximate pK a of 10.8 for the protonated amine HA, it should be >99% protonated, in the positively-charged, ammonium form:
