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- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Chem_51/16%3A_Acids_and_Bases/16.06_The_pH_ScalepH is a logarithmic function of [H+]. [H+] can be calculated directly from pH. pOH is related to pH and can be easily calculated from pH.
- https://chem.libretexts.org/Courses/Valley_City_State_University/Chem_122/Chapter_6%3A_Acids_and_Bases/6.5%3A_The_pH_of_Solutions_of_Weak_BasesThe pH of a solution of a weak base can be calculated in a way which is very similar to that used for a weak acid. Instead of an acid constant Ka, a base constant Kb must be used.
- https://chem.libretexts.org/Courses/Lansing_Community_College/LCC%3A_Chem_151_-_General_Chemistry_I/Text/04%3A_Reactions_in_Aqueous_Solution/4.3%3A_Acid-Base_ReactionsAn acidic solution and a basic solution react together in a neutralization reaction that also forms a salt. Acid–base reactions require both an acid and a base. In Brønsted–Lowry terms, an acid is a s...An acidic solution and a basic solution react together in a neutralization reaction that also forms a salt. Acid–base reactions require both an acid and a base. In Brønsted–Lowry terms, an acid is a substance that can donate a proton and a base is a substance that can accept a proton. Acids also differ in their tendency to donate a proton, a measure of their acid strength. The acidity or basicity of an aqueous solution is described quantitatively using the pH scale.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Foundations_of_Introductory_Chemistry-1/1.12%3A_Acids_and_Bases/16.6_The_pH_ScalepH is a logarithmic function of [H+]. [H+] can be calculated directly from pH. pOH is related to pH and can be easily calculated from pH.
- https://chem.libretexts.org/Courses/Northern_Alberta_Institute_of_Technology/CHEM1130_Principles_in_Chemistry_I/5%3A_Acids%2C_Bases%2C_and_pH/5.4%3A_pH_and_pOHThe concentration of hydronium ion in a solution of an acid in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greate...The concentration of hydronium ion in a solution of an acid in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of H3O+ in a solution can be expressed as the pH of the solution; \(\ce{pH} = -\log \ce{H3O+}\). The concentration of OH− can be expressed as the pOH of the solution: \(\ce{pOH} = -\log[\ce{OH-}]\). In pure water, pH = 7 and pOH = 7.
- https://chem.libretexts.org/Courses/City_College_of_San_Francisco/CCSF_Chemistry_Resources/01%3A_CHE_101_-_Introduction_to_General_Chemistry/1.05%3A_Acid-Base_Equilibria/1.5.01%3A_pH_and_pOHThe concentration of hydronium ion in a solution of an acid in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greate...The concentration of hydronium ion in a solution of an acid in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greater than \( 1.0 \times 10^{-7}\; M\) at 25 °C. The concentration of H3O+ in a solution can be expressed as the pH of the solution; \(\ce{pH} = -\log \ce{H3O+}\). The concentration of OH− can be expressed as the pOH of the solution: \(\ce{pOH} = -\log[\ce{OH-}]\). In pure water, pH = 7 and pOH = 7.
- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/6%3A_Equilibrium_Chemistry/6.10%3A_Using_Excel_and_R_to_Solve_Equilibrium_ProblemsIn solving equilibrium problems we typically make one or more assumptions to simplify the algebra. These assumptions are important because they allow us to reduce the problem to an equation in x that ...In solving equilibrium problems we typically make one or more assumptions to simplify the algebra. These assumptions are important because they allow us to reduce the problem to an equation in x that we can solve by simply taking a square-root, a cube-root, or by using the quadratic equation. Without these assumptions, most equilibrium problems result in a cubic equation (or a higher-order equation) that is harder to solve. Both Excel and R are useful tools for solving such equations.
- https://chem.libretexts.org/Under_Construction/Purgatory/CHEM_2100%3A_General_Chemistry_I_(Mink)/14%3A_Acid-Base_Equilibria/14.02%3A_pH_and_pOHThe concentration of hydronium ion in a solution of an acid in water is greater than 1.0×10⁻⁷M at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greater than 1.0×10⁻⁷M M...The concentration of hydronium ion in a solution of an acid in water is greater than 1.0×10⁻⁷M at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greater than 1.0×10⁻⁷M M at 25 °C. The concentration of H₃O⁺ in a solution can be expressed as the pH of the solution; pH=−log H₃O⁺. The concentration of OH⁻ can be expressed as the pOH of the solution: pOH=−log[OH⁻].
- https://chem.libretexts.org/Courses/Northern_Alberta_Institute_of_Technology/CHEM1130_Principles_in_Chemistry_I/5%3A_Acids%2C_Bases%2C_and_pH/5.5%3A_The_pH_of_Solutions_of_Weak_AcidsThis section details how to find the pH of weak acid solutions.
- https://chem.libretexts.org/Courses/Harper_College/CHM_110%3A_Fundamentals_of_Chemistry/04%3A_Water/4.18%3A_The_pH_ScalepH is a logarithmic function of [H+]. [H+] can be calculated directly from pH. pOH is related to pH and can be easily calculated from pH.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/14%3A_Ionic_Equilibria_in_Aqueous_Solutions/14.05%3A_The_pH_of_Solutions_of_Weak_BasesThe pH of a solution of a weak base can be calculated in a way which is very similar to that used for a weak acid. Instead of an acid constant Ka, a base constant Kb must be used.
