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- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/8%3A_Titrimetric_Methods/8.2%3A_Acid%E2%80%93Base_TitrationsAcid–base titrations, in which an acidic or basic titrant reacts with a titrand that is a base or an acid, is probably the most common titration used by students in laboratories. To understand the rel...Acid–base titrations, in which an acidic or basic titrant reacts with a titrand that is a base or an acid, is probably the most common titration used by students in laboratories. To understand the relationship between an acid–base titration’s end point and its equivalence point we must know how the pH changes during a titration. We will learn how to calculate a titration curve using the equilibrium calculations from Chapter 6.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.13%3A_Additional_ResourcesThe page provides a comprehensive list of references addressing various aspects of equilibrium chemistry. Topics covered include experimental determination of equilibrium constants, the impact of ioni...The page provides a comprehensive list of references addressing various aspects of equilibrium chemistry. Topics covered include experimental determination of equilibrium constants, the impact of ionic strength, solubility products, and buffer capacity. Historical perspectives on the field are also offered. Additionally, the list encompasses instructional strategies, simulations for teaching, and critiques of conventional approaches to equilibrium concepts.
- https://chem.libretexts.org/Courses/Los_Angeles_Trade_Technical_College/Analytical_Chemistry/2%3A_Analytical_Chemistry_2.0_(Harvey)/07%3A_Equilibrium_Chemistry/7.03%3A_Manipulating_Equilibrium_ConstantsWe will take advantage of two useful relationships when working with equilibrium constants. First, if we reverse a reaction’s direction, the equilibrium constant for the new reaction is simply the inv...We will take advantage of two useful relationships when working with equilibrium constants. First, if we reverse a reaction’s direction, the equilibrium constant for the new reaction is simply the inverse of that for the original reaction. Second, if we add together two reactions to obtain a new reaction, the equilibrium constant for the new reaction is the product of the equilibrium constants for the original reactions.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.03%3A_Manipulating_Equilibrium_ConstantsThe page elaborates on two principles regarding equilibrium constants: reversing a reaction inverts its equilibrium constant, and combining reactions involves multiplying their equilibrium constants. ...The page elaborates on two principles regarding equilibrium constants: reversing a reaction inverts its equilibrium constant, and combining reactions involves multiplying their equilibrium constants. An example and exercise demonstrate these principles. For the example, the equilibrium constant for a reaction is calculated by combining constants of related reactions, resulting in 0.10. In a similar exercise, the equilibrium constant for a different reaction is calculated to be approximately 31.
- https://chem.libretexts.org/Courses/Northern_Alberta_Institute_of_Technology/CHEM1130_Principles_in_Chemistry_I/4%3A_Chemical_Calculations/4.8%3A_UV/4.8%3A_UV%2F%2FVis_and_IR_SpectroscopyThe 1930s and 1940s saw the introduction of photoelectric transducers for ultraviolet and visible radiation, and thermocouples for infrared radiation. As a result, modern instrumentation for absorptio...The 1930s and 1940s saw the introduction of photoelectric transducers for ultraviolet and visible radiation, and thermocouples for infrared radiation. As a result, modern instrumentation for absorption spectroscopy became routinely available in the 1940s—progress has been rapid ever since. Frequently an analyst must select—from among several instruments of different design—the one instrument best suited for a particular analysis. In this section we examine several different instruments for mole
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/01%3A_Introduction_to_Analytical_Chemistry/1.03%3A_Common_Analytical_ProblemsTypical problems on which analytical chemists work include qualitative analyses (Is lead present in this sample ?), quantitative analyses (How much lead is present in this sample?), characterization a...Typical problems on which analytical chemists work include qualitative analyses (Is lead present in this sample ?), quantitative analyses (How much lead is present in this sample?), characterization analyses (What are the sample???s chemical and physical properties?), and fundamental analyses (How does this method work and how can it be improved?).
- https://chem.libretexts.org/Courses/Lakehead_University/Analytical_I/6%3A_Equilibrium_Chemistry/6.03%3A_Manipulating_Equilibrium_ConstantsWe will take advantage of two useful relationships when working with equilibrium constants. First, if we reverse a reaction’s direction, the equilibrium constant for the new reaction is simply the inv...We will take advantage of two useful relationships when working with equilibrium constants. First, if we reverse a reaction’s direction, the equilibrium constant for the new reaction is simply the inverse of that for the original reaction. Second, if we add together two reactions to obtain a new reaction, the equilibrium constant for the new reaction is the product of the equilibrium constants for the original reactions.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.11%3A_Some_Final_Thoughts_on_Equilibrium_CalculationsThe chapter discusses tools for evaluating system composition at equilibrium, highlighting the importance of selecting the appropriate tool based on the precision required. It emphasizes the need to i...The chapter discusses tools for evaluating system composition at equilibrium, highlighting the importance of selecting the appropriate tool based on the precision required. It emphasizes the need to include all relevant equilibrium reactions to prevent errors. It introduces computational programs like Visual Minteq and CurTiPot for modeling equilibria and the R package CHNOSZ for thermodynamic calculations in aqueous geochemistry.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.10%3A_Using_Excel_and_R_to_Solve_Equilibrium_ProblemsThe document discusses solving equilibrium problems in chemistry using tools like Excel and R, emphasizing the importance of simplifying assumptions to avoid complex equations. Excel's Solver function...The document discusses solving equilibrium problems in chemistry using tools like Excel and R, emphasizing the importance of simplifying assumptions to avoid complex equations. Excel's Solver function helps find polynomial roots and solve simultaneous equations, demonstrated with examples on solubility and pH calculations. R's uniroot command and custom functions can also solve these problems by iterating on solutions.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/10%3A_Spectroscopic_Methods/10.03%3A_UV_Vis_and_IR_SpectroscopyThe page discusses the evolution of color matching in spectroscopy, detailing the transition from Nessler's original method to modern photoelectric and infrared methods in the 1930s and 1940s. It then...The page discusses the evolution of color matching in spectroscopy, detailing the transition from Nessler's original method to modern photoelectric and infrared methods in the 1930s and 1940s. It then describes different instrument designs for molecular absorption spectroscopy, including filter photometers, single-beam and double-beam spectrophotometers, and diode array spectrometers, highlighting their features and limitations.
- https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Analytical_Chemistry_2.1_(Harvey)/06%3A_Equilibrium_Chemistry/6.06%3A_Ladder_DiagramsThe page discusses the importance of considering chemical interactions, like pH and solubility, when developing or evaluating analytical methods. It critiques the inappropriate use of NH3 in precipita...The page discusses the importance of considering chemical interactions, like pH and solubility, when developing or evaluating analytical methods. It critiques the inappropriate use of NH3 in precipitating AgCl due to its solubility-increasing effect. Key analytical errors often stem from overlooking chemical interferences. Ladder diagrams are introduced as tools for visualizing equilibrium chemistry, aiding in understanding reaction dynamics and evaluating changes in solution conditions.
