____________ INTRODUCTION Monitoring the pH range of a laboratory reaction or a process is very important. It is important to keep the pH almost constant even when addition of acids or bases takes place. One can easily know if a solution is an acid or a base using a visual indicator. Indicators are organic dye added to a solution that changes color base on the concentration of H3O ions in the solution. Each color change corresponds into a pH value. Common indicators used in the laboratory
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temperature‚ the pH‚ the turbidity‚ the conductivity‚ and the dissolved oxygen (A.K.A. DO) (1). Those are the focus of this study. Temperature and dissolved oxygen are both related to each other. The dissolved oxygen is inversely proportional to the temperature of the water. Anything decaying in the water will decrease the dissolved oxygen. A value less than 5 mg/L of dissolved oxygen is hard on the fish. When the dissolved oxygen has a value less than 2 mg/L‚ the fish will die (1). pH helps not
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Mass of Filter ▪ Height ▪ Timer ▪ Position ▪ Orientation of Filter • Materials: o 1 Coffee Filter o 1 Timer o 1 Meter Stick o 1 Ruler o 1 Tape • Procedure: I. Measure 1.5 meters off the ground and place tape on the wall to mark the height II. Grab the coffee filter and drop it from the measured height III. Measure and Record the time it takes for the coffee filter to
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suitable reference electrode and a sensitive potentiometer (a pH meter) may be advantageous. THEORY Any acid-base titration may be conducted potentiometrically. Two electrodes‚ after calibration [to relate potential in millivolts (mV) to a pH value] are immersed in a solution of the analyte. One is an indicator electrode‚ selective for H3O+ and the other a stable reference electrode. The potential difference‚ which after calibration is pH‚ is measured after the successive addition of known increments
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LAB 6. ACIDS AND BASES: PH AND BUFFERS PURPOSE: To determine the pH of common acids and bases using a pH meter‚ pH paper‚ and red cabbage indicator. To test the effect of adding an acid or base to a buffer solution. SAFETY CONCERNS: Always wear safety goggles. Wash with soap and water if skin contacts acids or bases. ACIDS: An Acid is a substance that when dissolved in water will produce hydrogen ions‚ H+‚ in the solution. An acid that does not contain carbon is called an inorganic
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acid-base titration can be detected by the use of a pH indicator‚ a pH meter‚ or a conductance meter. The use of a pH meter to quantitatively determine the end point of a titration reaction is preferred to the use of visual indicator. This is because the pH meter monitors the change in pH at the equivalence point rather than just observing the color change in the visual indicator‚ and this eliminates the indicator blank errors. The use of a pH indicator is often regarded as tedious as compared to
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Full Lab Report Experiment #2: Acid-Base Titration Lab Description: Acid-Base Titration Introduction In this lab exercise we will evaluate the effectiveness of several indicators for the determination of the point of completion of a specific acid-base neutralization reaction. We will also determine the unknown concentration of the strong base NaOH by its reaction with a known amount of the weak acid‚ potassium acid phtalate (HKC8H4O4‚ abbreviated KHP). This will be accomplished using the titration
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Introduction Acids and bases is an important aspect in chemistry. A specific example of such is in the body‚ acids and bases have to be balanced in order to provide the optimal pH in the system for normal physiological processes. Anything digested by the body has the ability to change the body’s standard (or current) pH. A pH of the body which is too acidic or too basic can lead to problems with one’s health1. An example of acid excess is hydrochloric acid in the stomach‚ causing someone to have acid
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Determining the equilibrium constant from pH values of changing concentrations of ethanoic acid Design Research question: How will altering the concentrations of ethanoic acid affect the pH value‚ and‚ in-turn‚ the equilibrium constant? Background information: When weak acids react‚ the reaction typically does not go to completion. Rather‚ the system goes to an intermediate state in which the rates of the forward and reverse reactions are equal. Such a system is said to be in chemical equilibrium
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phosphate solution using a pH meter and construct a titration curve of an amino acid to determine the pka values of its ionisable groups to identitfy an unknown amino acid. Method: The ratio of [HPO42-] to [H2PO4-] required to produce buffer solutions at pH values 5.9‚ 6.9 and 7.9 were calculated. 0.1M of H2PO4- and 0.1M HPO42- were used to mix appropriate volumes to 25mL of each of the buffer solutions. The calibrated pH meter was used to measure and record the pH of each buffer solution and
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