Titration Essays

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    Titration Lab Report

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    The aim of this lab is to determine the concentration of a potassium hydrogen phthalate solution (HKC8O4H4) using acid‐base titration. Introduction: Titration is a technique that chemists use to determine the unknown concentration of a known solution (we know what chemical is dissolved, but not how much in a solution). Because we know what the chemical is, we know how it will react with other chemicals and we can use that reaction to determine the concentration of the solution by measuring the formation

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    This experiment is carried out to determine the percentage of calcium carbonate, CaCO3 in the toothpaste provided with the experimental technique known as back titration. A back titration is also known as indirect titration. A known mass of toothpaste is neutralised with a known concentration and volume of hydrochloric acid, HCl. The mixture is then further neutralised by a known concentration and volume of sodium hydroxide solution, NaOH to determine the number of mole of HCl that reacted with CaCO3

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    purpose of the “Titration of the Unknown Acid” lab is to determine how much of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows:

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    Acid Titration Lab Report

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    1 Experiment 7: Titration of an Antacid Objective: In this experiment, you will standardize a solution of base using the analytical technique known as titration. Using this standardized solution, you will determine the acid neutralizing power of a commercially available antacid tablet. Introduction An understanding of the properties of acids and bases is an essential part of understanding chemical reactions (see Tro, pp 167-171). In aqueous solutions, a compound that produces H+ ions upon dissolution

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    Introduction: The acid-base titration experiment is the use of a titrant, an analyte, and an indicator. Titration is the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change.1 The titrate is what is later released into a beaker or flask that is filled with the analyte and indicator. The color change happens because of the indicator

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    End point in this acid-base titration experiment refers to the point where the chemical reaction has reached its conclusion and no additional titrant should be added. The end point of this experiment can be obtained when the indicator used changes colour. For example colourless to light pink when phenolphthalein is used and red to orange and subsequently yellow when methyl orange is used. Equivalence point, also known as stoichiometric point in an acid-base titration refers to the point where the

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    determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3. To identify the unknown acid. 4. To determine acid dissociation constant, Ka and pKa for the unknown acid. Introduction: Titration process is used in an acid-base experiment in order to determine the concentrations of solutions of acids and bases. Through the titration process, we are able to identify physical changes to the mixture such as the colour change to indicate the end

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    The technique utilized in this experiment was titration and is used to determine the concentration of an unknown solution by reaction with a known concentration of solution. In a titration, the titrant is placed into the burette and the analyte poured into the conical flask using a pipette. Titration involves adding a small amount of titrant slowly to the analyte to achieve the equivalence point. The equivalence point is when the moles of standard soluton are same as the solution of unknown concentration

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    Unknown Acid Molarity

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    Introduction: The unknown acid molarity will be determining by titration method. Titration is a process depends on concentration of known solution to another solution until the solute in the another solution completely react. Standard solution is the solution of known concentration that used in titration. In this experiment, NaOH was the titrant (base) however, the two analyte which used were HCl and H2SO4. The chemical reaction equations are molecular and ionic molecular equation for (NaOH) and

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    Acetic Acid Concentration

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    Titration is an analytical method used in the laboratory to determine the concentration of an unknown solution using a solution of accurately known concentration referred as the standard solution. Since the volumes of both solutions and the concentration of

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    Weak Acid Lab

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    unknown weak acid lab was to use titration in order to determine the K_a for an unknown solid weak acid knowing only its molar mass. The previous laboratory experiment was performed in order to determine whether titration or dilution would yield more accurate K_a. It was determined that titration yielded more accurate results. This lab was performed by taking a sample of solid weak acid and dissolving it in water before titrating with the strong base NaOH. Titration is a technique in which a reagent

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    Antacids Lab Report

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    In this lab, two different titrations were performed with three different antacids to determine which brand is the most effective at the cheapest price. The antacids were ground up separately and approximately 0.2 grams of it was placed in a flask. Methyl Orange, an indicator, and a stir bar were added into the flask. The flask was then put on a stir plate which was under a buret with 0.1M hydrochloric acid. The acid was poured into the flask until there was a permanent pink colour. The acid was

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    formula, and determine the limiting reactant in its formation. A reaction between iron III chloride hexahydrate and potassium oxalate monohydrate produced 3.307g of potassium trioxalatoferrate (III) trihydrate with a 62.0 percent yield. A permanganate titration determined the average percent composition of oxalate was 53.3% with a 2.22% standard deviation. The percent composition revealed the compound’s empirical formula to be FeK3(C2O4)3•3H2O. Potassium oxalate proved to be the limiting reactant. Results

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    Benzoic Acid Lab Report

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    formation of new bonds between solute and solvent. Results Table1. Results for titration of benzoic acid with NaOH at 20◦C V(NaOH) ml V(C_6

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    Unknown Solid Acid

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    Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value. Eventually using the NaOH and the acid’s

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    Base Titration Lab

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    lab consisted of determining whether a certain liquid was an acid or base and experimenting with the pH of various substances when either acid or base was added to them. The lab was executed by using two different types of indicators as well as a titration in the end. The first indicator used was litmus paper. Through litmus paper, it is possible to decide whether a liquid is an acid or a base. By placing one slip of red litmus paper by one slip of blue litmus paper and dropping beads of the liquid

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    Objective The objective of the experiment was to measure and analyze the reaction rate of tert-butyl chloride with sodium hydroxide, and plot it in a graph in order to observe the rate. Procedure Part A- Measurement of the SN1 Reaction Rate of Tert-Butyl Chloride • 100 mL of a solution of propan-2-ol and water (1:1 ratio) were collected from a container provided by the instructor, and they were placed in a 250 mL Erlenmeyer flask, which was subsequently cork-stoppered. Afterwards, 150 mL of NaOH

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    Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have

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    1.2 Statistical Testing A –Correlation check between the Start measure and End measure for those given Calcium. When running a simple scatterplot diagram so as to visually check the correlation of start and end measure for calcium, it would appear that there is no obvious correlation. Calcium Correlationsa Starting Value End Value Starting Value Pearson Correlation 1 .602 Sig. (2-tailed) .065 N 10 10 End Value Pearson Correlation .602 1 Sig. (2-tailed) .065 N 10 10 a. Treatment type

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    The purpose of this experiment was to perform a Wittig reaction using two different methods: In method I, 250 mg aldehyde was mixed with 785 mg phosphonium salt in 5 M NaOH solvent. This mixture was stirred for thirty minutes and filter by vacuum filtration for the product. In method 2, 250 mg of aldehyde, 785 mg, benzyltriphenylphosphonium chloride, and 380 mg potassium phosphate tribasic were homogenize with a pestle and mortar. Vacuum filtration was also used in this method to attain the product

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