Titration

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    two of NaOH can sneak out before the valve is closed. Those few missed drops as well as excess NaOH in titration can affect the accuracy of the results. Human error is almost always a factor for example when measuring any values without digital assistance leaves room for the naked eye to make mistakes. As far as the second part of the experiment was, the 0.0025% deviation indicates that the titration was accurate. The ending molar mass (202.59 g/mol) of the mystery acid points to two…

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    (aq) + H2O(l) + C_8 H_4 O_4 〖^(2-)〗(aq) In this titration endpoint will not coincide with the equivalence point because at the equivalence point the color of the solution will be colorless and we cannot observe the endpoint, so, excessive drop of the base will color the solution to the pink and we consider it as the end point. The next titration with standard solution of NaOH with unknown concentration of HCl. The procedure is like previous titration of KHP with NaOH, but in this case instead of…

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    Volumetric Analysis Lab

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    this experiment was to determine the percent by mass of acetic acid within a sample of vinegar using volumetric analysis with the titration technique. The theory is that if the volume and molar concentration of the standardized sodium hydroxide (NaOH) solution is known, then the percent by mass of the acetic acid (CH3COOH) in vinegar can be calculated after a titration.1 Within this experiment, a NaOH solution was standardized with a primary standard acid of potassium hydrogen phthalate…

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    Add the unknown acid solution to each of the three beakers using the pipet. Next, add 50 mL of deionized water to each of the solutions. • Using figure 18.3 layout the titration apparatus in order to measure the pH of each of the solutions. Take the electrode placed in the deionized water and make sure to dry it with Kimwipes and place it in the beaker containing solution 1 and continue to stir the solution. Record the accurate…

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    fields), we picked the titration cartridge with a concentration of (1.600) and multiplier number (1.0), now we are ready to conduct the analysis. - We Draw about (110) ml of the unknown solution from the churn splitter (avoid…

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    Hydrochloric Acid

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    Introduction The objectives in this laboratory were to explore the titrations of several known acids and bases as well as observing the mole reactions of the chemical reactions that each compound undertook. The four following acids and bases were used to predict when a set amount of reactant would reach equilibrium: Hydrochloric Acid (HCl), H2SO4 (Sulfuric Acid), NaOH (Sodium Hydroxide), and Ba(OH)2 (Barium hydroxide). An unbalanced equation of each reaction was given so the balanced equation…

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    The Bronsted-Lowry Theory

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    point of the reaction, indicating that the concentration of the acid can be measured. The point of equivalence will result at a pH of seven in the titration of sulfuric acid and hydrochloric acid with sodium hydroxide. Aim: The aim of the experiment is to find the unknown concentrations of the acids (Sulfuric and Hydrochloric) with the use of titration, using 50 cm3 of 0.1 M solution of the base (NaOH) as a titrant. In addition, the measured volume of the base consumed is used to reach the end…

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    and water. The pH of water is 7, but salt does not have a pH and does not interact with water molecules.3 Therefore, the pH of the solution is 7, or neutral. To determine how much of a base is required to neutralize an acid, acid-base titration is used. A titration measures how much of a substance, titrant, with a known concentration is required to react completely with a substance, analyte, with a known volume.4 This is known as the equivalence point. Once the volume of the titrant is found,…

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    Ksp Of Reaction Lab Report

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    In the second part of the experiment, KHT was added to solutions of different potassium ion concentrations. Similar to the first part, the concentration of HC4H4O6- was calculated through titrations of 0.05 M KCl and 0.1 M KCl solutions with known NaOH concentrations. The total concentration of K+ for the solutions with the common ion is equal to the K+ concentrations from the KCl solutions and the K+ concentration from the KHT itself, which…

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    temprature which was found using the data logger. • The enthalpy change can then be calculated after all these values are found. Each trial can then be avaraged to find a more accurate result for our experiment. Conclusion and evaluation: The titration should be carried out carefully while making sure the color of the neutralized solution is the same for all the trials. This can be done by keeping the first sample aside that can be used for reference of the other trials can do this. The…

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