• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Lab Report - What volume of concentrated 12N HCl is required to prepare 250 cm3 of 5N HCl solution?

Extracts from this document...

Introduction

Chemistry What volume of concentrated 12N HCl is required to prepare 250 cm3 of 5N HCl solution? Lab Report Experimental Design Aspect 1 Variables Responding Variables - 1. Normality of HCl solution - 12N Controlled Variables - 1. Volume of 5N HCl solution to be prepared - 250 cm3 2. Volume of 12N solution required - 104.16 cm3 Aspect 2 Hypothesis M1*V1 = M2*V2 So, V1 = (M2*V2) / M1 V1 = (5 * 250) / 12 Thus, V1 = 104.16 cm3 Therefore, 104.16 cm3 of 12N HCl is required to prepare 250 cm3 of 5N HCl solution. Aspect 3 Controlling Variables 1. Use a parallax card while measuring the amount of concentrated HCl in order to avoid any sort of error. ...read more.

Middle

Accurately measure out 104.2cm3 of 12N concentrated HCl in a measuring cylinder. 2. Take approximately around 100-120 cm3 of distilled water in the 500 cc beaker and add 104.2 cm3 of Concentrated 12N HCl carefully. Glass rod must be used for stirring. Gloves must be used along with safety goggles as a step of precaution. 3. Cool the beaker when it gets hot under the tap water from time to time and transfer the solution to the 250 cm3 measuring flask. 4. Add the remaining amount of distilled water using the wash bottle to get accurate results. 5. When the water level of the measuring flask reaches the 250 cm3 mark, shake the solution well so that the solution becomes uniform. ...read more.

Conclusion

5N HCl solution to be prepared 250 Conclusion and Evaluation Aspect 1 Conclusion Therefore, in order to prepare 5N HCl we require 104.16 cm3 of 12N HCl. Aspect 2 Evaluating Procedures * Percentage errors- Percentage error= Uncertainty*100/True Value * Volume of 12N concentrated HCl solution = 00.05 * 100 (Measuring flask) 104.5 = 0.049% * Volume of 5N HCl solution made = 00.05 * 100 (Measuring flask) 250 = 0.02% ? Total uncertainty = 0.069% Aspect 3 Improving the Investigation * All the utensils should be washed properly to remove the uncertainty. * Every time use a fresh sample of the chemicals. * Use tested equipments with the least amount of uncertainty. * Make sure you do the experiment carefully to avoid the manual errors. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Change of Potential Difference in Voltaic Cells Lab Report

    It has two main sections: the copper sulfate solution's concentrations (M) and the experimental voltage (the experiment's +results).Another similar data table can be developed for the second and third trials of the experiment. Trial 1 Trial 2 Trial 3 Copper Sulfate Concentrations (M)

  2. Indicator Lab Report - investigating acid-base reactions

    as well, but, theoretically, less NaOH would have needed to be added due to the lesser concentration of H+ ions compared to the first experiment. In the third graph (strong acid and weak base) no apparent equivalence point can be observed.

  1. Energetics Design Lab

    In comparison, ethanoic acid is not fully ionized. Evaluation: Overall, this experiment went very well; however, there were numerous limitations which affected the results. One very clear and important limitation is the heat loss. Heat loss was a huge factor which affected the results.

  2. Design Lab, HCl + Marble chips

    > Mixing the reactants. The reactants will not be mixed once the marble powder is added to the HCl. This is because it is difficult to measure the number and degree of mixing a solution. And if this process is performed, it would open room to errors and flaws in the experiment.

  1. IA - Lab Report. Aim to prepare a sample of p-nitro acetanilide from the ...

    acid * Concentrated acid * Concentrated sulfuric acid * Fuming metric acid * Methylated spirit * Ice cubes * Chilled water PROCEDURE * Preparation of the salt solutions o Weigh 5 g of acetanilide powder in a watch glass with the help of an electronic weighing machine and add this to a 100 cm3 conical flask.

  2. Titration of Na2CO3.xH2O with HCl

    Thus, a change of colour would indicate the end-point of the reaction. Variables: * Independent variable: There was no independent variable present. * Dependent variable: The dependent variable of this experiment was the volume of dilute acid (HCl) used to neutralize the sodium carbonate solution (Na2CO3).

  1. Chemistry lab reort-molar volume of hydrogen

    Although the first result is less accurate, it has a higher precision than the second, more accurate one. The random uncertainty of the first is only , while the second has a relatively high random uncertainty of . The great difference between random uncertainties owes to difference in percentage errors of the mole of hydrogen gas produced.

  2. The chemistry of atmospheric and water pollution.

    and then into the river, there would be increased levels of calcium, magnesium, sulfate and chloride ions. If the river was situated near a limestone deposit or cave, the water would leach the limestone and thus there would be a high concentration of calcium and carbonate ions.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work