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

The aim of the courework is to find the unknow concentration of HCl

Extracts from this document...


Aim: The aim of the courework is to find the unknow concentration of HCl Introduction Chemical procedure is used for determining the concentration of a solution. A known volume of a solution of unknown concentration is reacted with a known volume of a solution of known concentration (standard). The standard solution is delivered from a pipette so the volume added is known. This technique is known as titration. Often an indicator is used to show when the correct proportions have reacted. This procedure is used for acid-base, redox, and certain other reactions involving solutions. Making the standrad solution A stadard solution is a solution which the concentration is accurately known.the concertration is usely in mol dm . when making the standard solution it's in important that the correct mass is substanced acuratley and all of the solution successfully transferred to the volummetic flask. Uses of volumetic solution Volumetric solution can be used in many purposes, but it can also be used to find the following: * Concentration * Molecules mass of a substance * Percentage of an element present * Stoichiometry of an equation * Quality control Procedure Apparatus * Watch glass * Goggle * Balance * Volumtric flask * De-ioned water * Beaker * Glass rod * Teat pippette * Anhydrous sodium carbonate * Label * Spatual * Filter funnel * Bench mat Method 1. ...read more.


* Obtain a beaker ( which has been rinsed twice with de-ionised water) and a white tile. * Place the white tile under burette and then place the beaker on top of the white tile. * Next the burette casn be filled as close to 0.00 as possible. (make sure the tap is closed) * Fill the pippette with de-ionised water to clean any impurities away. * Using the pipette filler fill the pipette with your standard solutuion (sodium caronate) and pour it in the beaker. * Pour a couple of drops of methyl (orange) * open the for a few seconds at a time until the sandard solution changes from orange to pink. * lastly read the measurments of the hydrochloric acid in the burette and record the amount left. Burette: The precision of a burette makes careful measurement with a burette very important to avoid systematic error. When reading a burette, the viewer's eyes must be at the level of the graduation to avoid parallax error. Even the thickness of the lines printed on the burette matters; the bottom of the meniscus of the liquid should be touching the top of the line you wish to measure from. ...read more.


= 35.20g After getting the mass you take it away 36.60 - 35.20 = 1.40 Step 2: Find the RAM of Na CO Na = 23 mulitply by 2 C = 12 O = 16 mulitply by 3 = 48 So you add 23 + 23 + 12 + 16 + 16 + 16 = 106 Step 3: to find the number of moles in Na CO you divide 1.40 by 106 which you get 0.0132 moles Step 4: Next we find the concentration of Na CO soution you divide 0.01323 by 0. 025 which you get 0.0528 mol/dm Step 5: I need to balance the equation Na CO + 2HCl 2NaCl + CO +H O Step 6: After finding the concentration of Na CO we need to find the number of moles. So you do No of moles = concentration volume = 0.0528 0.025 = 0.00132 Step 7: In addition, we had to find the number of moles of HCl. To find this NO of moles of HCl = 0.00132 2 = 0.00262 Step 8:lastly you get the volume of HCl from the titration which is25.22, to give you final results HCl concentration = moles divided by volume dm 0.00264 = 1.046 = 1.050 mol/ dm 0.002522 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic 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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    I could make up my solution by weighing the sodium carbonate in the volumetric flask as this would mean I wouldn't have to move the solid, but it would be hard to get the exact amount as I couldn't really get to the solid once it was in, to adjust

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    Making the solution: Equipment needed: * Electronic balance: an electronic balance measures to 2 decimal places; this will give us an accurate weight of the solid used. * Weighing boat A weighing boat is a container used to prevent reagents from contacting the balance pan.

  1. effects Concentration and Temperature on the Rate of Reaction

    O = 1 x 16.0 = 16.0 = 94.0 grams needed = (0.0001 x 94 x 250) 1000 = 0.00235g dissolved in enough distilled water to make 250ml of solution. 0.01M potassium bromide: KBr: K = 1 x 39.1 = 39.1 Br = 1 x 79.9 = 79.9 = 119.0 grams needed = (0.01 x 119 x 250)

  2. determination of the percentage of oxalate in iron (II) oxalate by redox titration

    Permanganate ion is deep purple in colour, while other soluble manganese ion is different colour, like pale red or green. This titration gives an sharp end-point because the solution in the conical flask change from colourless to permanent pink at the end point due to the present of magnate (II)

  1. Chem Lab report. Objective: To determine the concentration of potassium manganate(VII) solution using ...

    ions. Then a larger volume of potassium manganate(VII) solution was needed and thus lead to an error. Also, nitric acid was also not appropriate in this experiment because it may act as an oxidizing agent to oxidize the ethanedioic acid. Then a smaller volume of potassium manganate(VII) solution was needed and thus lead to an error.

  2. Finding Out how much Acid there is in a Solution

    Procedures that reduced errors During the course of my investigation, I took several precautions that should have reduced errors, which should have contributed to my final result being accurate. These procedures included: * I repeated the titration until I had completed three titrations that had results within 0.1cm3 of each other.

  1. experiment to find the concentration of the ethanedioic acid

    Use an insulator to hold the conical flask when heated. * Carry out the titration as normal, ensuring that temperature is above 60 degrees using a thermometer. If needed stop titration and heat until over 60 degrees again and then continue.

  2. Chemistry - Data Analysis

    41 45 45 45 45 45 46 28 41 45 45 30 40 39 40 44 43 44 44 44 45 30 40 44 44 These results were then plotted on graphs and these were then analysed for the purpose of deriving a meaningful relationship between the materials and their ability to lose heat.

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