• 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)

    To do that, we will weigh a weighting boat (which is approximately 0.90g). Then we add the solid up to exactly 3.55, so our final mass of Na2CO3 will be exactly 2.65g of Na2CO3. This way of weighting will give us the exact amount of Na2CO3 needed.

  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. Thermal Decomposition of Calcium Carbonate

    This means there is a lesser chance of energy being lost. All these 3 errors are significant to the experiment, as they all can contribute to an increase/ decrease of the temperature of the mixture.

  1. The preparation, analysis, and reactions of an ethanedioate complex of iron

    While in the presence of dilute sulphuric acid, more Fe3+ ions can be released to form red complex with CNS- ions. Thus, the resulting solution is dark red. As the complex prepared had similar reactivity as FeCl3, we can assume that the oxidation state of iron in the complex is also +3.

  2. The Effects of Strong and Weak Acids on the Order of a Reaction.

    Number of moles = Mass RMM 0.004 = Mass 24 Therefore, the mass of magnesium that I needed was 0.096g After working out the moles of the Hydrogen gas, I can also work out the volume of the acid required by looking at the mole ratio (2:1)

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

    the concentration, I must first know the number of moles of sulphuric acid used in each titration. First, I must know how many moles of sodium carbonate were used per titration I can use the chemical equation for the titration to work out the mole ratio between sulphuric acid and sodium carbonate: H2SO4 (aq)

  2. 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.

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