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

Acid-base indicators - explore some of the properties of selected acid-base indicators and measure the pH of some common solutions.

Extracts from this document...

Introduction

Acid-base indicators - explore some of the properties of selected acid-base indicators and measure the pH of some common solutions. Acid-base indicators Aim: In this practical you will explore some of the properties of selected acid-base indicators and measure the pH of some common solutions. Theory: The pH of a solution is a measure of the hydrogen ion concentration. A pH below 7 indicates an acidic solution, a pH greater than 7 indicates an alkaline solution, while a pH of 7 indicates a neutral solution. A range of indicators is used in chemistry because a particular indicator tells us a great deal about its chemical properties. Method: (part A) 1. Your teacher will provide a range of acid-base indicators in the laboratory. Indicators can be in paper of liquid form. ...read more.

Middle

Red pH 3 Yellow pH 6 Blue pH 9 Litmus Red/pink. Red No change No Bromothymol blue Yellow Yellow/orange No change No Questions: Which of the above indicators could you choose to test the pH of a solution of (a) pH = 3, (b) pH= 6, (c) pH =9? You could use the universal indicator as in the tests taken out these three results were shown so this indicator pointed out that these results can be found as was in vinegar, pure water and NaOH. How might you measure the exact pH at which a particular indicator changes colour? You could measure this with a colour indicator that shows particular colours and what their pH is when this colour change takes place. ...read more.

Conclusion

Explain. Some substances used around the household such as cleaning products (ammonia, limewater etc.) are very high in acidity, which means that certain cleaning products must be high in acid to clean. Beverages are a lot lower in and means that are more base type solutions, which are more suitable for consuming. Why is universal indicator more useful for this second exercise? As we know the colours in which that they change to with the universal indicator as to their pH level Conclusion: In conclusion from this practical we can see that from using different substances to test certain products for the pH level. We have found how certain things we use everyday have different levels of pH and that we can see why they are used for this purpose and why they are made for this purpose. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous 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 GCSE Aqueous Chemistry essays

  1. Concentration of Vinegar

    coloured, and so occasionally more NaOH may have been added then was necessary. Also as I read the levels of the NaOH from the meniscus lines on the burette with my eyes these readings could be affected by human error and therefore may well be inaccurate.

  2. Acidic Solutions.

    Na2CO3(s) + H2SO4(aq) Na2SO4 (s) + H2O(l) + CO2(g) Sodium carbonate will react with sulphuric acid to form sodium sulphate salt, water and carbon dioxide. But firstly, I have to make a choice of indicator to use in helping me to know the stiochiometric point or equivalent point of the reaction, which will signify the end of the reaction.

  1. Investigating the effects of varying pH levels on the germination of cress seeds

    values, as I had already suspected that such acidic conditions would not have resulted in any germination. As expected, the samples with only distilled water showed great success in germination, and those with only 20% concentration showed very little, but some signs of germination.

  2. Calibrating pH meters

    with in your body just by inhaling the vapour through the air. One way of preventing this is by closing lids on all chemicals after use by closing the lid you are also preventing spillages so if the container is dropped the chemical remains inside the container.

  1. copper practical

    The copper sulphide reacts to produce a copper metal. The word equation to describe this is as follows: CuS2+O2 2Cu+SO2 6) The end product from all of these stages is called blister copper. It is about 98% pure. The method used for this is the same as I have done in the practical.

  2. See how the pH and the temperature levels change during an acid/base titration using ...

    The graph of the pH value against amount of acid added shows a negative correlation. For the 2 Molar solution, as the amount of acid added to the alkali increases the temperature of the solution begins to increase at a fairly steady rate until 22cm3 of acid is added to

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