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Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid variables
Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid variables
Why safety is important in the laboratory
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The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction between Sodium Thiosulphate and Hydrochloric Acid
I am going to be investigating the effect of varying the concentration
of Hydrochloric acid on the rate of reaction between Sodium
thiosulphate and Hydrochloric acid.
Chemical reactions can be affected by:
Ÿ Changes in the surface area of solid reactants
Ÿ Changes in concentration
Ÿ Changes in pressure (with gases)
Ÿ Changes in temperature
Ÿ Catalysts
Ÿ Light
But I am changing the concentration, as it is the most practical
experiment to carry out in a school laboratory. I could have changed
the temperature but I have done that experiment before in class.
When carrying out my experiment I need to make sure I follow the
following safety precautions:
Ÿ To keep my lab coat fastened as the laboratory is very crowded.
Ÿ Keep the experiment area clear and tidy to avoid spillages as
hydrochloric acid is corrosive and can damage the bench.
Ÿ Wear safety goggles so that the corrosive acid doesn't get into my
eyes.
Ÿ Tie back my hair so it doesn't get it in the way.
Ÿ I must report any accidents to the teacher immediately, as HCl and
Sodium thiosulphate can be dangerous substances, broken glass can
cause injuries.
Ÿ Wash my hands after practicals involving chemicals, HCl is corrosive
and dangerous if left on skin for too long.There aren't enough fume
cupboards for everyone in the class to use.
I will be using GCSE Chemistry textbooks and class notes for
information for research, which will be secondary quotes.
From experiments I have done in class using Sodium thiosulphate and
Hydrochloric acid. I added 5cm of Hydrochloric acid to 10cm of Sodium
thiosulphate with 40 cm of water. I expect the solution to turn from a
clear solution to a creamy yellow cloudy liquid, which has an
unpleasant smell.
I know that the term concentration is the amount of a particular
substance within a solution or mixture.
Investigating How the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Calcium Carbonate
Rate of reaction is the speed of reaction. In essays written by young scientists, they have used concentration as variable in their experiments; some have used a light sensor. connected to a data logger, to measure the amount of light passing. through the "cloudy" liquid. 1 moles = 6.02 1023 The particles in the hydrochloric acid and sodium thiosulphate need to
The Effect of Temperature on the Rate of Reaction Between Sodium Thiosulphate and Hydrochloric Acid
The Arrhenius equation ln k = ln A – (Ea / RT) can be shown
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
The Effect of Sodium Thiosulphate Solution on the Rate of its Reaction with Hydrochloric Acid
Effect of Temperature on the Rate of Reaction between Sodium Thiosulphate and Hydrochloric Acid Investigation Chemical reactions are used in our everyday life, they literally keep us alive. They are used in food, respiration and everywhere else in the environment. A chemical reaction mainly occurs when reactants react together to produce a new product. The speed at which this reaction takes place is called the rate of reaction. The product produced has a number of particles in the solution that has formed from the reactants.
The Rate of Reaction Between Calcium Carbonate and Hydrochloric Acid Planning. CaCO3 (s) + 2HCl (aq) ---- CaCl2 (aq) + H2O (l) + CO2 The rate of reaction depends on how hard and how often the reacting particles collide with each other. A rate of reaction is how fast a reaction takes place.
a bigger one so I can fit the cross under it and also be able to pour
from 10cm to 50cm to make it easier to see the difference in a graph.
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
Conclusion This experiment was set out to find the effect of different temperatures of hydrochloric acid on the rate of reaction with magnesium. The information recorded was then interpreted and compared to the hypothesis. From this information, a conclusion can be made to show that the rate of reaction relates to temperature in the reaction between hydrochloric acid and magnesium. In conclusion, as proven in this experiment, the higher the temperature of hydrochloric acid, the faster the reaction it has with magnesium.
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
My aim in this piece of work is to see the effect of temperature on the rate of a reaction in a solution of hydrochloric acid containing sodium thiosulphate.
Rate of Reaction - Sodium Thiosulphate and Hydrochloric Acid. Aim Investigation, to find out how the rate of reaction between sodium thiosulphate and hydrochloric acid is affected by changing the concentration. Introduction I must produce a piece of coursework investigating the rate of reaction, and the effect different changes have on them. The rate of reaction is the rate of loss of a reactant, or the rate of development of a product during a chemical reaction. It is measured by dividing 1 by the time taken for the reaction to take place.