You are investigating how the rate of reaction depends upon the concentration of hydrochloric acid when it is reacted with sodium thiosulfate in a small glass beaker. Which reagent in this experiment poses the greatest hazard?sodium thiosulfatehydrochloric acid

A student performed an experiment in which they reacted 50cm3 of 0.300mol dm-3 sodium thiosulfate with 5.0cm3 of 2.000 dm-3 hydrochloric acid. They are investigating the affect of changing conditions on the rate of reaction. Which of the following concentrations of hydrochloric acid would result in the slowest rate of reaction?

The reaction between magnesium and hydrochloric acid is exothermic, so it releases heat. This could be a problem for Gemma's investigation because temperature also affects reaction rate. The rise in temperature could, therefore, influence the outcome in addition to the independent variable, concentration.Describe one way that Gemma could deal with this problem to improve the validity of her experiment.

Q3. Now consider the moment when the blue colour change is about to occur (i.e. when there is no more thiosulfate remaining in solution). Based on the initial experiment and initial concentrations of reagents, calculate the concentrations of the reagents present in the flask at the moment just before the blue colour change begins (ignore the starch, and the S4O62- which is formed as the other by-product in this reaction). Does Reaction (1) continue beyond this point? a. yes b. no Based on what you have calculated, which reagent in Reaction (1) is the limiting reagent? a. H+ b. H2O2 c. I- d. S2O32-

In Experiment II, 20 cm3 of 0.1 mol/dm3 hydrochloric acid is reacted with excess calcium carbonate. Suggest the concentration of hydrochloric used if the same volume was used for Experiment III.

Dilute hydrochloric acid will dissociate into ________ .