The ionic equation for the reaction between sodium thiosulfate and hydrochloric acid is: $$\[ \mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}(\mathrm{aq})+2 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow \mathrm{S}(\mathrm{s})+\mathrm{SO}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \]$$ The solid sulfur formed causes the reaction mixture to become cloudy and opaque. You will carry out experiments to investigate the relationship between the concentration of sodium thiosulfate and the rate of reaction. Small amounts of $$\(\mathrm{SO}_{2}\)$$ gas are released during this reaction. Take care to avoid inhaling this gas. It is important that, as soon as each experiment is complete, the contents of the beaker are emptied into the quenching bath and the beaker is rinsed thoroughly. FA 1 is 0.10 moldm $$\({ }^{-3}\)$$ sodium thiosulfate, $$\(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\)$$. FA 2 is $$\(2.00 \mathrm{moldm}^{-3}\)$$ hydrochloric acid, HCl . distilled water The final instruction for each experiment is to rinse and dry the beaker. State the effect on the reaction time of not drying the beaker before carrying out each of Experiments 2-5. Explain your answer. ............................................................................................................................................... . ............................................................................................................................................... . .........................................................................................................................................

Answer:

Knowledge points:

Solution: