Potassium carbonate reacts with dilute nitric acid as shown below:
K2CO3(aq)+2HNO3(aq)→2KNO3(aq)+CO2(g)+H2O(l) \text{K}_2\text{CO}_3(\text{aq}) + 2\text{HNO}_3(\text{aq}) \to 2\text{KNO}_3(\text{aq}) + \text{CO}_2(\text{g}) + \text{H}_2\text{O}(\text{l}) K2CO3(aq)+2HNO3(aq)→2KNO3(aq)+CO2(g)+H2O(l)Give the simplest ionic equation for this reaction.
The gas CO2\text{CO}_2CO2 released from the combustion of fossil fuels can dissolve in seawater, causing ocean acidification.
State the chemical property of CO2\text{CO}_2CO2 that causes acidification when it dissolves in water.
Give an equation to show the reaction of CO2\text{CO}_2CO2 with water.
Draw a diagram to show the shape of a molecule of H2O\text{H}_2\text{O}H2O. Include any lone pairs of electrons in your diagram.
State the H−O−H\text{H}-\text{O}-\text{H}H−O−H bond angle.
Explain this shape and bond angle in terms of electron pair repulsion.
The initial rate of the reaction between hydrogen peroxide and iodide ions (the iodine clock reaction) can be monitored by measuring the time taken for a fixed amount of iodine to be produced in the presence of a starch indicator and a small, known amount of sodium thiosulfate.
Describe an experiment to investigate the effect of the concentration of iodide ions on the initial rate of this reaction.
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