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- Why is dimethyloxonium cation stronger acid than hydronium?
A powerful but often overlooked factor in determining a substance's acidity and basicity is the effect of the solvent (or lack thereof) in which it is dissolved You are not wrong; in the gas phase, $\ce {H_3O^ {+}}$ is indeed a stronger acid than $\ce { (CH_3)_2OH^ {+}}$, by a factor of about $5\times 10^ {18}$ This can be seen by comparing the proton affinities of the conjugated bases
- How to calculate Ka for hydronium and Kb for hydroxide?
Including water on both side of the equation is a bit of a mistake here For hydronium: $$\ce {K_a = \frac { [H^+] [H_2O]} { [H_3O^+]}}$$ and the source of the proton in question is not likely water (normally a stronger mineral acid) If you put the water on both sides of the equation you are describing another process, which would be proton transfer equilibrium In that case, you are correct
- Difference in properties of water as ligand vs in lattice
Both notations can be combined as for example in copper (II) sulfate: $\ce { [Cu (H_2O)_4]SO_4 · H_2O}$ referring to water which is coordinately bonded to the copper and water which is in the crystal structure left over
- Reaction between sulfur and sodium hydroxide
$\ce {3S + 6NaOH->2Na_2S + Na_2SO_3 + 3H_2O}$ It is a disproportionation reaction: sulfur's oxidation changes from zero to -2 in sodium sulfide and from zero to +4 in sodium sulfite But how to remember the products of this reaction? By rote memorization? The preparation of sodium sulfide is apparent
- Which is better leaving group out of iodide and water?
It is probably the concentrations of the various reagents that is the major force in pushing the equilibrium in one direction or the other For example, when you are hydrolysing something in the lab, you add a whole lot of water and a small amount of reagent Whereas when you are reacting alcohol with HI, you would probably use a lot of HI with a small amount of the reactant (though I have
- Reaction of hydrogen peroxide with sodium carbonate
2) $\ce {Na_2O_2}$ reacts so easily with $\ce {CO_2}$ that it is used for rendering air charged with $\ce {CO_2}$ respirable as in submarines and diving bells 3) $\ce {Na_2O_2}$ absorbs water from the air forming sodium hydroxyde and hydrogen peroxide, the latter quickly decomposed into Oxygen and water
- In acidic solution, what does ClO₃⁻ reduce into?
In acidic solution, what does $\ce {ClO3-}$ reduce into and, most importantly, why? It's $$\ce {6e- +ClO_ {3}^- +6H^+ -> Cl^- + 3 H_2O} $$ Now, with the gift of foresight, why was the equation for
- How does a dry shampoo work? - Chemistry Stack Exchange
1 From my chemistry knowledge, I know that soaps are made from fatty acids and some sort of base and this reaction also gives us $\ce {H_2O}$ so the grease in hair dissolves and gets washed away in water What I don't understand is how dry shampoos can have a cleaning effect on dirt or grease and how they work
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