You make a solution by dissolving 0.0010 mol of hcl in enough water to make 1.0L of solutio. If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain.
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You make a solution by dissolving 0.0010 mol of hcl in enough water to make 1.0L of solutio.
If you were to measure the pH of 10 drops of the original HCl solution, would you expect it to be different from the pH of the entire sample? Explain.
Given : moles of HCl = 0.0010 mol
And volume of solution = 1.0 L
Since HCl is a strong acid. Hence it will dissociate completely into hydronium ions as per the reaction,
HCl (aq) + H2O (l) -------> H3O+ (aq) + Cl- (aq)
From the above reaction we can say that moles of H3O+ ions produced = moles of HCl taken = 0.0010 mol
Since moles = concentration X volume of solution in L
=> 0.0010 = concentration of H3O+ ions X 1.0
=> concentration of H3O+ ions = [H3O+ ] = 0.0010 M
Since pH = -log[H3O+ ]
=> pH of the entire solution = -log(0.0010) = 3.0
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