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19 Nov 2019
A student reads that mixing a strong acid and a strong base is a neutralization reaction and should produce a solution with a neutral pH. So the student mixes equal volumes of equally concen- trated sulfuric acid and sodium hydroxide. Rather than a neutral pH, however, the pH of the result- ing solution is acidic. Why is this? (Assume the neutralization reaction goes to completion.) A. Sulfuric acid is sufficiently strong as an acid so as not to react at all but still neutralize the sodium hydroxide. B. There are more moles of sulfuric acid tharn sodium hydroxide, so there is sulfuric acid left over at the end of the reaction. C. There are more hydrogen ions from the sulfuric acid than there are hydroxide ions from the sodium hydroxide, so there are hydrogen ions left over at the end of the reaction. D. There are fewer hydrogen ions from the sulfuric acid than there are hydroxide ions from the sodium hydroxide, so there are hydroxide ions left over at the end of the reaction.
A student reads that mixing a strong acid and a strong base is a neutralization reaction and should produce a solution with a neutral pH. So the student mixes equal volumes of equally concen- trated sulfuric acid and sodium hydroxide. Rather than a neutral pH, however, the pH of the result- ing solution is acidic. Why is this? (Assume the neutralization reaction goes to completion.) A. Sulfuric acid is sufficiently strong as an acid so as not to react at all but still neutralize the sodium hydroxide. B. There are more moles of sulfuric acid tharn sodium hydroxide, so there is sulfuric acid left over at the end of the reaction. C. There are more hydrogen ions from the sulfuric acid than there are hydroxide ions from the sodium hydroxide, so there are hydrogen ions left over at the end of the reaction. D. There are fewer hydrogen ions from the sulfuric acid than there are hydroxide ions from the sodium hydroxide, so there are hydroxide ions left over at the end of the reaction.
Casey DurganLv2
10 Apr 2019