The hydrogen ion concentration, [H+] in a solution with pH 10 is ________ than the [H+] in a solution with pH 13.

Question

BlackTom AI · Accepted Answer

The question asks how the hydrogen ion concentration [H+] at pH 10 compares with that at pH 13. 
First, recall that pH is the negative logarithm of [H+]: pH = -log10[H+]. A difference of 1 pH unit corresponds to a tenfold change in [H+].
Here, the pH drops from 13 to 10, which is a decrease of 3 pH units. Since each unit represents a tenfold increase in [H+], a 3-unit decrease in pH means [H+] at pH 10 is 10^3 times greater than [H+] at pH 13. 
Now evaluate the options:
- '100 times less' would imply [H+] at pH 10 is 100 times smaller, which contradicts the 3-unit difference that yields a 1000-fold increase, so this is incorrect.
- '1,000 times greater' aligns with the 10^3 factor resulting from three pH unit differences, so this is correct.
- '3 times greater' ignores the logarithmic (powers of ten) relationship between pH and [H+], making it inaccurate.
- '1,000 times less' suggests a decrease rather than the actual increase in [H+], which is false for the pH change described.
In summary, understanding the logarithmic scale of pH is key: every one-unit change multiplies [H+] by 10, so a three-unit difference yields a 1000-fold change in concentration, specifically increasing as pH decreases from 13 to 10.

The hydrogen ion concentration, [H+] in a solution with pH 10 is ________ than the [H+] in a solution with pH 13.

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