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Ch.16 - Acids and Bases
All textbooksTro 4th EditionCh.16 - Acids and BasesProblem 134
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Chapter 16, Problem 134

White wines tend to be more acidic than red wines. Find the [H3O+] concentration in a Sauvignon Blanc with a pH of 3.23 and a Cabernet Sauvignon with a pH of 3.64. How many times more acidic is the Sauvignon Blanc than the Cabernet Sauvignon?

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1
Understand that pH is a measure of the acidity of a solution, defined as the negative logarithm (base 10) of the hydronium ion concentration: \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).
To find the \([\text{H}_3\text{O}^+]\) concentration for the Sauvignon Blanc, use the formula \([\text{H}_3\text{O}^+] = 10^{-\text{pH}}\) and substitute the given pH value of 3.23.
Similarly, calculate the \([\text{H}_3\text{O}^+]\) concentration for the Cabernet Sauvignon using its pH value of 3.64.
To determine how many times more acidic the Sauvignon Blanc is compared to the Cabernet Sauvignon, divide the \([\text{H}_3\text{O}^+]\) concentration of the Sauvignon Blanc by that of the Cabernet Sauvignon.
Interpret the result: a higher \([\text{H}_3\text{O}^+]\) concentration indicates a more acidic solution, so the quotient from the previous step tells you how many times more acidic the Sauvignon Blanc is.
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