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Chapter 15: Problem 152

Solution A has a \(\mathrm{pH}\) of 3 . Solution \(\mathrm{B}\) has a \(\mathrm{pH}\) of 6 . Which solution is more acidic, and by how much?

Short Answer

Expert verified
Solution A is more acidic than Solution B since it has a lower \(\mathrm{pH}\) value (3 compared to 6). The difference in their acidities is a factor of 1000.

Step by step solution

01

The \(\mathrm{pH}\) scale is used to measure the acidity or basicity (alkalinity) of a solution. The scale ranges from 0 to 14, with 7 representing a neutral solution (pure water). A solution with a \(\mathrm{pH}\) value below 7 is considered acidic, and a \(\mathrm{pH}\) value above 7 indicates a basic solution. The more acidic a solution, the lower its \(\mathrm{pH}\) will be. #Step 2: Comparing the \(\mathrm{pH}\) values of Solutions A and B#

We are given that Solution A has a \(\mathrm{pH}\) of 3 and Solution B has a \(\mathrm{pH}\) of 6. As mentioned earlier, a lower \(\mathrm{pH}\) represents a more acidic solution. In this case, Solution A has a lower \(\mathrm{pH}\) than Solution B, so it is more acidic. #Step 3: Calculating the difference in acidity as a ratio#
02

To determine the difference in acidity, we must consider the fact that the \(\mathrm{pH}\) scale is logarithmic, meaning that a change of one \(\mathrm{pH}\) unit represents a tenfold change in acidity. The difference in \(\mathrm{pH}\) values between Solution A and Solution B is: \[\text{Difference in }\mathrm{pH} = \mathrm{pH}_B - \mathrm{pH}_A = 6 - 3 = 3\] Now, we can find the ratio of the \(\mathrm{H}^+\) ion concentration between the two solutions using the following formula: \[\text{Ratio of }\mathrm{H}^+ = 10^{\mathrm{pH}_A - \mathrm{pH}_B} = 10^{3 - 6} = 10^{-3}\] To express the difference in acidity as a ratio, we will take the reciprocal of the calculated ratio: \[\text{Acidity ratio} = \frac{1}{10^{-3}} = 10^3 = 1000\] #Conclusion#

Solution A is more acidic than Solution B, and the difference in their acidities is a factor of 1000.

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Most popular questions from this chapter

Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate: (a) \(\mathrm{HNO}_{3}\) and \(\mathrm{OH}^{-}\) (b) \(\mathrm{HF}\) and \(\mathrm{OH}^{-}\) (c) \(\mathrm{NH}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{H}_{2} \mathrm{O}\)

What is the \(\mathrm{pH}\) of a solution whose \(\mathrm{OH}^{-}\) concentration is \(10^{-14} \mathrm{M} ?\) Is the solution acidic or basic?

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Can a buffer resist \(\mathrm{pH}\) changes for any added amount of strong acid or base? Explain.

The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?
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