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The pOH of a solution is 9.40 at 25C. Calculate the hydronium ion concentration of the solution.

Short Answer

Expert verified
The hydronium ion concentration is approximately 2.51×105 M.

Step by step solution

01

Understand the relationship between pOH and pH

The relationship between pH and pOH is given by the equation: pH+pOH=14. At 25C, this equation allows us to find the pH if we know the pOH.
02

Calculate the pH of the solution

Given pOH=9.40, use the relationship: pH=14pOH=149.40=4.60. Now we know the pH of the solution is 4.60.
03

Understand the relationship between pH and hydronium ion concentration

The pH of a solution is related to the hydronium ion concentration [H3O+] by the formula: pH=log10([H3O+]). We can use this to find the hydronium ion concentration after calculating the pH.
04

Calculate hydronium ion concentration

Rearrange the formula to solve for [H3O+]: [H3O+]=10pH. Using pH=4.60, we find [H3O+]=104.602.51×105 M.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

pOH
The pOH of a solution provides insight into its basicity. It measures the concentration of hydroxide ions (OH⁻) in a solution. The formula to calculate pOH is pOH=log10([OH]). This logarithmic scale is similar to pH and is used to understand the acidic or basic nature of a solution.
When dealing with pOH, you should know:
  • The lower the pOH, the more basic the solution is.
  • To switch between pH and pOH, you can use the formula: pH+pOH=14.
  • This relationship is valid in water at 25C.

For the solution with a pOH of 9.40, you can use these basics to find out more about its acidic counterparts, specifically the pH and the hydronium ion concentration.
pH
The pH of a solution is a measure of the concentration of hydrogen ions (H⁺) or hydronium ions (H3O+). It indicates how acidic or basic a solution is, using a scale from 0 to 14. The formula used is pH=log10([H3O+]).
Here are some key points about pH:
  • If the pH is less than 7, the solution is acidic.
  • If the pH is greater than 7, the solution is basic.
  • A pH of 7 is considered neutral, as is the case with pure water.

In our example, once we calculated the pH from a pOH of 9.40 (which turned out to be 4.60), we could then determine that the solution is acidic. From the pH, calculations can be done to determine the hydronium ion concentration.
Relationship between pH and pOH
The relationship between pH and pOH is a fundamental aspect of acid-base chemistry. The equation pH+pOH=14 expresses this balance in any aqueous solution at 25C.
Understanding this relationship helps in:
  • Interconverting between pH and pOH.
  • Assessing the acidity or basicity of a solution quickly by knowing either value.

This relationship ensures that if you know one value, you can effortlessly deduce the other. For instance, with a pOH of 9.40, the pH calculates as 4.60. This knowledge is key in tackling a variety of chemical problems, particularly when determining the characteristics of an unknown solution.
Acid-base equilibria
Acid-base equilibria involve reactions that establish the balance between acids and bases in a solution. The essence of these equilibria lies in understanding the exchange of protons (H+) between acids and bases. pH and pOH values are central to analyzing such equilibria, detailing how acidic or basic a given solution is.
Consider the following aspects when exploring acid-base equilibria:
  • Equilibrium constant expressions denote the extent of ionization of acids or bases.
  • A strong acid fully ionizes in water, while a weak acid only partially does so.
  • These equilibria help predict how changing concentrations or conditions affects the solution.

Being well-versed in acid-base equilibria allows one to predict the effects of adding acids or bases to solutions, further informing the pH or pOH changes. These reactions are at the heart of many natural and industrial processes, making comprehension vital for students and professionals alike.

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Most popular questions from this chapter

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