The current average pH of our oceans is 8.1. What is the concentration of protons in the oceans? How has the proton concentration changed in our oceans when compared to before the industrial revolution, when the average pH was 8.2? Express this change as a percentage increase.

Verified step by step guidance

Calculate the concentration of protons (H+) in the ocean for the current average pH of 8.1 using the formula: \( [H^+] = 10^{-pH} \).

Calculate the concentration of protons (H+) in the ocean for the pH before the industrial revolution, which was 8.2, using the same formula: \( [H^+] = 10^{-pH} \).

Compare the two proton concentrations to find the absolute change in proton concentration. This can be done by subtracting the proton concentration at pH 8.2 from the proton concentration at pH 8.1.

To find the percentage increase in proton concentration, use the formula: \( \text{Percentage Increase} = \left( \frac{\text{New Concentration} - \text{Old Concentration}}{\text{Old Concentration}} \right) \times 100\% \).

Interpret the results to understand how the proton concentration in the oceans has changed due to changes in pH levels, reflecting on the impact of acidification.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

pH Scale

The pH scale measures the acidity or alkalinity of a solution, ranging from 0 to 14. A pH of 7 is neutral, while values below 7 indicate acidity and above 7 indicate alkalinity. Each whole number change on the pH scale represents a tenfold change in hydrogen ion concentration, meaning that a decrease in pH corresponds to an increase in proton concentration.

Proton Concentration

Proton concentration in a solution is directly related to its pH value. The formula to calculate proton concentration ([H+]) from pH is [H+] = 10^(-pH). Therefore, a lower pH indicates a higher concentration of protons, which is crucial for understanding changes in ocean chemistry over time, particularly in relation to ocean acidification.

Ocean Acidification

Ocean acidification refers to the decrease in pH levels of ocean waters due to increased carbon dioxide (CO2) emissions. Since the industrial revolution, the absorption of CO2 by oceans has led to a measurable drop in pH, resulting in higher proton concentrations. This change can have significant impacts on marine life, particularly organisms that rely on calcium carbonate for their shells and skeletons.

Recommended video:

Guided course

03:57

Seasonal Turnover & Ocean Upwelling

Related Practice

Textbook Question

When H₂ and CO₂ react, acetic acid can be formed spontaneously while the production of formaldehyde requires an input of energy. Which of these conclusions can be drawn from this observation?

a. More heat is released when formaldehyde is produced compared to the production of acetic acid.

b. Compared to the reactants that it is formed from, formaldehyde has more potential energy than does acetic acid.

c. Entropy decreases when acetic acid is produced and increases when formaldehyde is produced.

d. Only acetic acid could be produced under conditions that existed in early Earth.

1471

views

Textbook Question

From what you have learned about water, why do coastal regions tend to have milder climates with cooler summers and warmer winters than do inland areas at the same latitude?

1807

views

Textbook Question

Consider the reaction between carbon dioxide and water to form carbonic acid (CH2O3):

CO2(𝑔)+H2O(𝑙)⇌CH2O3(𝑎𝑞)

In the ocean, carbonic acid immediately dissociates to form a proton and bicarbonate ion, as follows:

CH2O3(𝑎𝑞)⇌CHO3−(𝑎𝑞)+H+(𝑎𝑞)

As atmospheric CO2 increases, the ocean absorbs more of the gas. Would this sequence of reactions be driven to the left or the right? How would this affect the pH of the ocean?

375

views