Purchase Solution

pH of rainwater and diprotonic acids.

Not what you're looking for?

Ask Custom Question

The pH of a sample of rain is found to be 3.3. Calculate the percentage of HSO4- that is ionized in this sample, given that the acid dissociation constant for the second stage of ionization of H2SO4 is 1.2E-2.

Purchase this Solution
Solution Summary

The solution (2 pages in length) shows how to seal with dissociation of acids that can contribute two protons, such as sulphuric acid. The solution shows how not to fall into the common trap of assuming full dissociation right in the first reaction.

Solution Preview

The solution is attached below in two files. the files are identical in content, only differ in format. The first is in MS Word XP Format, while the other is in Adobe pdf format. Therefore you can choose the format that is most suitable to you.

Here are the steps to solve the problem:

1. Find the final [H] ions using the pH. denote this concentration x.
2. Assume ...

Purchase this Solution
Free BrainMass Quizzes
Periodic table

Functional groups in Organic Chemistry

You will be tested on the names of functional groups in Organic Chemistry. It is very important to know the functional groups to understand Organic reactions.

Organic Chemistry Naming: Alkanes

This is a quiz which is designed to assist students with learning the nomenclature used to identify organic compounds. This quiz focuses on the organic compounds called Alkanes.

General Chemistry - Classification of Matter

This test will assess your knowledge on the classification of matter which includes elements, compounds and mixtures.

Thermochemistry

The quiz helps in revising basic concepts about thermochemistry.

View More Free Quizzes
Related BrainMass Solutions

  • calcium carbonate dissovled in rainwater

    253234 Calculate the amount of calcium carbonate (mg) dissolved per liter of rainwater. The average pH of precipitation in rural areas is 6.10.

  • concentration of calcium carbonate in rainwater

    162501 The average pH of precipitation in rural areas is 5.70. calculate the amount of calcium carbonate (mg) dissolved per liter of rainwater. Could you please explain what formula and step are invovled and please provide (example) if possible?

  • concentration of calcium carbonate in rainwater

    The solution includes detailed explanation of the calculation of concentration of calcium carbonate (CaCO3) dissolved in rainwater with known pH of the precipitation.

  • Calcium Carbonate Dissolved per Litre

    Assuming that the pH is controlled by the carbonate system, i.e., no anthropogenic acid gases are present in the atmosphere, calculate the amount of calcium carbonate (mg) dissolved per liter of rainwater. pKa1=6.33, KCO2=3.388e-02 Hint: pCO2=3.162e

  • Concentration of Atmospheric CO2

    This solution of 98 words shows step-by-step calculations to determine the pH of the rainwater considering the CO2 acidic input.

  • Titrations - rain water with NaOH

    A 155 mL sample of rainwater is titrated using 0.0095 M NaOH solution. If 4.8 mL of the NaOH solution was required to reach the endpoint, what was the pH of the rainwater?

  • Rate of S(IV) to S(VI) at Different pHs using O3 and H2O2

    If the pH of the rainwater is 4.3, calculate the rate of SO2 oxidation by H2O2 in the plume if the H2O2 concentration is 1 ppb. Which oxidation (O3 or H2O2) sequence dominates at a pH of 4.3?

  • Calculating moles using volume, density, molar mass, pressure and temperature

    Naturally, rainwater should have a pH of not less than 5.5, but in the northeastern United States for example, the average pH of the rainwater is about 4.5.

  • Leachate from landfills

    Putting the mine waste in an area that is not permeable to rainwater, or has soil that can counteract the acids, therefore keeping th leachate out of the groundwater, but not out of the lakes and streams. Probably a few more....

View More Related Solutions