Share
Calculate The Ph Of 0.002M H2So4 By Assuming Complete Dissociation
Question
Introduction
If you have a solution of 0.002M H2SO4 and want to find out the pH, you need to first determine the number of moles of H3O+ produced by complete dissociation of one mole of H2SO4 (pKa = 12.28). The acid dissociation constant (Ka) for H2SO4 at 25 C is 14×10^(-3)(L/mol)(s), which means that if we can find the number of moles per liter that are produced when one mole undergoes complete dissociation, then we can multiply this figure by 10^(-14) to get the concentration in molarity units:
The acid dissociation constant (Ka) of 0.002M H2SO4 is 14×10^(-3)(L/mol)(s) and its pKa is 12.28 at 25 C.
The acid dissociation constant (Ka) of 0.002M H2SO4 is 14×10^(-3)(L/mol)(s). The pKa of 12.28 at 25 C means that the concentration of H+ ions in this solution is 1/[1 + 14×10^(-3)] = 1/15 = 0.0667 M, so there are 15 times more H+ ions than OH- ions at 25 C.
Calculate the pH by first calculating [H+] and then taking its negative logarithm: [H+] = 1/15 = 0.067 M; pH = -log(0.067)=1
Step 1: Calculate the total molarity of H2SO4 in 0.002M solution
To calculate the number of moles of H2SO4 in 0.002M solution, you must first calculate the total molarity of H2SO4 in a liter of solution. This can be done using the equation M x L = moles:
M = 0.002mol/L = (0.002mol)(1L) = 0.0002mol
Now that we know how many moles there are per liter, we can simply multiply this by how many liters we have to find out how many total moles there are in our sample:
(0.0002 mol)(0.1 L) = 0.00002 mol
Step 2: Calculate number of moles of H2SO4 = M x L
You can calculate the number of moles of H2SO4 by multiplying the concentration (M) of H2SO4, in this case 0.002 molarity, by its volume (L), which is 0.1 liters:
- [0.002 mole/L x L] = 0.00002 mol
Step 3: Moles of H2SO4 = 0.002 mole/L x L = 0.00002 mol
Next, you’ll need to convert the molarity of H2SO4 into moles of acid. Molarity is simply a measurement of how many grams of solute are dissolved in one liter of solution (or volume). In this case, we have 0.002 mole/L x L = 0.00002 mol.
You can also write this equation as:
moles = M x V
Step 4: Number of moles of H3O+ = 0.00002 mol/(14×10^(-3)(L/mol)(s)) = 9.14×10^11 s-1(molecules/liter) wt%H3O+ at 25 C
In step 4, you will calculate the number of moles of H3O+. You can do this by first converting 0.00002 mol/(14×10^(-3)(L/mol)(s)) to moles by multiplying it by Avogadro’s number (6.022×10^23) and then dividing this value by the volume of solution (1 L). The resulting number is 9.14×10^11 s-1(molecules/liter) wt%H3O+ at 25 C.
Step 5: Conversion factor to calculate pH from pKa based on acid dissociation constant (Ka)
The next step is to convert the pKa value into a pH. To do this, you need to know the conversion factor for each unit of measurement. The conversion factor for pKa is -log(1/Ka). So, if we use this equation:
pH = -log(1/14×10^(-3))
And we plug in our numbers from above:
pH = 12.28 – log(1/(0.00014))
To calculate the pH of a solution, you need to know the acid dissociation constant (Ka) of the acid that’s present in it and its pKa value. The general equation for this calculation is as follows: pH = -log(1/Ka)
Answers ( 2 )
Calculate The Ph Of 0.002M H2So4 By Assuming Complete Dissociation
When preparing a solution ofH2SO4 (potassium sulfate) in water, it is important to take into account the solubility of the SO4. If all of the SO4 dissociates completely from the water, the Ph of the solution would be zero. In this blog post, we will explore a method for calculating the Ph of a solution of H2SO4 assuming complete dissociation. By following this procedure, we can ensure that our solutions are correctly labeled and measured.
What is Phosphorus?
Phosphorus is an essential nutrient for humans and other animals. It’s a mineral that helps make bones and teeth, as well as hormones and enzymes. Phosphorus is also important in the production of energy in the body.
How to Calculate Phosphorus in a Solution
To calculate the phosphorus in a solution, assume complete dissociation. The chemical equation for phosphorus is P4O10+4H2O=P2O5. Phosphorus can be found by multiplying the concentration of phosphorus in the solution (in mg/L) by the conversion factor 1g/L.
Dissociation of H2SO4
When an acid is completely dissociated into its hydrogen and sulfur atoms, its pH rises to 13. Lemon juice has a pH of about 2.8-3.2 due to the presence of organic acids.
Phosphorus in the Environment
Phosphorus is an essential element in the environment. It is found in both wet and dry soil, water, air, and even the interstellar medium. Phosphorus can be found in all living things and is necessary for their growth. Phosphorus is also a component of many important minerals including calcium phosphate and apatite.
Phosphorus can be present as a free element or combined with other elements to make compounds such as phosphates. Dissociation of phosphorus molecules into atoms leaves the molecule with a positive charge. The majority of phosphorus in the environment is bound to other elements such as nitrogen, oxygen, and sulfur which makes it difficult to measure accurately.
The Environmental Protection Agency (EPA) has developed methodologies to measure phosphorus levels in water using both direct and indirect methods. One method involves measuring phosphorus levels in biological samples that have been collected from different parts of the country. This method can help identify areas where phosphorus levels are high or low. Indirect methods involve measuring changes in atmospheric concentrations of phosphorus over time. These measurements allow scientists to estimate how much phosphorus is present in the environment.
Phosphorus can cause significant environmental problems when it becomes enriched in water bodies or soils due to human activities such as waste disposal or agricultural runoff. When this happens, it can create toxic environments that are harmful to humans, plants, and animals alike. Phosphorus can also contaminate drinking water supplies when it accumulates at low concentrations but is sensitive to changes in water temperature or pH.
There are many ways that the EPA is working to reduce the levels of phosphorus in the environment. For example, they have developed regulations that require companies to reduce the amount of phosphorus that they discharge into waterways. They also work to encourage people to use less phosphorus-containing products and to recycle materials that contain phosphorus.
Conclusion
In order to calculate the ph of 0.002M H2So4, it is necessary to assume complete dissociation. Although this may seem like a daunting task, by using simple algebraic equations and practical examples, it is possible to solve these problems easily. By taking these steps, you can develop a strong foundation in basic chemistry and mathematics, which will prove invaluable as you progress through your education or career.
The pH of a solution is a measure of how acidic or basic it is, and it can be determined by the concentration of hydrogen ions (H+) present. Calculating the pH of a solution can be difficult, but it is not impossible.
For this particular exercise, we will be calculating the pH of a 0.002M H2SO4 solution. This is an acidic solution, as it contains hydrogen ions, so the pH will be less than 7.
To calculate the pH of a solution, we must first assume complete dissociation of the acid. In the case of H2SO4, this means that it will break down into 2 hydrogen ions (H+) and 1 sulfate ion (SO4-). Therefore, the total concentration of hydrogen ions in the solution will be twice the initial concentration of the acid.
Therefore, the total concentration of hydrogen ions in the 0.002M H2SO4 solution will be 0.004M. We can then use the equation pH = -log[H+] to calculate the pH of the solution. Plugging in the concentration of hydrogen ions, we get
pH = -log[0.004] = 2.40
So, the pH of a 0.002M H2SO4 solution is 2.40. 🤓
This calculation gives us a general idea of the pH of a solution, but in reality, the pH may be slightly different due to the presence of other ions in the solution. However, this calculation is a good starting point for understanding the basic pH of a solution. 🤓