# Mass of ammonia through nitrate concentration problem

• Frankenstein19
In summary, Homework Statement states that the nitrate concentration in an aquifer is 20 ppm, and its volume is ten million liters. It is possible that 1mg/L equals 1ppm, and NH3+O2-->NO3- (through aerobic contitions and nitrification, idk if this is applicable >: ). The Attempt at a Solution calculates that there is an equal amount of ammonium?1:1 in terms of moles, not mass. After you are sure about that, you have to convert the nitrate mass into ammonium mass as Borek and the question itself have indicated.
Frankenstein19

## Homework Statement

The nitrate concentration in an aquifer is 20 ppm, and its volume is ten million
liters. What mass of ammonia upon oxidation would have produced this mass of
nitrate? [Hint: The moles of nitrogen in reactant and product are identical.]

## Homework Equations

Possibly 1mg/L & NH3+O2---->NO3-

## The Attempt at a Solution

Since 1mg/L equals 1ppm then I'd get a 2*10^8mg for nitrate mass. And NH3+O2---->NO3- (through aerobic contitions and nitrification, idk if this is applicable >: ) then the 1:1 ratio means there's an equal amount of ammonium?

1:1 in terms of moles, not mass.

Frankenstein19 said:

## Homework Statement

The nitrate concentration in an aquifer is 20 ppm, and its volume is ten million
liters. What mass of ammonia upon oxidation would have produced this mass of
nitrate? [Hint: The moles of nitrogen in reactant and product are identical.]

## Homework Equations

Possibly 1mg/L & NH3+O2---->NO3-

## The Attempt at a Solution

Since 1mg/L equals 1ppm then I'd get a 2*10^8mg for nitrate mass. And NH3+O2---->NO3- (through aerobic contitions and nitrification, idk if this is applicable >: ) then the 1:1 ratio means there's an equal amount of ammonium?

Why not be a bit simpler? You have 20 parts per million, then if you have 1 million, 20 parts of it is 20, 20 parts per million of 10 million is 200!

We have a disagreement there by a factor of 1000.

After you are sure about that, you have to convert the nitrate mass into ammonium mass as Borek and the question itself have indicated.

Do they really use these units? I suppose it is in order to give the general public an idea they can appreciate of the concentrations?

For anyone knowing a bit of chemistry It sounds rather odd - ppm would be okay to give as a formula for somebody to weigh out grams to be put in a lake or something. You can weigh out sodium nitrate or calcium nitrate, but there is no substance called just 'nitrate' that you can weigh out.

epenguin said:
For anyone knowing a bit of chemistry It sounds rather odd - ppm would be okay to give as a formula for somebody to weigh out grams to be put in a lake or something. You can weigh out sodium nitrate or calcium nitrate, but there is no substance called just 'nitrate' that you can weigh out.

Come on, in many places we report things using proxies - like amount of P2O5 in fertilizer. For me NO3- doesn't sound worse than ammonia or just nitrogen, the meaning is obvious

## 1. What is the mass of ammonia produced from a given concentration of nitrate?

The mass of ammonia produced from a given concentration of nitrate can be determined by using the balanced chemical equation for the reaction between nitrate and ammonia. This equation will give the molar ratio between the two substances, which can then be used to calculate the mass of ammonia based on the concentration of nitrate.

## 2. How is the concentration of nitrate related to the mass of ammonia produced?

The concentration of nitrate is directly proportional to the amount of ammonia produced. This means that as the concentration of nitrate increases, the mass of ammonia produced will also increase. This relationship is determined by the balanced chemical equation for the reaction between nitrate and ammonia.

## 3. What units are used to express the mass of ammonia and concentration of nitrate?

The mass of ammonia is typically expressed in grams (g) or kilograms (kg), while the concentration of nitrate is typically expressed in moles per liter (mol/L) or milligrams per liter (mg/L).

## 4. How can the mass of ammonia and concentration of nitrate be experimentally determined?

The mass of ammonia and concentration of nitrate can be experimentally determined by conducting a chemical reaction between the two substances and measuring the resulting mass of ammonia or the change in concentration of nitrate. This can be done in a controlled laboratory setting or through field sampling and analysis.

## 5. What factors can affect the accuracy of the mass of ammonia and concentration of nitrate calculations?

The accuracy of the mass of ammonia and concentration of nitrate calculations can be affected by various factors such as experimental errors, impurities in the reactants, incomplete reactions, and changes in environmental conditions. It is important to carefully control and monitor these factors to ensure accurate results.

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