Paul Milham
If you cannot find a recipe I suggest that you calculate the required amount of one of the ammonium citrate salts that will give abour the pH you want
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Nigel Gale
Calculating the amount of ammonium citrate: First, you will need to calculate how much ammonium citrate to add. Ammonium citrate is a source of ammonia, and 1 mole of ammonium citrate will contain 1 mole of ammonia. The molar mass of ammonia is approximately 17 g/mol. Since you want your solution to contain 42 g/L of ammonia nitrogen, and considering that nitrogen is approximately 82.35% of the mass of ammonia, you would want approximately (42 g/L) / 0.8235 = 51 g/L of ammonia. Therefore, you will need 51 g/L * 0.2 L = 10.2 g of ammonia, which equates to 10.2 g of ammonium citrate for 200 ml of solution. Preparation: Dissolve 10.2 g of ammonium citrate in about 150 mL of distilled or deionized water. Adjusting the pH: Slowly add ammonium hydroxide (NH4OH) or another suitable base to increase the pH of the solution. It is important to add this slowly while stirring, to ensure that the base is fully mixed into the solution. Monitor the pH using a pH meter until the pH reaches the desired range of 9.4 to 9.7. Adjusting the volume and density: After the pH is adjusted, add more water to bring the total volume of the solution to 200 mL. The density of the solution might be around the desired 1.082 to 1.083 range due to the presence of ammonium citrate and ammonium hydroxide. However, precisely achieving the desired density range might require further fine-tuning of the concentration of the components or the addition of another component that doesn't affect the pH or ammonia nitrogen content. Verification: Verify the solution meets all criteria (pH, density, and ammonia content). You may need to use an analytical method to determine the concentration of ammonia nitrogen in the solution to confirm that it is indeed 42 g/L.
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