How to conduct an ammonia titration test? How to convert tt into the concentration of ammonia?

This post was last edited by 654262293 on 2010-7-2 16:19. Titer is a common method for indicating the ammonia concentration in a solution. 1 titre = 1/20 equivalent concentration = 1/20 × 17 grams of ammonia per liter = 0.85 grams of ammonia per liter. Percentage concentration = titre of ammonia solution × 0.85 / density (weight) of the solution × 100% = 0.85 × titre of ammonia solution / weight of the solution

1 titre = 1/20 of equivalent concentration. The titrant commonly used to titrate ammonia solution is 1-equivalent dilute sulfuric acid; by knowing the amount of dilute sulfuric acid used in the titration, the concentration of the ammonia solution can be determined, and multiplying this value by 20 gives the titre

The ammonia concentration in an ammonia solution is commonly expressed as a titration value or mass percentage. 1 titre (tt) = 1/20 molar concentration. Since an ammonia solution with a concentration of 1 mole per liter contains 17 g of ammonia per liter, an ammonia solution with a concentration of 1 tt contains: 1 tt = 1/20 molar concentration = 1/20 × 17 g/L = 0.85 g/L. The mass percentage concentration of ammonia indicates the amount of ammonia in grams per 100 g of solution. The mass percent concentration of ammonia solution can be converted to its titration value using the following formula: Mass percent concentration of ammonia solution = Titration value of ammonia solution × 0.85 / Concentration of ammonia solution × 100% = 85 × Titration value of ammonia solution / Solution density %.

This post was last edited by chen3jun on 2010-7-5 08:17. 1. Principle: The ammonia content is determined using the neutralization method; the reaction equations are as follows: 2NH4OH + H2SO4 ===(NH4)2SO4 + 2H2O; 2NH4HCO3 + H2SO4 ===(NH4)2SO4 + 2CO2↑ + 2H2O; (NH4)2CO3 + H2SO4 ===(NH4)2SO4 + CO2↑ + H2O; 2NH4HS + H2SO4 ===(NH4)2SO4 + 2H2S↑. 2. Instruments: ① Erlenmeyer flask: 250 ml; ② Pipette: 1 ml; ③ Titration tube: acid type, 50 ml. 3. Reagents: ① Standard sulfuric acid solution, i.e., 1N sulfuric acid. ②Methyl orange indicator: 0.1%. 4. Procedure for determination: ① Accurately transfer 1 ml of the solution into a 250 ml Erlenmeyer flask containing 50 ml of distilled water, and add 3 drops of 0.1% methyl orange indicator. ②Rapidly titrate with a sulfuric acid standard solution until an orange-red color is reached. 5. In the calculation formula, V1 represents the volume of the standard sulfuric acid solution consumed during titration, in ml; N represents the equivalent concentration of the standard sulfuric acid solution. V—Volume of the solution absorbed, in ml. 20—Conversion factor between molar concentration and titration value. 6. The neutralization reaction between sulfuric acid and ammonia can be simplified as follows: 2(NH4+) + SO42- → (NH4)2SO4. It can be seen that 1 mole of ammonium ions reacts with 0.5 moles of sulfate ions. Or rather ； 1 mole of ammonium ions reacts with 1 equivalent of sulfuric acid. Therefore, the ammonia content can be calculated from the amount of sulfuric acid used. By substituting N=1 and V=1 into the formula, we obtain: the titration degree of ammonia = V1×20 (tt), where V1 is the volume of the standard sulfuric acid solution consumed during titration, in ml