Enter the target concentration and volume to find how much salt to weigh or how much concentrated reagent to measure. Then enter the primary-standard titration to get the actual concentration and the correction factor.
Pre-sizing and estimating tool: results do not replace design, calculations or reports signed by a licensed professional, nor verification against the applicable codes and standards.
Actual concentration from the primary standard mass and the volume used.
Concentration in each flask of the series, on a log scale, starting from the actual concentration.
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For HCl, normality equals molarity. 37% acid with a density of 1.184 g/mL is about 12.0 mol/L, so measure 0.1 × 1000 ÷ 12.0 = 8.32 mL, add it to about 500 mL of water in a 1 L flask and make up to the mark after it cools. Because bottle strength varies, standardize the solution afterwards.
Because the real strength of reagents varies: HCl loses gas, NaOH picks up water and CO₂ from air and labels give ranges. Titrating a primary standard measures the actual concentration. In the example, 0.1300 g of sodium carbonate used a net 24.35 mL, giving 0.1007 mol/L and a factor of 1.0069.
The mass to weigh uses the molar mass of the salt including crystal water. For sodium thiosulfate pentahydrate, M = 158.11 + 5 × 18.015 = 248.18 g/mol; 1 L of 0.1 mol/L needs 24.82 g of the pentahydrate versus 15.81 g if anhydrous.
Potassium hydrogen phthalate (KHP) for NaOH and KOH; dried sodium carbonate for HCl and H₂SO₄; sodium oxalate for KMnO₄; potassium iodate or potassium dichromate for thiosulfate; sodium chloride for AgNO₃; calcium carbonate for EDTA. Dry the standard as the method says and keep it in a desiccator.
Enough to use most of the burette without going past 90%, because reading error weighs less on larger volumes. For 0.1 M HCl and a 25 mL burette, about 0.106 g of sodium carbonate takes roughly 20 mL; the suggested-mass result does that math for the chosen standard.
Always add acid to water, slowly and with stirring, never the reverse, especially with sulfuric acid. Work in a fume hood with HCl, HNO₃ and ammonia, wear splash goggles, gloves and a lab coat, and keep an eyewash nearby, as your Chemical Hygiene Plan requires. Label the bottle with name, concentration, factor, date and initials.
It is diluting several times by the same factor, each time from the previous flask. With a factor of 10 and three steps, the 0.1007 mol/L solution becomes 0.0001007 mol/L taking 10 mL into each 100 mL flask. It is how very dilute calibration standards are made with volumes that are easy to measure.
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