What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below?
To calculate the molarity of HCl solution, you would first titrate it against a known concentration of a base (e.g., NaOH) and use the stoichiometry of the reaction to determine the molarity of the HCl. The factor for the HCl solution would be the ratio between the molarity determined experimentally and the intended molarity. For the borax solution, you would titrate it against a standardized HCl solution to determine its molarity. The factor for the borax solution would similarly be the ratio of the experimental molarity to the intended molarity of the borax solution.
Titrate it with a standard base.
Titrate is a process used in chemistry to determine the concentration of a substance in a solution. It involves slowly adding a solution of known concentration (titrant) to another solution until a reaction is complete, allowing the concentration of the unknown substance to be calculated.
The balanced chemical equation for the reaction between NaOH and H2SO4 is 2NaOH + H2SO4 ⟶ Na2SO4 + 2H2O. From the equation, it is a 1:1 ratio of NaOH to H2SO4. Therefore, to neutralize 10.00 ml of 0.526 M H2SO4, you will need the same amount of 0.526 M NaOH, which is 10.00 ml.
titrate with mercuric nitrate solution
If you titrated to a dark pink color, it signifies that you have overshot the endpoint and added excessive NaOH. This would make your calculated molarity of NaOH too high due to the excess base added beyond the equivalence point, affecting the accuracy of the results.
Titrate it with a primary standard
Double titration is a titration method used to determine the concentration of a solution by performing two successive titrations. In the first titration, a known concentration of a standard solution is used to titrate the unknown solution. In the second titration, a different standard solution is titrated with the excess volume from the first titration to determine its concentration.
Firstly, write out and balance your equation (as always!); this'll also require calculating the Molarity (mol of solute/ ml of solution). Next, you should already have an indicator (litmus strips or even red cabbage juice will work). Then add exactly the amount needed to neutralize the intended reagents. If you're doing the work on paper only, ignore this part: However, have you considered baking soda as opposed to NaOH? It's less dangerous.
To prepare a buffer solution which may be acidic. Titrate ethanoic acid (weak acid) with sodium ethanoate(salt).
A chemical reaction must exist between the titrant an the ion to be analyzed.
You could use a standardized solution of potassium permanganate (KMnO4) to titrate an oxalic acid solution. Potassium permanganate is a strong oxidizing agent that reacts with oxalic acid in an acidic medium, forming carbon dioxide gas, manganese dioxide, and water.