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Can you titrate a solution of unknown concentration with another solution of unknown concentration and still get a meaningful answer?
yes you can, however you need the chemical coumpound name, how many grams of that chemical compound was used, and the litres that it was mixed with.
for example:
2g of NaF was used to mix in a 1L solution
(NaF has a molas mass of about 42g)
2g of NaF x 1 mol/42g (grams cancel and left with mols)
0.048mol/1L = 0.048mol/L conentartion
What else can I help you with?
If 81.7 ml of 1.34 m hno3 were used to titrate 56.3 ml of an lioh solution find the concentration of the lithium hydroxide?
moles HNO3 ---> (1.34 mol/L) (0.0817 L) = 0.109478 molHNO3 and LiOH react in a 1:1 molar ratio.This means 0.109478 mol of LiOH was neutralized.molarity LiOH ---> 0.109478 mol / 0.0563 L = 1.944547 MThe sig figs yields 1.94 M for the answer.
What experiment can you do to prove neutralisation?
check the pH, there are many methods for this. simple pH paper or probes. Or you could titrate
Why is HCl added before titration?
Without the specific details, one cannot be sure, but this is probably a back titration. You add a known amount of acid to your unknown, then titrate to measure how much has not reacted. You can then calculate how much of your first chemical must have been present.
When a 3.529 g sample of Liquid-Plumr was titrated with 0.1025 M HCl two end points were obtained. The first end point occurred at 16.33 mL the second at 41.58 mL. Calculate the mass percent of both N?
Liquid-Plumr is a chemical drain opener made of 0.5-2% sodium hydroxide (NaOH, M=40,00 g/mol) and 5-10% sodium hypochlorite (NaClO, M=74.44 g/mol), and a surfactant (detergent, unknown), according to the producer Clorox (to calculate mass% these underscored date are essential)The first part of this titration is for NaOH, being the strongest alkali:0.1025(mmol/mL)*16.33(mL)*40.00(mg/mmol)*0.001(g/mg) / 3.529(g) * 100% = 1.897% NaOHThe second part is for NaClO, a weak, though still titrable base when the right indicator is used.At first it is assumed that the total volume was 41.58 mL, so the second part of this titration only took (41.58-16.33) = 25.25 mL (net value), then 0.1025(mmol/mL)*(25.25) (mL)*74.44(mg/mmol)*0.001(g/mg) / 3.529(g) * 100% = 5.458% NaClO(this looks this most reasonable value to me, because the tatration can be done with one buret filling)However, if 41.58 mL is used to titrate the second part (thus total volume would have been 59.91) then:0.1025(mmol/mL)*(41.58)(mL)*74.44(mg/mmol)*0.001(g/mg) / 3.529(g) * 100% = 8.988%(I would advise to use a smaller weight of sample next tim, e.g. about 2 gram LP)Note: all value were calculated in 4 signifcant digits according to the given figures.However this does not suggest that the outcomes are as accurate; at least triplicate titrations on 3 different weights (amounts) of the same sample are needed for an accuracy of
What is titrate?
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.
What must be done to determine the concentration of a non standard solution?
Titrate it with a primary standard
What is The process of adding a known amount of solution of known concentration to determine the concentration of another solution is called?
titration is the best method to determine the unknown concentration of the unknown. if ur known is a solid then you would have to used distilled water to ensure it is submerged before you titrate.
In a titration what two things are always equal to each other at the endpoint?
In a titration, the moles of the titrant added are equal to the moles of the analyte in the solution at the endpoint. This equality is essential for determining the concentration of the analyte in the solution.
How do you standardise 0.1M HCl?
To standardize 0.1 M HCl, you would first need to titrate it against a solution of known concentration, usually sodium hydroxide (NaOH). By carefully adding the NaOH solution to the HCl solution until the reaction is complete, you can determine the exact concentration of the HCl solution. This process allows you to adjust the concentration of the HCl solution to the desired 0.1 M.
How do you standardize 1N H2SO4 with a KHP?
To standardize 1N H2SO4 with KHP, you would first prepare a solution of KHP of known concentration. Then, titrate the KHP solution with the 1N H2SO4 solution until the endpoint is reached. The volume of H2SO4 used in the titration can then be used to calculate the exact concentration of the H2SO4 solution.
Standardization of hcl solution with primary standard na2co3 solution?
To standardize an HCl solution with a primary standard Na2CO3 solution, first, prepare a Na2CO3 solution of known concentration. Then, titrate the Na2CO3 solution with the HCl solution using a suitable indicator until the equivalence point is reached. From the volume of HCl solution used and the known concentration of Na2CO3, you can calculate the exact concentration of the HCl solution.
Can you provide me with the proper procedure for conducting a titration, as outlined in the lab manual?
To conduct a titration, first prepare the solution of known concentration in a burette. Then, add the solution of unknown concentration to a flask with an indicator. Slowly titrate the known solution into the flask until the indicator changes color. Record the volume of the known solution used. Repeat the titration until consistent results are obtained. Calculate the concentration of the unknown solution using the volume and concentration of the known solution.
How do you standardization 1N hcl?
To standardize 1N HCl (hydrochloric acid), you would typically use a primary standard base, such as sodium hydroxide (NaOH), of known concentration to titrate the HCl solution. By carefully titrating the HCl with the NaOH, you can determine the exact concentration of the HCl solution. This information can then be used to adjust the concentration of the HCl solution as needed to make it accurately 1N.
How we standrise sodium carbonate solution?
Titrate it with a standard base.
Why titrate a flask?
Titration is a common laboratory technique used to determine the concentration of a substance in a solution. By carefully adding a titrant (a solution of known concentration) to the solution being analyzed until the reaction reaches an endpoint, the exact amount of substance in the solution can be quantified. Titrating in a flask allows for controlled mixing and easy observation of color changes or other indicators.
What is double titration?
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.
