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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?
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?
What else can I help you with?
Calculating molarity and factor of HCl and Borax solutions in standidization?
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.
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.
How we standrise sodium carbonate solution?
Titrate it with a standard base.
What volume of 0.744 Molarity of NaOH is required to titrate 10.00ml of 0.526 M H2SO4?
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.
Would your calculated molarity of NaOH be too high too low or unaffected if you titrated to a dark pink color?
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.
What is the chloride test procedure for waste water?
titrate with mercuric nitrate solution
What must be done to determine the concentration of a non standard solution?
Titrate it with a primary standard
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.
How do you standardize the sodium hydro oxide solution with oxalic acid?
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.
How do you prepare buffer solution?
To prepare a buffer solution which may be acidic. Titrate ethanoic acid (weak acid) with sodium ethanoate(salt).
How many milliliters of a stock solution of 11.4 m hno3 would you have to use to prepare 0.500 l of 0.470 m hno3?
To prepare 0.500 L of 0.470 M HNO3 solution, you would need 103.6 mL of the 11.4 M stock solution. This can be calculated using the dilution formula: M1V1 = M2V2, where M1 is the concentration of the stock solution, V1 is the volume of stock solution needed, M2 is the final concentration, and V2 is the final volume.
How many mL of 0.1010 M HCl will be needed to titrate 0.3151 grams of primary standard Na2CO3?
To determine the volume of HCl needed, first calculate the moles of Na2CO3 using its molar mass. Then use the balanced chemical equation to find the moles of HCl required to fully react with the moles of Na2CO3. Finally, use the concentration of the HCl solution to calculate the volume required using the formula: moles = molarity x volume (in liters).
