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To calculate the pH after each volume of NaOH is added, you need to determine the moles of HBr initially, moles of NaOH added, and then use these values to calculate the final concentration of H3O+ ions in the solution. From there, you can calculate the pH using the equation pH = -log[H3O+]. Repeat these calculations for each volume of NaOH added to find the pH at 12.5 ml, 18.7 ml, 20.0 ml, 29.5 ml, and 34.2 ml.
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A 50.0 ml sample of 0.43 m benzoic acid c6h5cooh is titrated with 0.50 m naoh calculate the pH at the equivalence point ka of c6h5cooh equals 6.5 10-5?
At the equivalence point, the moles of NaOH added will equal the moles of benzoic acid initially present in the sample. Since benzoic acid is a weak acid, it will partially dissociate in solution to produce benzoate ions and protons. At the equivalence point, all the benzoic acid has been converted to benzoate ions, resulting in a buffer solution of benzoate and its conjugate base. To calculate the pH at the equivalence point, you can use the Henderson-Hasselbalch equation, which considers the concentration of benzoate ions and benzoic acid to determine the pH of the solution.
How do you calculate non volatile matter percentage in a solution?
Non volatile matter = [(W2-W1)/V] x 100 where W2 :Weight of beaker [Before sample addition & evoporation] W1 :Weight of beaker [after sample evoporation] V : Volume of sample taken
A sample of 76g of NaCl is dissolved to make 1L of solution. what is the molarity of the solution?
1.3g
What is the procedure for determining the percentage purity of amino acid sample by sorenson formol titration method?
To determine the percentage purity of an amino acid sample using the Sorenson formol titration method, you would first prepare a standard solution of formaldehyde. Then, titrate the standard formaldehyde solution with the amino acid sample. Calculate the percentage purity of the amino acid sample using the volume of formaldehyde solution consumed during titration and known concentrations of the solutions used.
How do you make a pure sample of salt?
Sodium hydroxide is an alkali. If you take solutions of hydrochloric acid and sodium hydroxide that have the same concentration, and mix equal volumes of them, the sodium hydroxide neutralises the acid. if you take tests with the solution on universal indicator paper, you will find it has pH7. If you leave the solution to evaporate, you will see crystals of salt. This is the kind of salt you put on your chips but remember not to eat them in a laboratory! =)
A 30.0 ml sample of 0.200 m koh is titrated with 0.150 m hclo4 solution calculate the pH after 39.9 ml of hclo4 is added?
To solve this problem, you first need to determine the moles of KOH present in the 30.0 mL sample. Then calculate the moles of HClO4 added after 39.9 mL. Based on these concentrations, determine the excess and limiting reagents to find the resulting pH. Consider the reaction that occurs between KOH and HClO4, and use the stoichiometry to calculate the amount of products formed. Finally, calculate the pH using the concentration of the resulting solution.
A 25 ml sample of 723 m hclo4 is titrated with a 273 m koh solution the h3o concentration after 66.2 ml of koh is?
The balanced chemical equation for the reaction between HClO4 and KOH is HClO4 + KOH → KClO4 + H2O. By using the stoichiometry of the reaction, you can calculate the moles of HClO4 reacted with KOH. Then, use the remaining volume of KOH solution added to calculate the final H3O+ concentration in the solution.
Why is it necessary to filter different volume of sample?
It is necessary to filter in different volumes of a sample because it may take more or less liquid for a solid to completely dilute in the solution. The amount of solution you use is completely dependant on the formula.
In equal volumes of normal rainfall and baking soda solution which sample would have a greater amount of hydrogen ions?
normal rainfall
How do you determine the concentration of ascorbic acid in unknown sample?
first measure the volume of the sample solution needed to change the blue color of the DCPIP solution into colourless. then, weigh the mass of the sample solution. finally calculate the concentration by using the formula: volume required t change the color of DCPIP solution (dm) per mass of the sample solution (g)
Can density of an entire solution be measured from a small sample?
Yes, the density of an entire solution can be estimated through the measurement of a small sample. By accurately measuring the volume and mass of a small sample, you can calculate the density of the entire solution using the formula Density = Mass/Volume.
What science equipment are used during titration?
Some common science equipment used during titration include a burette for delivering precise volumes of titrant, an Erlenmeyer flask or beaker to hold the sample being titrated, a pipette for transferring small volumes of liquids, an indicator to show the endpoint of the reaction, and a magnetic stirrer to ensure thorough mixing.
A 50.0 ml sample of 0.43 m benzoic acid c6h5cooh is titrated with 0.50 m naoh calculate the pH at the equivalence point ka of c6h5cooh equals 6.5 10-5?
At the equivalence point, the moles of NaOH added will equal the moles of benzoic acid initially present in the sample. Since benzoic acid is a weak acid, it will partially dissociate in solution to produce benzoate ions and protons. At the equivalence point, all the benzoic acid has been converted to benzoate ions, resulting in a buffer solution of benzoate and its conjugate base. To calculate the pH at the equivalence point, you can use the Henderson-Hasselbalch equation, which considers the concentration of benzoate ions and benzoic acid to determine the pH of the solution.
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
Using the balanced chemical equation for the reaction between HBr and NaOH (1:1 ratio), we can determine the moles of NaOH used. From the volume of NaOH used, we can then calculate the moles of HBr present in the sample. Finally, dividing moles of HBr by the initial volume of the sample (in liters) gives the molar concentration of HBr.
How do you standardize a solution of NaOH and what reagents to be used?
To standardize a solution of NaOH, you can use a primary standard acid such as potassium hydrogen phthalate (KHP) or oxalic acid. You'll titrate the acid with the NaOH solution until neutralization occurs. The balanced chemical equation for this reaction is typically: NaOH + HX → NaX + H2O, where X is the anion of the acid being titrated.
What happens during a back titration?
During a back titration, a known excess of a standard solution is added to react with the analyte present in the sample. The excess reactant is then titrated with a second standard solution to determine the amount consumed, allowing for the calculation of the original analyte concentration. Back titrations are useful when the analyte is insoluble or when the reaction is slow or inefficient.
Why is sulfuric acid added to the dilute bleach and iodide in the conical flask during titration of sodium hypochlorite with sodium thiosulphate?
Sulfuric acid is added to the bleach and iodide solution to acidify the solution and promote the reaction between hypochlorite and iodide to produce iodine. The iodine produced is then titrated with sodium thiosulfate to determine the concentration of hypochlorite in the sample. Acidifying the solution helps in stabilizing the generated iodine for a more accurate titration.
