A 30.84 ml sample of 0.128 M NaOH id needed to reach an endpoint for a titration of a 5.441 gram sample of vinegar. Calculate the % acetic acid in the vinegar sample.
A 0.405 gram sample of KHP is dissolved in 50 ml of water . The sample is then titrated with 15.5o ml of NaOH solution. What is the molar concentration of the NaOH solution?
A 25.0 ml aliquot of an HCl solution of unknown concentration is pipetted into a 125 ml Erlenmeyer flask. Three drops of indicator are added and the resulting solution is titrated to the endpoint with 35.0 ml of 0.1005 M NaOH. What is the molar concentration of aliquot?
As the acid solution is titrated with the base, the pink color forms where the drops hit the solution but them disappear when the solution is mixed until the endpoint is reached and the color persists. Explain why this happens?
If the pink solution you obtain when the titration is complete is allowed to stand the color will eventually fade and the solution will again be colorless. Explain how this could happen.
Oxalic acid ( a diprotic acid MW= 90.0 g/mol) is sometimes used instead of KHP for the standardization of NaOH . If a 0.145 gram sample of Oxalic acid is titrated to a phenolphthalein endpoint with 23.75 ml of the NaOH solution, calculate the molar concentration of the base. ( Hint: What is the balanced equation for NaOH and a diuretic acid)
Please answers the question. Thanks!