Calculate the concentrations of NaOH and maleic acid.
100 mL of 0.1 M NaOH was transferred into a buret. 0.433 g of maleic acid was dissolved in a 100 mL volumetric flask. 25 mL of this solution was transferred into a plastic beaker, and 50 mL of distilled water was added.
6 mL of NaOH was added to get to the first equivalence point (brought pH to 1.99), and a total of 30 mL was added to reach the second point (brought pH to 5.54).
Calculate the concentrations of NaOH and maleic acid. 100 mL of 0.1 M NaOH was transferred...
In the titration of 100 ml of a 0.1 M H3PO4 with 0.5 M NAOH, calculate the pH of the solution at each of the following points: A) before any NaOH added B) After 10 mL of NaOH added C) at 1st equivalence point
Using the standardized concentrations for M(OH)2 and HCl determined in this investigation, calculate the pH for a strong acid + strong base titration in which 5.00 mL of the M(OH)2 was transferred via pipet to a beaker and HCl was added from the buret. concentration M(OH)2 .07 concentration HCl .0512 Calculate the pH: a) before any HCl is added b) after the addition of 4.00 mL HCl c) after the addition of 9.00 mL HCl d) 4.00 mL beyond the...
A student measures out 0.120 g of maleic acid (C4H4O4) and titrates it with 0.100 M NaOH. How many mL of NaOH will be added to reach the second equivalence point? Show your calculations. What would be the volume of NaOH added at the first equivalence point?
3. If 15.0 mL of 0.125 M phosphoric acid is titrated with 0.100 M NaOH, what volume of the titrant (in mL) must be added to completely neutralize the acid? Show all of your work (including the chemical equation). (1 point) Post-lab Questions: Experiment #9: Acid-Base Titrations Student Learning Objectives : Students will gain practice with the accurate preparation of solutions. Students will perform acid-base titrations and prepare titration curves. Students will identify strong and weak acids by the shapes...
We’re going to titrate formic acid with the strong base, NaOH. There is initially 100. mL of 0.50 M formic acid and the concentration of NaOH is 1.0 M. What is the initial pH of the formic acid solution? 2) What is the percent ionization under initial conditions? 3) After the addition of 10 mL of NaOH, what is the pH? 4) After the addition of 25 mL of NaOH, what is the pH? Think about where in the titration...
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
A chemistry student weighs out 0.0768g of ascorbic acid H2C6H6O6, a diprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits.
A chemistry student weighs out 0.217g of hypobromous acid HBrO into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0500M NaOH solution.Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.
A chemistry student weighs out 0.0959 g of acrylic acid (HCH2CHCO2 into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0900 M NaOH solution Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. mL ×10
A chemistry student weighs out 0.0609g of lactic acid HC3H5O3 into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1300M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.