A sodium hydroxide solution contains a small amount of sodium carbonate as a result of contamination by atmospheric carbon dioxide. A 25.00-mL aliquot requires 25.62 mL of 0.1021 M HCl to reach the phenolphthalein end point and an additional 0.80 mL to reach the methyl red end point. Calculate the molar concentration of NaOH in the solution. Type the numerical answer only.

Chadwick the chemistry student carries out a titration by adding an aqueous solution of NaOH to an aqueous solution of the weak acid HX. The images below represent the solutions formed at various points during this titration. (Na+ and H2O are omitted for clarity.)   Select the image corresponding to each of the following points in Chadwick's titration. Before adding any NaOH: Solution A, B C, D, or E? Partway to the equivalence point: Solution A, B C, D, or E? At the equivalence point : Solution A, B C, D, or E? After the equivalence point : Solution A, B C, D, or E?

How many mls of 0.125 M HCl must be added to 65.5 mls of 0.234 M NH3 to completely neutralize the NH3

Consider the diagram of an aqueous solution of a soluble ionic compound. 2+ 2+ 2+ Determine which ionic compound is dissolved in solution. 2+ O K,CO3 MgSO, NaNO, O CaCl,

Calculate the change in pH that occurs when 1.0 g NaOH is added to 250 mL of each of the following solutions.a. Pure water b. 0.0200 M NH3 c. 0.100 M NaOHd. 0.250 M HCL e. 0.100 M HClO4   Please answer it correctly. Show complete solutions.

Final Volume Burret

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...

Part 3 Prepare a data table for the titration of NaOH with diluted vinegar. Include enough data columns for at least 3 titrations. PRELAB QUESTIONS 1. Calculate the molar mass of Potassium acid phthalate, KHC8H404 (KHP). You will use this number to do the calculations for part 1 once you do the titration. 2. Calculate the molar mass of acetic acid, HC₂H3O2. You will use this number to do the calculations for part 3 once you do the titration. 3. Solve the following problem: If it takes 35.04 mL of a 0.2455 M NaOH solution to neutralize 25.00 mL of an unknown HCl solution, what is the molarity of the HCl solution? Use the roadmap given under part 2 to calculate this problem. MA Chemistry 60 lab Page 110 3

A 25.0-mL volume of a sodium hydroxide solution requires 19.6 mL of a 0.189 M hydrochloric acid for neutralization. A 10.0-mL volume of a phosphoric acid solution requires 34.9 mL of the sodium hydroxide solution for complete neutralization. Calculate the concentration of the phosphoric acid solution.

23 mL of 0.0916M NaOH neutralizes an unknown volume of 0.12 M HCI. If 74 mL of HCI was added to 0.685 g of TUMS, how much HCI was used to neutralize TUMS? How much HCl will be needed for 0.75 g of TUMS?