c. Use the pH curve, and the information show in the table above, to select the most appropriate indicator to show the end-point of this titration. State the colour change that would be observed.

Give the letters of the solutions below that represent buffers. (a) a solution of oxalic acid and potassium hydrogen oxalate; (b) a solution of formic acid and potassium formate; (c) a solution of potassium sulfate and potassium hydroxide; ( d) a solution of methylamine and methylammonium chloride.

Interpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0

A 27.4 mL sample of 0.356 M ammonia, NH3, is titrated with 0.279 M hydrobromic acid. At the titration midpoint, the pH is Use the Tables link in the References for any equilibrium constants that are required.

How many milliliters of 1.27 M NaOH must be added to 275 mL of 0.11 M H₂PO4 to make a buffer solution with a pH of 6.407 Round your answer to 2 significant digits. Note: Reference the pK, of weak acids at 25 °C table for additional information,

Solve only D ...   Don't provide handwriting solutions....

It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form.  b) After the HCl was added, essentially all the indicator was in the HIn form.  Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.

How can we answer these questions? 1) What other methods could you have used to identify the unknown chemical? 2). What is/are the dominant species in solution at pH = 4.4? 3) Does the solution at pH = 4.9 constitute a buffer? What about at pH- 5.9? Explain

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working