Two 25.0-ml. samples of unknown monoprotic weak acids, A and B, are titrated with 0.100 M NAOH solutions. The titration curve for each acid is shown below. ACID A ACID B 14 14 12 12 10 10 10 15 20 25 30 35 40 45 30 10 15 20 25 o 33 40 45 30 Volume of NaOH added (ml.) Volume of NaOH added (ml) Part A Which of the two weak acid solutions is less concentrated? A Submit Bequest Answer

A 28.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1422 MM KOHKOH solution. A volume of 43.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution?         Express your answer using four significant figures.

moles of NaOH moles moles of acid moles Concentration of acid in original sample in M Volume in mL

Which statement about acid-base indicators is not correct? *       A- A weak acid can be used as an acid-base indicator provided that the chemical structures of the weak acid and its conjugate base differ slightly.       B- The end point of the titration is not a specific colour but the point where one drop of acid or base from the burette changes the colour of the solution in the conical flask.       C- Phenolphthalein can be used to detect the end point of the titration of a strong base with a weak acid.       D- All these statements are correct.       E- None of these statements are correct.

You are given a package of chemical material to make an identification. The only known information of this package is that it is a monoprotic acid. You dissolved 1.0 g of the acid into 100 mL of water and titrated it with 0.1 M NaOH solution. The equivalence point was found after titrating 118.4 mL NAOH solution. What is this unknown acid?

Question 9