The flask contains 10.0 mL of HCl and a few drops of indicator. The buret contains phenolphthalein 0.150 M NaOH. It requires 16.2 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: M HCI

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?

An analytical chemist weighs out 0.045 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1800 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 4.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol

You are given a package of chemical material to make an identification. The only known information about 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?