Chemistry 1223 Molar Weight of a Solid Acid Laboratory Exercise An unknown acid is chosen from the list in the 1223 Lab Procedure. Determine the Identify the unknown diprotic acid. The procedure for identifying an unknown acid is exactly as described in the lab manual. Part 1: Standardization of NaOH. 1.4378 g of oxalic acid was dissolved in 250.0 mL of water and a 25.00 mL aliquote was titrated with NaOH. 24.73 mL of titrant was required. Determine the concentration of sodium hydroxide. Answer: Part 2: Titration of the diprotic unknown acid. 1.9875 g of the unknown acid was dissolved in 250.0 ml of water and 25.00 ml of this solution was titrated with the NaOH. 29.50 mL of titrant was required. Determine the Molar Mass of the diprotic unknown. units g/mol Answer: MyASUS

A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to HCl. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.20 ml of 0.100M NaOH? Select one:a. 9.80b. 10.26c. 9.90d. 11.08

You set up a titration in the lab to determine the concentration of an HCl solution. What is the molarity of an HCl solution if 0.0100 L of 0.245 M NaOH soln’ are required to neutralize 0.0150 L HCl?      2.25 M     0.163 M     1.34 M     0.245 M

A 25.00 mL sample of magnesium hydroxide solution is titrated with 0.00500 M HCl and 2 drops of methyl orange indicator. The endpoint of the titration is reached when 14.65 mL of HCI has been added. How many moles of hydroxide are present in the sample? O A. 1.25 x 10^-4 moles O B. 6.60 x 10^-5 O C. 2.64 x 10^-5 O D. 7.33 x 10^-5 moles