Suppose a student needs to determine the concentration of a NaOH solution. He performed a standardization titration using the primary standard, benzoic acid. mass of NaOH (g) 1.550 volume of NaOH solution (mL) 250.0 mass of benzoic acid (g) 0.705 volume of benzoic acid solution (mL) 100.0 volume of NaOH dispensed (mL) 40.12 What is the expected concentration of the solution? The molar mass of sodium hydroxide is 39.997 g/mol. and the molar mass of benzoic acid is 122.12 g/mol. 0.1431 expected concentration of NaOH: Incorrect What is the actual concentration of the NaOH solution based on the experimental results? actual concentration of NaOH: 0.1438 M M

What volume, in mL, of 0.1126 M sodium hydroxide (NaOH) is required to titrate 15.00 mL of 0.1012 M acetic acid (HC₂H₂O₂)? Be sure your answer has the correct number of significant digits. mL X

The normality of an aqueous solution of hydrobromic acid is determined by titration with a 0.151 N sodium hydroxide solution. If 32.8 mL of sodium hydroxide are required to neutralize 16.7 mL of the acid, what is the normality of the hydrobromic acid solution? N

Acetic Acid Titration with NaOH. 50.00 ml of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to reach the endpoint of the titration. What is the molarity of the acetic acid solution? (Do NOT include units)

A 1.054-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The resulting solution is titrated with NaOH solution of unknown concentration. If 22.50 mL of the base (NaOH) is needed to reach the equivalent point, what is the molar concentration of NaOH solution? The reaction occurs as follows: NaOH(aq) + KHC3H4O4(aq) NaKCgH404(aq) + H2O(I) --> (A) 0.07119 M (B) 0.1147 M (C) 0.1424 M (D) 0.2294 M

Suppose you are titrating vinegar, which is an acetic acid solution of unknown concentration, with a sodium hydroxide solution according to the equation HC₂H3O2 + NaOH →→→ H₂O + NaC2H3O2 If you require 30.40 mL of 0.1769 M NaOH solution to titrate 10.0 mL of HC₂H3O2 solution, what is the molar concentration of acetic acid in the vinegar? Type answer:

A 0.15 M solution of HCl is used to titrate 30.0 mL of a Ca(OH)2 solution of unknown concentration. If 140.0 mL of HCl is required, what is the normality of the Ca(OH)2 solution? What is the molarity?

Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of citric acid to be 192.124 g/mol. Give your answer to one decimal place. initial volume (mL) final volume (mL) Buret reading (mL) 1.75 14.32

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1886 M0.1886 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.42 mL12.42 mL of the standard solution. What is the concentration of the original sulfuric acid solution?

A 1.22 g sample of KHP is used to titrate a NaOH solution.  A student finds that it requires 15.00 mL of the NaOH solution to reach the end point.  What is the molarity of the NaOH solution?