2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

A student is asked to standardize a solution of barium hydroxide. He weighs out 0.952 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid).It requires 15.6 mL of barium hydroxide to reach the endpoint.A. What is the molarity of the barium hydroxide solution?  This barium hydroxide solution is then used to titrate an unknown solution of hydrochloric acid.B. If 21.0 mL of the barium hydroxide solution is required to neutralize 21.7 mL of hydrochloric acid, what is the molarity of the hydrochloric acid solution?

In this assignment, you will determine the mass % of an unknown sample of baking soda (NaHCO3) by titrating it with an HCl solution of known concentration.  The laboratory will open with a beaker on the stir plate with 1.5000 g of impure solid NaHCO3 and with sufficient water added to make the total volume 25.00 mL. The buret will be filled with 0.3015 M HCl. Pouring HCI until pH is 2. The volume in the buret went from 0 mL to 43 mL Question 1: Calculate the moles of HCl transferred during the titration. (number and unit) (Keep four significant digits in all of the calculations.) Question 2: How many moles of NaHCO3 are present in the sample? Question 3: What mass of NaHCO3 is present in the sample? Question 4: What percent of the original sample mass was NaHCO3?

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.150 M NaOH.0.150 M NaOH. It requires 20.2 mL20.2 mL of the NaOHNaOH solution to reach the end point of the titration.   What is the initial concentration of HClHCl? concentration:   M HCl