00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M.  Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH.   Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL        0.1506 M      0.0753 M      0.0376 M      0.1431 M      0.0526 M

Please explain

A 1.8M HCl solution was standardized against 1.4g sodium carbonate Na2CO3  (MW = 106g/mol) . The Na2CO3 standard required 13.5 mL of the HCl solution to completely react up to the indicator endpoint. Two chemists prepared their samples by taking 12.0-mL aliquots of each household ammonia solution and diluting it to 25.0 mL. With the same titrant and indicator, Chemist #1’s ammonia solution required 15 mL of the standardized titrant, whereas, Chemist #2's ammonia solution required 35 mL of the same titrant. Write the balanced equation for the analyte and the titrant Solve for the exact concentration of the HCl titrant in molarity. What are the respective concentrations of ammonia of Chemist #1's sample and Chemist #2's samples in Molarity?

Using the volumes from trial 1 determine the molarity of hcl show set up