Describe the process of standardizing hydrochloric acid (Solution A) using sodium hydrogen carbonate and the calculations involved.

You're on a roll — This problem involves preparing a standard solution, performing titrations, and calculating concentrations. Since no experimental data is provided, the calculations will be demonstrated using example values, and the procedures will be described. Given: Sodium hydrogen carbonate (NaHCO_3) Solution A: Hydrochloric acid (HCl) Solution B: Aqueous Sodium hydroxide (NaOH) Indicators: Phenolphthalein, Methyl orange Molar mass of Sodium hydrogen carbonate (NaHCO_3): Na: 22.99 g/mol H: 1.01 g/mol C: 12.01 g/mol O: 16.00 g/mol Molar mass of NaHCO_3 = 22.99 + 1.01 + 12.01 + (3 × 16.00) = 84.01 g/mol a) Make up a solution of Sodium hydrogen carbonate and use it to standardize solution A. Step 1: Prepare the standard Sodium hydrogen carbonate solution. Weigh accurately between 2.01 g and 2.08 g of solid Sodium hydrogen carbonate using a weighing boat or watch glass. Record the exact mass. (For demonstration, let's assume a mass of 2.05 g). Transfer the weighed NaHCO_3 quantitatively into a 250 cm^3 volumetric flask. Use a funnel to avoid spillage and rinse the weighing boat/watch glass and funnel with distilled water into the flask. Add distilled water to the flask, swirling gently to dissolve the solid. Once dissolved, add more distilled water until the bottom of the meniscus aligns with the 250 cm^3 mark on the volumetric flask. Ensure your eye is at the same level as the meniscus. Stopper the flask and invert it several times to ensure the solution is thoroughly mixed and homogeneous. This is your standard Sodium hydrogen carbonate solution. Step 2: Standardize Solution A (Hydrochloric acid) using the standard Sodium hydrogen carbonate solution. Rinse a burette with Solution A (HCl) and then fill it with Solution A. Ensure no air bubbles are trapped and the initial reading is recorded. Rinse a 25.0 cm^3 pipette with the standard NaHCO_3 solution and then pipette