As background, an antacid contains an unknown number ofmilligrams (mg) of CaCO3 per 2.0 g tablet according to the label.(CaCO3: 100.09 g/mol). Based on the questions below, determine themg of CaCO3 in the 2.0 g tablet. The reaction by which the antacidneutralizes HCl is 2 HCl(aq) + CaCO3(s) --> CaCl2(aq) + CO2(g) +H2O(l) Q1: How many moles of HCl are neutralized by one mole ofCaCO3(s)? ___ mol Q2: 50.0 mL of 0.300 M HCl are added to anErlenmeyer flask containing a 2.00 g antacid tablet. Calculate themoles of acid in the 50.0 mL of 0.300 M HCl? ___ mol Q3: A studentfills her burette with NaOH to the 2.5 mL mark. She titrates hersample of the NaOH until she reaches the endpoint (i.e. all theacid has been neutralized by the NaOH). The volume marking on herburette - at the endpoint - is 52.5 mL. How many mL of NaOH did sheuse to reach the endpoint? Q4: Some of the 2.0 g of antacidneutralizes the HCl. However, there is excess acid, not neutralizedby the antacid. To determine the excess moles of acid, a studentused 50.00 mL of 0.100 M NaOH to titrate the excess acid. How manymoles of excess acid are there? ___ mol HCl Q5: How many moles ofHCl were neutralized by the 2.0 g antacid tablet? ___ mol Q6: Howmany mg of CaCO3 were in the original 2.00 g tablet? ___ mg