A student is given a solution containing 0.932 g of an unknown acid, H2A(aq) To determine the molar mass of the acid, the student titrates the sample using a 0.481 M solution of KOH(aq). 1. Write the balanced equation for the reaction taking place. Include states of matter.

2. If 28.9 mL of KOH is required to consume the acid completely, calculate the moles of H2A.

3. Calculate the molar mass of H2A.

Achemical equilibrium between gaseous reactants and products is shown. n2(g) + 3h2(g) ⇌ 2nh3(g) how will the reaction be affected if the pressure on the system is increased? it will shift toward the reactant side as there is lower pressure on the reactant side. it will shift toward the product side as there is higher pressure on the product side. it will shift toward the reactant side as there are a greater number of moles of gas on the reactant side. it will shift toward the product side as there are a fewer number of moles of gas on the product side.