Question

HCL reacts with NaCO3 forming NaCl waters and carbon dioxide this equation is balanced as written: 2HCl (aq) + Na2 CO3(aq) right arrow 2NaCl (aq) +H2O (l) + CO2)g)

1- what volume of 2.50 M HCL in liters is needed to react completely ( with nothing left over) with 0.750 L of 0.200 M Na2CO3?

Express your answer usining Three sig figs and indicate the appropriate units

2- a 531 ml sample of unknown HCL solution reacts completely with Na2CO3 to form 17.1g CO2. What was the concentration of the HCL solution?

Express your answer using Three sig figs and include the appropriate units.

Answer 1

Ans 1 :

Number of moles of Na2CO3 = 0.750 x 0.200 = 0.15 moles

1 moles of Na2CO3 requires two moles of HCL according to the balanced reaction

So 0.15 moles of Na2CO3 will require 0.15 x 2

= 0.30 moles of HCl

Ans 2 :

17.1 g of CO2 = 17.1 / 44 = 0.39 moles

1 mole of CO2 is formed by 2 moles of HCl in the balanced chemical reaction

So number of moles of HCl required by 0.39 moles will be 0.39 x 2 = 0.78 moles

Concentration of HCl = no. of moles / volume of HCl in L

= 0.78 / 0.531

= 1.47 M