The volume of 0.300 mol/L HCl that can be completely neutralized by 2.00 g of Ca(OH)2 in a stomach antacid tablet is? Please help me show the work.
Here M of HCl = 0.300 mol/L
Measn 0.300 mol of HCl is present in HCl.
First write the reaction equation;
Ca(OH)2 + 2HCl --> CaCl2 + 2H2O
Now calcualte the number of moles of Ca(OH)2 which will use to neutralized:
0.300 mol of HCl * 1 mol of Ca(OH)2 / 2 mol of HCl
= 0.15 mol Ca(OH)2
Now calcualte the number of moles of Ca(OH)2 as followS:
2.00 g / 74.0927 g/ mol = 0.02699 mol
But here the moles of Ca(OH)2 is less than required mole sof Ca(OH)2 hence it cannot be neutrilized.
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