if you add 13.75 mL of 1.35M HCl to 22.80 mL of .955 M Ca(OH)2, will you neutralize all the Ca(OH)2?
mols HCl = M x L = ?
mols Ca(OH)2 = M x L = ?
2HCl + Ca(OH)2 ==> CaCl2 + 2H2O
1 mol Ca(OH)2 will neutralize 2 mols HCl.
you need twice the moles of acid as in the base;
moles base=.955*.0228 = .0217moles
moles acid: 1.35*.01375=.0186 moles
you do not have enough acid.
To determine if all the Ca(OH)2 will be neutralized, we need to perform a stoichiometric calculation using the balanced equation for the reaction between HCl and Ca(OH)2.
The balanced equation is as follows:
2HCl + Ca(OH)2 -> CaCl2 + 2H2O
From the balanced equation, we can see that it takes 2 moles of HCl to react with 1 mole of Ca(OH)2. So, we need to convert the given volumes of solutions to moles.
To do this, we first calculate the moles of HCl:
Moles of HCl = Volume of HCl solution (in L) x Concentration of HCl (in mol/L)
Moles of HCl = 13.75 mL x (1 L / 1000 mL) x 1.35 mol/L
Next, we calculate the moles of Ca(OH)2:
Moles of Ca(OH)2 = Volume of Ca(OH)2 solution (in L) x Concentration of Ca(OH)2 (in mol/L)
Moles of Ca(OH)2 = 22.80 mL x (1 L / 1000 mL) x 0.955 mol/L
Now that we have the moles of each substance, we can determine the limiting reactant.
The limiting reactant is the one that is completely consumed and determines the maximum amount of product that can be formed. To find the limiting reactant, we compare the ratios of moles between HCl and Ca(OH)2 using the coefficients from the balanced equation.
From the balanced equation, we see that the ratio of moles between HCl and Ca(OH)2 is 2 to 1. So, to compare the moles of HCl and Ca(OH)2, we multiply the moles of Ca(OH)2 by 2.
Moles of Ca(OH)2 (adjusted) = 2 x Moles of Ca(OH)2
Next, we compare the moles of HCl and moles of Ca(OH)2 (adjusted). The reactant with the smaller number of moles is the limiting reactant.
If the moles of Ca(OH)2 (adjusted) is smaller than the moles of HCl, it means that Ca(OH)2 is limiting and will be completely consumed. In this case, not all the Ca(OH)2 will be neutralized.
If the moles of Ca(OH)2 (adjusted) is larger than the moles of HCl, it means that Ca(OH)2 is in excess, and all of it will be neutralized.
By following this calculation process, you can determine whether all the Ca(OH)2 will be neutralized in this reaction.