I need walked through this question, please.
In testing for the efficacy of an antacid compound, 5.0g of hydrochloric acid is mixed with 24.0g of magnesium hydroxide. Is this enough base to react with all the acid?
To determine if there is enough base to react with all the acid, we need to do a stoichiometric calculation.
First, we need to write and balance the chemical equation for the reaction between hydrochloric acid (HCl) and magnesium hydroxide (Mg(OH)2). The balanced equation is:
2HCl + Mg(OH)2 -> MgCl2 + 2H2O
From the balanced equation, we can see that for every 2 moles of HCl, we need 1 mole of Mg(OH)2.
Now, we need to calculate the number of moles of HCl and Mg(OH)2 in the given masses.
To find the number of moles, we use the formula:
moles = mass / molar mass
The molar mass of HCl is 36.5 g/mol, and the molar mass of Mg(OH)2 is 58.33 g/mol.
For HCl:
moles of HCl = 5.0 g / 36.5 g/mol
For Mg(OH)2:
moles of Mg(OH)2 = 24.0 g / 58.33 g/mol
Now that we have the moles of HCl and Mg(OH)2, we can compare their stoichiometric ratio.
Divide the moles of HCl by 2 to get the equivalent moles of Mg(OH)2 needed.
If the moles of Mg(OH)2 are equal to or more than the equivalent moles needed, then there is enough base to react with all the acid. Otherwise, there is not enough base.
- Calculate moles of HCl
- Calculate moles of Mg(OH)2
- Divide moles of Mg(OH)2 by 2
- Compare the calculated equivalent moles of Mg(OH)2 with the actual moles of Mg(OH)2
Let's calculate the moles of HCl and Mg(OH)2:
moles of HCl = 5.0 g / 36.5 g/mol
moles of HCl = 0.137 moles
moles of Mg(OH)2 = 24.0 g / 58.33 g/mol
moles of Mg(OH)2 = 0.411 moles
Now, divide the moles of Mg(OH)2 by 2:
equivalent moles of Mg(OH)2 = 0.411 moles / 2
equivalent moles of Mg(OH)2 = 0.205 moles
Since the moles of Mg(OH)2 (0.411 moles) are more than the equivalent moles needed (0.205 moles), there is enough base to react with all the acid.