Question
Asked Nov 13, 2019
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Calculate the maximum volume in mL of 0.15 M HCl that each of the following antacid formulations would be expected to neutralize. Assume complete neutralization. (Show work.) 
a) a tablet containing 250 mg Al(OH)3 and 150 mg Mg(OH)2

b) a tablet containing 850 mg of CaCO3

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Expert Answer

Step 1

Given

Mass of Al(OH)3 = 250mg

Mass of Mg(OH)2 = 150mg

Mass of CaCO3 = 850mg

Molarity of HCl= 0.15M

The reactions with the given compounds are

Al(ОН); +
ЗНС
AICI, + зH,0
-MgCl2 2H20
2HC
Mg(OH)2
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Al(ОН); + ЗНС AICI, + зH,0 -MgCl2 2H20 2HC Mg(OH)2

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Step 2

No of moles

mass of Al(OH
'A(OH)
no of moles
molar mass
250x103
78
=3.21mmol
mass of Mg (OH
no of moles
Mg(OH)
molarmass
150x103
58.32
-2.57mmol
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mass of Al(OH 'A(OH) no of moles molar mass 250x103 78 =3.21mmol mass of Mg (OH no of moles Mg(OH) molarmass 150x103 58.32 -2.57mmol

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Step 3

According to the reactions

3 moles of HCl are required per mole of Al(OH)3 and 2 moles of HCl are re...

3-(moles of Al(OH))+ 2x(moles of Mg (OH),)
= 3x(3.21mmol)+ 2x(2.57)
= 9.63mmol+5.14mmol
14.77mmol
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3-(moles of Al(OH))+ 2x(moles of Mg (OH),) = 3x(3.21mmol)+ 2x(2.57) = 9.63mmol+5.14mmol 14.77mmol

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