A single dose of a certain antacid contains 250. mg of Mg(OH)2 and 300. mg of CaCO3. How many mmol of H+ can be neutralized by one dose of this antacid? Do not include units in your answer

Mg(OH)2 + 2H^+ ==> 2H2O + Mg^2+

mmols Mg(OH)2 = mg/molar mass = approx 250/58.3 = about 4 but that's only an estimate.

mmols H^+ = twice that approx. Again, an estimate.

CaCO3 + 2H^+ ==> 2H2O + Ca^2+
mmols CaCO3 = 300/100 = about 3
mmols H^+ = twice that.

Add mmols H^+ = total mmols H^+.

To find the number of millimoles (mmol) of H+ that can be neutralized by one dose of this antacid, we need to consider the chemical reaction that occurs between these compounds and H+.

The key reaction is as follows:

Mg(OH)2 + 2H+ -> Mg^2+ + 2H2O
CaCO3 + 2H+ -> Ca^2+ + CO2 + H2O

From the balanced equations above, we can see that 1 mole of Mg(OH)2 can neutralize 2 moles of H+, and 1 mole of CaCO3 can neutralize 2 moles of H+.

To calculate the number of millimoles of H+ that can be neutralized, we need to convert the given mass of each compound to moles:

First, let's convert the mass of Mg(OH)2 to moles:

Molar mass of Mg(OH)2 = 24.31 g/mol (Mg) + 2(16.00 g/mol (O) + 1.01 g/mol (H))
= 24.31 g/mol + 2(16.00 g/mol + 1.01 g/mol)
= 24.31 g/mol + 2(17.01 g/mol)
= 24.31 g/mol + 34.02 g/mol
= 58.33 g/mol

Number of moles of Mg(OH)2 = (mass of Mg(OH)2) / (molar mass of Mg(OH)2)
= 250 mg / 58.33 g/mol
= 0.00428 mol

Now, let's convert the mass of CaCO3 to moles:

Molar mass of CaCO3 = 40.08 g/mol (Ca) + 12.01 g/mol (C) + 3(16.00 g/mol (O))
= 40.08 g/mol + 12.01 g/mol + 3(16.00 g/mol)
= 40.08 g/mol + 12.01 g/mol + 48.00 g/mol
= 100.09 g/mol

Number of moles of CaCO3 = (mass of CaCO3) / (molar mass of CaCO3)
= 300 mg / 100.09 g/mol
= 0.00299 mol

Now that we have the number of moles for each compound, we can calculate the number of moles of H+ that can be neutralized:

Number of moles of H+ = 2 * (moles of Mg(OH)2 + moles of CaCO3)
= 2 * (0.00428 mol + 0.00299 mol)
= 2 * 0.00727 mol
= 0.0145 mol

Finally, we convert the moles of H+ to millimoles (mmol) by multiplying by 1000:

Number of mmol of H+ = (number of moles of H+) * 1000
= 0.0145 mol * 1000
= 14.5 mmol

Therefore, one dose of this antacid can neutralize 14.5 mmol of H+.