Question

Specialized cells in the stomach release HCl to aid digestion. If they release too much, the excess can be neutralized with a base in the form of an antacid. Magnesium hydroxide is a common active ingredient in antacids. As a government chemist testing commercial antacids, you use 0.107 M HCl to simulate the acid concentration in the stomach. How many milliliters of this "stomach acid" will react with a tablet containing 0.252 g of magnesium hydroxide? Enter to 2 decimal places.

Answer 1

Answer:

.

Explanation:

Answer 2

The number of milliliters of this "stomach acid"  that will react with a tablet containing 0.252 g of magnesium hydroxide is  80.75 mL

We have the equation of the reaction as follows;

2HCl(aq) + Mg(OH)2(aq) -----> MgCl2 (aq) + 2H2O(l)

The amount Mg(OH)2 in the tablet is = mass/molar mass

Molar mass of 58.3197 g/mol

Amount of Mg(OH)2 =  0.252 g/58.3197 g/mol = 0.00432 moles

According to the reaction equation;

2 moles of HCl react with 1 mole of Mg(OH)2

x moles of HCl reacts with 0.00432 moles of Mg(OH)2

x = 2 * 0.00432 moles = 0.00864 moles of HCl

Since;

Number of moles = concentration * volume in milliliters/1000

volume in milliliters = 1000 * Number of moles /concentration

volume in milliliters =  1000 * 0.00864 moles/0.107 M

volume in milliliters = 80.75 mL

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