let's consider the effectiveness of two antacids to illustrate how chemical calculations can be important in daily life. Baking soda NaHCO3, is often used as an antacid. It neutralizes excess hydrochloric acid sereted by stomach. The balanced equation for the reaction is NaHCO3 (s) + HCl (aq) = H20 (l) + CO2 (g). Milk of magnesia, which is an aqueous suspension of magnesium hydroxide, Mg (OH) 2 (s) + 2HCl (aq) = 2H20 (l) + MgCl2 (aq), Which anatacid can consume the most stomach acid, 1.00g of NaHCO3, or 1.00g of Mg (OH) 2?

Question

Chemistry

Toby Dickson

28 August, 11:13

let's consider the effectiveness of two antacids to illustrate how chemical calculations can be important in daily life. Baking soda NaHCO3, is often used as an antacid. It neutralizes excess hydrochloric acid sereted by stomach. The balanced equation for the reaction is NaHCO3 (s) + HCl (aq) = H20 (l) + CO2 (g). Milk of magnesia, which is an aqueous suspension of magnesium hydroxide, Mg (OH) 2 (s) + 2HCl (aq) = 2H20 (l) + MgCl2 (aq), Which anatacid can consume the most stomach acid, 1.00g of NaHCO3, or 1.00g of Mg (OH) 2?

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Answers (1)

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Cordell · Answer 1

Milk of Magnesia would consume the most stomach acid at almost 3 times the amount as baking soda.

Explanation:

Baking Soda = NaHCO3 (s) + HCl (aq) = H20 (l) + CO2 (g)

NaHCO3 Molar mass of 84.007 g/mol

0.012 Moles of NaHCO3 and since an equal ratio of HCl is required

we therefore neutralize 0.012 Moles of HCl

Milk of magnesia = Mg (OH) 2 (s) + 2HCl (aq) = 2H20 (l) + MgCl2 (aq)

Mg (OH) 2 (s) Molar mass: 58.3197 g/mol

0.017 Moles of Mg (OH) 2 and the ratio is 2:1, so 2 moles for each 1 mole of Mg (OH) 2, so we need 0.034 Moles of HCl