The daily output of stomach acid (gastric juice) is 1000 to 2000 ml. prior to a meal, stomach acid (hcl) typically has a ph of 1.49.b.) one chewable tablet of the antacid maalox contains 600. mg of caco3. enter the neutralization equation. express your answer as a molecular equation including phasesc.) given that one chewable tablet of the antacid maalox contains 600. mg of caco3, calculate the milliliters of stomach acid neutralized by two tablets of maalox. express the volume in milliliters to two significant figures. d.) the antacid milk of magnesia contains 400. mg of mg(oh)2 per teaspoon. enter the neutralization equation. express your answer as a molecular equation including phases. e.) given that the antacid milk of magnesia contains 400. mg of mg(oh)2 per teaspoon, calculate the number of milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia. (1 tablespoon = 3 teaspoons.)express the volume in milliliters to two significant figures.

B.) 2 HCl(aq) + CaCO₃(s) → CaCl₂(aq) + H₂O(l) + CO₂(g)

C.) 7.4 × 10² mL

D.) 2 HCl(aq) + Mg(OH)₂(aq) → MgCl₂(aq) + H₂O(l)

E.) 1.3 × 10³ mL

Explanation:

The daily output of stomach acid (gastric juice) is 1000 to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1.49.

We can calculate the concentration of H⁺ using the definition of pH.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog (-1.49) = 0.0324 M

Since HCl is a strong monoprotic acid, we can consider this to be the concentration of HCl as well.

B.) One chewable tablet of the antacid Maalox contains 600 mg of CaCO₃. Enter the neutralization equation. Express your answer as a molecular equation including phases.

The neutralization equation is:

2 HCl(aq) + CaCO₃(s) → CaCl₂(aq) + H₂O(l) + CO₂(g)

C.) Given that one chewable tablet of the antacid Maalox contains 600 mg of CaCO₃, calculate the milliliters of stomach acid neutralized by two tablets of Maalox. Express the volume in milliliters to two significant figures.

We can establish the following relations:

The mililiters of HCl that neutralize 2 tablets of Maalox are:

D.) The antacid milk of magnesia contains 400 mg of Mg(OH)₂ per teaspoon. Enter the neutralization equation. Express your answer as a molecular equation including phases.

The neutralization equation is:

2 HCl(aq) + Mg(OH)₂(aq) → MgCl₂(aq) + H₂O(l)

E.) Given that the antacid milk of magnesia contains 400 mg of Mg(OH)₂ per teaspoon, calculate the number of milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia. (1 tablespoon = 3 teaspoons.)Express the volume in milliliters to two significant figures.

We can establish the following relations:

The mililiters of HCl that neutralize 1 tablespoon of milf of magnesia are:

hey there!

mass = 6.75 g

volume =   9 cm³

therefore:

d = mass / volume

d   = 6.75 / 9

d = 0.7 g/cm³

answer b