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.) 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:

Each tablet has 600 mg (0.600 g) of CaCO₃.
The molar mass of CaCO₃ is 100.09 g/mol.
The molar ratio of HCl to CaCO₃ is 2:1.
The concentration of HCl is 0.0324 mol/L.

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

[tex]2Tablet.\frac{0.600gCaCO_{3}}{1Tablet} .\frac{1molCaCO_{3}}{100.09gCaCO_{3}} .\frac{2molHCl}{1molCaCO_{3}} .\frac{1000mLHCl}{0.0324molHCl} =7.4 \times 10^{2} mLHCl[/tex]

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:

1 tablespoon = 3 teaspoons
1 teaspoon contains 400 mg (0.400 g) of Mg(OH)₂
The molar mass of Mg(OH)₂ is 58.32 g/mol.
The molar ratio of HCl to Mg(OH)₂ is 2:1.
The concentration of HCl is 0.0324 mol/L.

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

[tex]1Tablespoon.\frac{3Teaspoon}{1Tablespoon} .\frac{0.400gMg(OH)_{2}}{1Teaspoon} .\frac{1molMg(OH)_{2}}{58.32gMg(OH)_{2}} .\frac{2molHCl}{1molMg(OH)_{2}} .\frac{1000mLHCl}{0.0324molHCl} =1.3 \times 10^{3} mLHCl[/tex]

jayilych4real jayilych4real · Answer 2 · 2022-03-29T17:14:48+02:00

The neutralization equation for the given elements is: B.) 2 HCl(aq) + CaCO₃(s) → CaCl₂(aq) + H₂O(l) + CO₂(g)

The milliliters of stomach acid neutralized by two tablets of Maalox is: C.) 7.4 × 10² mL

The neutralization equation is D.) 2 HCl(aq) + Mg(OH)₂(aq) → MgCl₂(aq) + H₂O(l)

The number of milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia is E.) 1.3 × 10³ mL

Calculation and Parameters

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

Then, we 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.

Read more about neutralization equation here:

https://brainly.com/question/203541