Explain why subscripts cannot change when balancing a chemical equation

Chemistry

2 answers:

melisa1 [442]3 years ago

6 0

not be changed to balance an equationSubscripts are part of the chemical formula for reactants or products and can

Changing a subscript changes the substance represented by the formula

pav-90 [236]3 years ago

3 0

Subscripts are the identity of the element (the number of atoms) whereas coefficients are the number of molecules of the element.

If you change the subscript, you change the number of atoms an element has. This changes the entire element since each element in the periodic table have different atomic numbers.

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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

Semmy [17]

Answer:

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:

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:

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

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:

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