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sergejj [24]
2 years ago
13

Stomach acid is approximately 0.10 M HCl. How many mL of stomach acid can be neutralized by one regular antacid tablet that cont

ains 500 mg of solid CaCO3 (100.09 g/mol)?
Chemistry
1 answer:
Radda [10]2 years ago
7 0

Answer:

100 mL

Explanation:

The reaction that takes place is:

  • CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂

First we <u>convert 500 mg of CaCO₃ into mmoles</u>, using its <em>molar mass</em>:

  • 500 mg ÷ 100 mg/mmol = 5 mmol CaCO₃

Then we <u>convert 5 mmoles of CaCO₃ into HCl mmoles</u>, using the <em>stoichiometric coefficients of the balanced reaction</em>:

  • 5 mmol CaCO₃ * \frac{2mmolHCl}{1mmolCaCO_3} = 10 mmol HCl

Finally we <u>calculate the volume of a 0.10 M HCl solution (such as stomach acid) that would contain 10 mmoles</u>:

  • 10 mmol / 0.10 M = 100 mL
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Determine the empirical and molecular formula:
Bingel [31]

Answer:

The empirical formula = molecular formula = C13H18O2

Explanation:

in 100% compound we have 75.6 % Carbon ( Molar mass = 12g/mole), 8.80% hydrogen ( Molar mass = 1.01 g/mole) and 15.5% Oxygen (Molar mass = 16.01 g/mole).

Carbon: 75.6g / 12 = 6.29

Hydrogen: 8.80/ 1 = 8.80

Oxygen: 15.5/ 16 = 0.97

⇒0.97 is the smallest so we divide everything through by 0.97

C: 6.29 / 0.97 =  6.48 ≈ 6.5

H: 8.80 /0.97 = 9

O: 0.97 / 0.97 = 1

To get rid of decimals, we multiply by 2  

C: 6.5 x 2 = 13

H: 9 x 2 = 18

O: 1 x 2 = 2

The empirical formula = C13H18O2

13x 12g/mol + 18x1g/mol  + 2x 16g/mol = 156 + 18 + 32 = 206g/mol  which is the molar mass of ibuprofen

The empirical formula = molecular formula = C13H18O2

6 0
3 years ago
a chemist dissolves 0.564 moles of manganese (IV) oxide (MnO2) in water, and adds enough water to make 0.510 L of solution. Calc
ladessa [460]

Answer:

The molarity of the solution is 1.1 \frac{moles}{liter}

Explanation:

Molarity is a measure of the concentration of that substance that is defined as the number of moles of solute divided by the volume of the solution.

The molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:

molarity=\frac{number of moles of solute}{volume}

Molarity is expressed in units \frac{moles}{liter}

In this case

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  • volume= 0.510 L

Replacing:

molarity=\frac{0.564 moles}{0.510 L}

Solving:

molarity= 1.1 \frac{moles}{liter}

<u><em>The molarity of the solution is 1.1 </em></u>\frac{moles}{liter}<u><em></em></u>

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6b<br> Which of the following is a starting compound during<br> cellular respiration?
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Answer: Oxygen and glucose.

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