Milk of magnesia is a base. What happens when you drink milk of magnesia for an upset stomach?

2 answers:

8 0

I think the correct answer from the choices listed above is option A. When you drink milk of magnesia for an upset stomach, most likely, it would raise the pH in your body since it reacts with the acid inside reducing the amount of acid. Hope this answers the question.

liubo4ka [24]3 years ago

5 0

Answer:

It raises the pH of your stomach.

Explanation:

Milk of magnesia raises the pH of your stomach. This is because the pH of your acidic stomach is well below 7. Adding something with a high pH (a base) will raise the pH back to where it should be.

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What is the molarity of HCl if 34.81 mL of a solution of HCl contain 0.3297 g of HCl?

Temka [501]

Answer:

0.2598 M

Explanation:

Molarity is mol/L, so we have to convert the grams to moles and the mL to L. To convert between grams and moles you need the molar mass of the compound, which is 36.46g/mol.

$0.3297gHCl*\frac{1molHCl}{36.46gHCL} = 0.00904279 mol HCl$

$34.81 mLHCl * \frac{1L}{1000L} = 0.03481 L HCl$

$\frac{0.00904279molHCl}{0.03481 L HCl} = 0.25977554 mol/L$

Round to the lowest number of significant figures = 0.2598 M

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3 years ago

Find δs∘ for the reaction between nitrogen gas and hydrogen gas to form ammonia:12n2(g) 32h2(g)→nh3(g)

Dima020 [189]

Nitrogen (N2) and hydrogen (H2) gases react to form ammonia, which requires -99.4 J/K of standard entropy (ΔS°).

What is standard entropy?

The difference between the total standard entropies of the reaction mixture and the summation of the standard entropies of the outputs is the standard entropy change. Each entropy in the balanced equation needs to be compounded by its coefficient, as shown by the letter "n."

Calculation:

Balancing the given reaction following-

1/2 N₂(g) + 3/2 H₂ (g)→ NH₃ (g)

ΔS° = [1 mol x S° (NH₃)g] - [1/2 mol x S° (N₂)g] - [3/2 mol x S°(H₂)g]

Here S° = standard entropy of the system

Insert into the aforementioned equation all the typical entropy values found in the literature:

ΔS° = [1 mol x 192.45 J/mol.K] - [1/2 mol x 191.61 J/mol.K] - [3/2 mol x 130.684 J/mol.K]

⇒ΔS° = - 99.4 J/K

Therefore, the standard entropy, ΔS° is -99.4 J/K.

Learn more about standard entropy here:

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