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Irina-Kira [14]
3 years ago
14

Milk of magnesia is often taken to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 te

aspoon, which contains 4.00×102mg of Mg(OH)2. Part A What volume of an HCl solution with a pH of 1.3 can be neutralized by one dose of milk of magnesia?
Chemistry
1 answer:
Triss [41]3 years ago
6 0

Answer:

Volume of HCl = 0.0688 L

Explanation:

pH is defined as the negative logarithm of the concentration of hydrogen ions.

Thus,  

pH = - log [H⁺]

So, pH = 1.3

Thus, 1.3 = - log [H⁺]

[H⁺] = 0.05012 M

Since, HCl is a strong acid, the concentration of HCl = 0.05012 M

Also,

Moles of Mg(OH)_2:-

Mass = 4.00\times 10^2\ mg

Also, 1 mg = 0.001 g

So =, Mass = 0.4\ g

Molar mass of Mg(OH)_2 = 58.32 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{0.4\ g}{58.32\ g/mol}

Moles_{Mg(OH)_2}= 0.0069\ mol

According to the reaction:-

Mg(OH)_2 + 2 HCl\rightarrow MgCl_2 + 2 H_2O

1 mole of Mg(OH)_2 neutralizes 2 moles of HCl

Considering:

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

So,

Moles =Molarity \times {Volume\ of\ the\ solution}

Thus,

Moles_{Mg(OH)_2}=2\times Molarity_{HCl}\times Volume_{HCl}

Appyling values as:-

0.0069=2\times 0.05012\times Volume_{HCl}

<u>Volume of HCl = 0.0688 L</u>

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Answer:

0.56L

Explanation:

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Since all of the answer choices are given in units of Liters, it will be convenient to use a value for R that contains "Liters" in its units:R=0.0821\frac{L\cdot atm}{mol\cdot K}

Since the conditions are stated to be STP, we must remember that STP is Standard Temperature Pressure, which means T=273.15K and P=1atm

Lastly, we must calculate the number of moles of O_2(g) there are.  Given 0.80g of O_2(g), we will need to convert with the molar mass of O_2(g).  Noting that there are 2 oxygen atoms, we find the atomic mass of O from the periodic table (16g/mol) and multiply by 2:  32g\text{ }O_2=1mol\text{ }O_2

Thus, \frac{0.80g \text{ }O_2}{1} \frac{1mol\text{ }O_2}{32g\text{ }O_2}=0.25mol\text{ }O_2=n

Isolating V in the Ideal Gas Law:

PV=nRT

V=\frac{nRT}{P}

...substituting the known values, and simplifying...

V=\frac{(0.025 mol \text{ }O_2)(0.0821\frac{L\cdot atm}{mol \cdot K} )(273.15K)}{(1atm)}

V=0.56L \text{ } O_2

So, 0.80g of O_2(g) would occupy 0.56L at STP.

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