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Chapter 4: Problem 95

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2}\), and \(\mathrm{Al}(\mathrm{OH})_{3}\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of \(0.10 \mathrm{M} \mathrm{HCl}\) per gram?

Short Answer

Expert verified
The balanced chemical equations for the neutralization of hydrochloric acid by MgO, Mg(OH)2, and Al(OH)3 are: a. MgO + 2HCl → MgCl2 + H2O b. Mg(OH)2 + 2HCl → MgCl2 + 2H2O c. Al(OH)3 + 3HCl → AlCl3 + 3H2O To neutralize 0.10 moles of HCl, the required mass of each substance is: a. MgO: 2.02 g b. Mg(OH)2: 2.92 g c. Al(OH)3: 2.60 g MgO is the most effective antacid, as it requires the least mass (2.02 g) to neutralize the same amount of HCl (0.10 moles) compared to the other two substances.

Step by step solution

01

Write balanced chemical equations

Write the balanced chemical equations for the neutralization reactions: a. MgO + 2HCl → MgCl2 + H2O b. Mg(OH)2 + 2HCl → MgCl2 + 2H2O c. Al(OH)3 + 3HCl → AlCl3 + 3H2O
02

Calculate moles of HCl neutralized by 1 mole of each substance

Determine the stoichiometric ratio of each substance reacting with HCl from the balanced chemical equations: a. 1 mole of MgO neutralizes 2 moles of HCl b. 1 mole of Mg(OH)2 neutralizes 2 moles of HCl c. 1 mole of Al(OH)3 neutralizes 3 moles of HCl
03

Calculate the mass of each substance to neutralize 0.10 moles of HCl

Determine the mass of each substance needed to neutralize 0.10 moles of HCl using the molar mass of each substance and the stoichiometric ratios calculated in Step 2: a. MgO: \( (1 \ mol\ of\ MgO) \cdot \frac{40.31\ g}{1\ mol} \cdot \frac{0.10\ mol\ of\ HCl}{2\ mol\ of\ HCl} \approx 2.02\ g \) b. Mg(OH)2: \( (1 \ mol\ of\ Mg(OH)_2) \cdot \frac{58.33\ g}{1\ mol} \cdot \frac{0.10\ mol\ HCl}{2\ mol\ HCl} \approx 2.92\ g \) c. Al(OH)3: \( (1 \ mol\ of\ Al(OH)_3) \cdot \frac{78.00\ g}{1\ mol} \cdot \frac{0.10\ mol\ HCl}{3\ mol\ HCl} \approx 2.60\ g \)
04

Compare masses of substances to determine the most effective antacid

Compare the masses of the substances required to neutralize 0.10 moles of HCl: a. MgO: 2.02 g b. Mg(OH)2: 2.92 g c. Al(OH)3: 2.60 g From the comparison, we can see that MgO requires the least mass (2.02 g) to neutralize the same amount of HCl (0.10 moles) compared to the other two substances. Therefore, MgO will neutralize the greatest amount of 0.10 M HCl per gram.

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Most popular questions from this chapter

The drawings below represent aqueous solutions. Solution A is \(2.00 \mathrm{~L}\) of a \(2.00 \mathrm{M}\) aqueous solution of copper(II) nitrate. Solution \(\mathrm{B}\) is \(2.00 \mathrm{~L}\) of a \(3.00 \mathrm{M}\) aqueous solution of potassium hydroxide. a. Draw a picture of the solution made by mixing solutions \(\mathrm{A}\) and \(\mathrm{B}\) together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions \(\mathrm{A}\) and \(\mathrm{B}\), and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in \(M\) ) of all ions left in solution (from part a) and the mass of solid formed.

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Complete and balance each acid-base reaction. a. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) Contains three acidic hydrogens b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \rightarrow\) Contains two acidic hydrogens c. \(\mathrm{H}_{2} \mathrm{Se}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow\) Contains two acidic hydrogens d. \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) Contains two acidic hydrogens.

When the following solutions are mixed together, what precipitate (if any) will form? a. \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CuSO}_{4}(a q)\) b. \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{CaCl}_{2}(a q)\) c. \(\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{MgI}_{2}(a q)\) d. \(\mathrm{Na}_{2} \mathrm{CrO}_{4}(a q)+\mathrm{AlBr}_{3}(a q)\)
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