Question
Aluminum hydroxide $\left(\mathrm{Al}(\mathrm{OH})_{3}\right)$ is often present in antacids toneutralize stomach acid $(\mathrm{HCl})$ The reaction occurs as follows: $\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})+3 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{D}) .$ If 14.0 $\mathrm{g}$ of $\mathrm{Al}(\mathrm{OH})_{3}$ is present in an antacid tablet, determine the theoretical yield of $\mathrm{AlCl}_{3}$ produced when the tablet reacts with $\mathrm{HCl}$
Step 1
We know that the molar mass of Al(OH)3 is 78.0 g/mol. So, we have: \[ \frac{14.0 \, \text{g}}{78.0 \, \text{g/mol}} = 0.179 \, \text{mol} \] Show more…
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Aluminum hydroxide $\left(\mathrm{Al}(\mathrm{OH})_{3}\right)$ is often present in antacids to neutralize stomach acid (HCl). The reaction occurs as follows: $\mathrm{Al}(\mathrm{OH})_{3}(\mathrm{s})+3 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2} \mathrm{O}(1) .$ If 14.0 $\mathrm{g}$ of $\mathrm{Al}(\mathrm{OH})_{3}$ is present in an antacid tablet, determine the theoretical yield of AlCl_ produced when the tablet reacts with HCl.
Several brands of antacids use Al(OH)3 to react with stomach acid, which contains primarily HCl: Al(OH)3 (s) + HCl (aq) ------> AlCl3 (aq) + H2O (l) Calculate the number of grams of AlCl3 produced from a reaction of 12.1g Al(OH)3 and 8.4g HCl?
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