Question
Answer the following for the reaction:$$2 \mathrm{HCl}(a q)+\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CaCl}_{2}(a q)$$a. How many milliliters of a $0.200 \mathrm{M} \mathrm{HCl}$ solution can react with $8.25 \mathrm{~g}$ of $\mathrm{CaCO}_{3}$ ?b. How many liters of $\mathrm{CO}_{2}$ gas can form at STP when $15.5 \mathrm{~mL}$ of a $3.00 \mathrm{M} \mathrm{HCl}$ solution reacts with excess $\mathrm{CaCO}_{3}$ ?c. What is the molarity of a $\mathrm{HCl}$ solution if the reaction of 200. $\mathrm{mL}$ of the $\mathrm{HCl}$ solution with excess $\mathrm{CaCO}_{3}$ produces $12.0 \mathrm{~L}$ of $\mathrm{CO}_{2}$ gas at $725 \mathrm{mmHg}$ and $18{ }^{\circ} \mathrm{C}$ ?
Step 1
We know that the molar mass of $\mathrm{CaCO}_{3}$ is 100.09 g/mol. Therefore, the number of moles of $\mathrm{CaCO}_{3}$ is: $$ \frac{8.25 \, \text{g}}{100.09 \, \text{g/mol}} = 0.0824 \, \text{mol} $$ Show more…
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Calcium carbonate reacts with $\mathrm{HCl}$ according to the following equation: $$ 2 \mathrm{HCl}(a q)+\mathrm{CaCO}_{3}(a q) \longrightarrow \mathrm{CaCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) $$ (a) How many moles of $\mathrm{HCl}$ are in $65 \mathrm{~mL}$ of $0.12 \mathrm{M} \mathrm{HCl}$ ? (b) What mass of calcium carbonate (in grams) is needed for complete reaction with the $\mathrm{HCl}$ in (a)?
Answer the following for the reaction: $$ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{H}_{2}(g)+\mathrm{MgCl}_{2}(a q) $$ a. How many milliliters of a $6.00 \mathrm{M} \mathrm{HCl}$ solution are required to react with $15.0 \mathrm{~g}$ of magnesium? b. How many liters of hydrogen gas can form at STP when $0.500 \mathrm{~L}$ of a $2.00 \mathrm{M} \mathrm{HCl}$ solution reacts with excess magnesium? c. What is the molarity of a $\mathrm{HCl}$ solution if the reaction of $45.2 \mathrm{~mL}$ of the $\mathrm{HCl}$ solution with excess magnesium produces $5.20 \mathrm{~L}$ of $\mathrm{H}_{2}$ gas at $735 \mathrm{mmHg}$ and $25^{\circ} \mathrm{C} ?$
Solutions
Chemical Reactions in Solution
Answer the questions about the following reaction: Ca(OH)2(aq) + 2HCl(aq) → CaCl2(aq) + 2H2O(l) An aqueous solution of Ca(OH)2 with a concentration of 0.125 M was used to titrate 25.00 mL of aqueous HCl. 16.23 mL of the Ca(OH)2 was required to reach the endpoint of the titration. Part 1 How many moles of base were required to react completely with the acid in this reaction? ____ mol Ca(OH)2 Part 2 How many moles of HCl were present in the original 25.00 mL of acid? ____ mol HCl Part 3 What is the molarity of the original HCl solution? Choose one: 0.250 M 0.102 M 0.162 M 1.02 × 10-4 M 0.0408 M
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