Question

What volume of 1.00 M HCl in liters is needed to react completely (with nothing left over) with 0.500 L of 0.500 M Na2CO3 ?Express your answer to three significant figures and include the appropriate units.

Answer 1

The volume of the acid is 0.5 L

Step-by-step explanation

Given that;

The molarity of HCl is 1.00 M

The volume of Na2CO3 is 0.500 L

The molarity of Na2CO3 is 0.500M

To find the volume of HCl needed, follow the steps below

Step 1; Write the balanced equation for the reaction

`\text{ 2HCl\lparen aq\rparen }+\text{ Na}_2CO_(3(aq))\text{ }\rightarrow\text{ 2NaCl}_((aq))\text{ }+\text{ CO}_(2(g))\text{ }+\text{ H}_2O_((l))`

In the above reaction, 2 moles of HCl is needed to completely react with Na2CO3 .

Step 2; Apply the molarity concept to find the volume of the acid

`\text{ }(C_AV_A)/(C_BV_B)\text{ = }(n_A)/(n_B)`

Where

CA is the concentration of the acid

VA is the volume of acid

CB is the concentration of the base

VB is the volume of the base

nA is the number of moles of acid

nB is the number of moles of base

Step 3; Substitute the given data into the formula in step 2

`\begin{gathered} \text{ }\frac{1\text{ }*\text{ V}_A}{0.5\text{ }*\text{ 0.5}}\text{ = }(2)/(1) \\ \text{ Cross multiply} \\ \text{ 1 }* V_A\text{ = 2 }*\text{ 0.5 }*\text{ 0.5} \\ \text{ V}_A\text{ = 0.5 L} \end{gathered}`

Hence, the volume of the acid is 0.5 L