How to calculate the approximate volume of 6M HCl needed to neutralize 14 mL of 1.1M NaHCO_3.

Question:

How to calculate the approximate volume of 6M HCl needed to neutralize 14 mL of 1.1M NaHCO_3.

Molarity

The molar concentration of a solution is the measure of the concentration of chemical species, in particular of a solute in a solution, in terms of amount of substance per unit volume of solution. Molar concentration or molarity is most commonly expressed in units of moles of solute per liter of solution.

Answer and Explanation:

moles of {eq}NaHCO_3 {/eq} = Molarity ofNaHCO3 {eq}\times {/eq} volume of NaHCO3 in liters

= 1.1 M {eq}\times {/eq} 0.014 L

= 0.0154 mol

{eq}NaHCO_3{(aq)} + HCl_{(aq)} \rightarrow NaCl_{(aq)} + H_2O_{(l)} + CO_2{(g)} {/eq}

one mole of HCl required one mole of HCl

moles of {eq}NaHCO_3 {/eq} = 0.0154 mol

volume of HCl = {eq}\frac {moles of HCl} { Molarity of HCl} {/eq} = {eq}=\frac {0.0154 mol } {6M} = 0.00257 L {/eq}

= 2.6 mL


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What is Molar Mass? - Definition, Formula & Examples

from General Studies Science: Help & Review

Chapter 27 / Lesson 24
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