5.0 cm3 of 0.050 mol/dm3 sodium carbonate was completely neutralised by 20.00 cm3 of dilute hydrochloric acid. Calculate the concentration in mol/dm3 of the hydrochloric acid.
Question
5.0 cm3 of 0.050 mol/dm3 sodium carbonate was completely neutralised by 20.00 cm3 of dilute hydrochloric acid. Calculate the concentration in mol/dm3 of the hydrochloric acid.
Solution
Sure, here's how you can calculate the concentration of the hydrochloric acid:
Step 1: Calculate the number of moles of sodium carbonate (Na2CO3).
The number of moles = concentration x volume. So, the number of moles of Na2CO3 = 0.050 mol/dm3 x 5.0 cm3 x (1 dm3/1000 cm3) = 0.00025 mol.
Step 2: Write the balanced chemical equation for the reaction.
Na2CO3 + 2HCl -> 2NaCl + H2O + CO2
From the balanced equation, you can see that 1 mole of Na2CO3 reacts with 2 moles of HCl.
Step 3: Calculate the number of moles of HCl.
So, the number of moles of HCl = 2 x number of moles of Na2CO3 = 2 x 0.00025 mol = 0.0005 mol.
Step 4: Calculate the concentration of HCl.
The concentration = number of moles/volume. So, the concentration of HCl = 0.0005 mol / 20.00 cm3 x (1 dm3/1000 cm3) = 0.025 mol/dm3.
So, the concentration of the hydrochloric acid is 0.025 mol/dm3.
Similar Questions
A dilute solution of sodium chloride was prepared with a concentration of 50.0 ppm. Convert this concentration to a molar concentration in mol dm−3.
In Experiment II, 20 cm3 of 0.1 mol/dm3 hydrochloric acid is reacted with excess calcium carbonate. Suggest the concentration of hydrochloric used if the same volume was used for Experiment III.
Calculate the molar concentration of a solution that is prepared by dissolving 5.00 g of sodium chloride, NaCl, in 2.00 dm3 of water.
What is the concentration of chloride ions, in mol dm−3, in a solution formed by mixing 200 cm3of 1 mol dm−3 HCl with 200 cm3 of 5 mol dm−3 NaCl?
Calculate the amount (in mol) of hydrochloric acid, HCl (aq), in 50.0 cm3 of a 2.00 mol dm–3 solution of HCl.
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.