A chemist needs to neutralise aqueous hydrochloric acid solution (currently pH 1) to pH 7 or higher, so it can be safely disposed of. They have access to solid NaCl, NaBr and Na2CO3.

A) Which of the three solids should they add to the acid solution to achieve this?
ans: Na2CO3 [1 mark]
B) Hence give a balanced chemical equation showing the reaction of the hydrochloric acid with your chosen solid.
ans: 2HCl + Na2CO3 --> 2NaCl + H2O + CO2 [2 marks]
C) The hydrochloric acid solution contains 0.1 moles of HCl. If the chemist wants to react all of the HCl as per your equation above, what mass of the chosen solid should they add?
ans: need 0.05 mol Na2CO3, molar mass is 106 g mol-1, so need 0.05 mol x 106 g mol-1 = 53 g. [2 marks]

Answered by Alexander N. Chemistry tutor

1317 Views

See similar Chemistry GCSE tutors

Related Chemistry GCSE answers

All answers ▸

Explain the physical properties of graphite in terms of its structure and bonding


Why does the temperature decrease in the endothermic reaction?


Why does the structure of lithium oxide allow it to conduct electricity under certain conditions?


What is the Haber process? What are the optimal conditions for the reaction and why are they not used in practice?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences