How to answer the question: How does a bicarbonate buffer solution control pH when either an acid or a base is added?

A buffer solution is resistant to changes in pH upon the addition of relatively small amounts of acid or base. In this case, the equilibrium resisting changes to the pH is: H2CO3 <-> H+ + HCO3-.

Upon addition of acid;

H+ reacts with HCO3-, forming H2CO3, shifting the equilibrium to the left.

Upon addition of base;

OH- reacts with H2CO3, forming water and HCO3-, shifting the equilibrium to the right.

HJ
Answered by Harvey J. Chemistry tutor

3783 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Define relative atomic mass.


How do buffers work?


Alcohols can be converted into alkenes in an elimination reaction. The elimination of H2O from pentan-2-ol forms a mixture of organic products. Give the names and structures of all the organic products in the mixture.


A solution of acetic acid and sodium acetate was prepared, by dissolving 4.1 g of sodium acetate in 750 cm^3 of 0.085 mol/dm^3 acetic acid, at 25 degrees. 10 Cm^3 of 2 mol/dm^3 HCl was added. Ka is 1.76*10^-5, calculate and explain the change in pH


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