You are Here: Home

Help with chemistry homework, please show all working out and answer! watch

1. calculate the volume of 1.20M hydrochloric acid which is required to neutralise exactly the barium oxide formed by decomposition of 5.00g of barium nitrate. Barium oxide reacts with hydrochloric acid as follows

Ba0 + 2HCL - BaCl2 + H20
2. Barium nitrate - Ba(NO3)2 - formula weight = 261 g/mol

Moles = mass / formula weight

Moles of Ba(NO3)2 in 5.00 g = 5.00 / 261 = 0.0192 mol

Therefore you form 0.0192 mol of BaO

As you need 2 HCl to neutralise 1 BaO, you need 0.0192 x 2 = 0.0384 mol of HCl

Volume = moles / concentration

Volume of HCl required = 0.0384 / 1.20 = 0.032 dm^3

= 32 cm^3
3. *sigh*

Yet another "please do my homework for me"

number of moles = mass/Mr
number of moles = concentration x volume (in dm3)

you need that and a calculator.

TSR Support Team

We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out.

This forum is supported by:
Updated: October 27, 2011
Today on TSR

The TSR A-level options discussion thread

Choosing A-levels is hard... we're here to help

BF mum...

Poll

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE