Hi guys can i get help with this question:
In some laboratory analyses the preferred technique is to dissolve an impure solid sample of acid or base in solution containing an excess of acid or base, and then 'back-titrate' the excess with a standard base or acid of known concentration.
This technique is used to assess the purity of a sample of KHSO4.
A 0.4696-g solid sample of impure KHSO4 was dissolved in 50 mL of 0.1 M KOH. This solution contains more base than is needed to neutralise the acid, HSO4-. After neutralisation of the HSO4-, the excess base is neutralised by 10.44 mL of 0.2127 M HCl.
Calculate the percentage by mass of pure KHSO4 in the sample.
express concerntrations of KHSO4 as %w/w
If you could working out would be appreciated, thx
In some laboratory analyses the preferred technique is to dissolve an impure solid sample of acid or base in solution containing an excess of acid or base, and then 'back-titrate' the excess with a standard base or acid of known concentration.
This technique is used to assess the purity of a sample of KHSO4.
A 0.4696-g solid sample of impure KHSO4 was dissolved in 50 mL of 0.1 M KOH. This solution contains more base than is needed to neutralise the acid, HSO4-. After neutralisation of the HSO4-, the excess base is neutralised by 10.44 mL of 0.2127 M HCl.
Calculate the percentage by mass of pure KHSO4 in the sample.
express concerntrations of KHSO4 as %w/w
If you could working out would be appreciated, thx
