Help I get the first example with hcl but not the h2s one… how do I do this 😭 I don’t get why it’s s2- and not just a because the 2 is on the outside of brackets
Help I get the first example with hcl but not the h2s one… how do I do this 😭 I don’t get why it’s s2- and not just a because the 2 is on the outside of brackets
Not my exam board but I'll give it a go - so for H2S it seems that one H2S molecule protonates two MEA molecules - the remaining S2- ion forms ionic bonds with two protonated MEA molecules (each with a charge of 1+), hence forming a neutrally changed molecule (ie a salt). Sort of similar to Mg(OH)2, the 2 outside the brackets symbolises two hydroxide or MEA molecules.
Not my exam board but I'll give it a go - so for H2S it seems that one H2S molecule protonates two MEA molecules - the remaining S2- ion forms ionic bonds with two protonated MEA molecules (each with a charge of 1+), hence forming a neutrally changed molecule (ie a salt). Sort of similar to Mg(OH)2, the 2 outside the brackets symbolises two hydroxide or MEA molecules.
Help I get the first example with hcl but not the h2s one… how do I do this 😭 I don’t get why it’s s2- and not just a because the 2 is on the outside of brackets
June 2010 F324 Q5
The MS allowed the use of either HS^- or S^2- with or without the charges within the salt shown.
Normally, you would show the negative charge second, just like you do with NaCl and CaCO3, so (HO-CH2-CH2-NH3)2 S would be more natural.