Log in Daniel 9 years agoPosted 9 years ago. Direct link to Daniel's post “Just to be clear, in the ...” Just to be clear, in the problem H and OH are not spectator ions because they form a compound with a covalent bond as a product, rather than one with an ionic bond? • (31 votes) yuki 9 years agoPosted 9 years ago. Direct link to yuki's post “Yup! To be more specific,...” Yup! To be more specific, they form a covalent molecule as opposed to a soluble ionic compound (if they made an insoluble ionic compound, they would not get cancelled out as spectator ions either). (51 votes) Aud Montrull 8 years agoPosted 8 years ago. Direct link to Aud Montrull's post “how do you know whether o...” how do you know whether or not the ion is soulable or not? • (12 votes) Matt B 8 years agoPosted 8 years ago. Direct link to Matt B's post “You need to know the diss...” You need to know the dissociation constant but it is not uncommon for ionic salts to dissolve in water (18 votes) nik.phatslap 9 years agoPosted 9 years ago. Direct link to nik.phatslap's post “How can we tell if someth...” How can we tell if something is a strong base or acid? It seems kind of important to this section, but hasn't really been spoken about until now. • (6 votes) Ernest Zinck 9 years agoPosted 9 years ago. Direct link to Ernest Zinck's post “Memorize the six common s...” Memorize the six common strong acids: HCl, HBr, HI, HNO₃, H₂SO₄, and HClO₄. (30 votes) fombahj 9 years agoPosted 9 years ago. Direct link to fombahj's post “In getting the net iconic...” In getting the net iconic equation from the above equation, why did we have to get rid of the stoichiometric coefficient in front of each chemical species in the net ionic reaction in order for the answer to be correct? • (8 votes) wchargin 9 years agoPosted 9 years ago. Direct link to wchargin's post “I'm assuming that you're ...” I'm assuming that you're talking about the last reaction—H2SO4 (aq) + 2 NaOH (aq) → Na2SO4 (aq) + 2 H2O (ℓ). When we break this up into its ions, we get H2 (aq) + SO4(2−) (aq) + 2 Na+ (aq) + 2 OH− (aq) → 2 Na+ = SO4(2−) (aq) + 2 H2O(ℓ). So we can "cancel" the 2 Na+ (aq) and the SO4(2−) (aq) on each side. Okay. Then the resulting reaction is H2 (aq) + 2 OH− (aq) → 2 H2O (ℓ). But when diatomic hydrogen dissolves in water to form H2 (aq), the protons are separated, so we really just have 2 H+ (aq) + 2 OH− (aq) → 2 H2O (ℓ). Now the factor of two is redundant, so we factor it out to get the result listed: H+ (aq) + OH− (aq) → H2O (ℓ). (13 votes) Quinn Becker 9 years agoPosted 9 years ago. Direct link to Quinn Becker's post “Why when you divide 2H+ b...” Why when you divide 2H+ by two do you get H+, but when you divide 2Na- by two it goes away? • (3 votes) Jessica 9 years agoPosted 9 years ago. Direct link to Jessica's post “You're not dividing the 2...” You're not dividing the 2Na- to make it go away. It goes away because it's a spectator ion (it's unchanged during the reaction so it is present on both sides of the equation and you can cross them out). You should end up with: You can then divide all of these by 2 (like simplifying a math problem) to get: (19 votes) Siddesh Minde 8 years agoPosted 8 years ago. Direct link to Siddesh Minde's post “What are cation and anion...” What are cation and anions • (3 votes) Ernest Zinck 8 years agoPosted 8 years ago. Direct link to Ernest Zinck's post “Cations are atoms that ha...” Cations are atoms that have lost one or more electrons and therefore have a positive charge. (6 votes) Kelli Evans 7 years agoPosted 7 years ago. Direct link to Kelli Evans's post “I have a question....I am...” I have a question....I am really confused on how to do an ionic equation....Please Help! • (4 votes) RogerP 7 years agoPosted 7 years ago. Direct link to RogerP's post “Without specific details ...” Without specific details of where you are struggling, it's difficult to advise. But often, if you don't understand one tutor's presentation then it's worth seeking out other teachers who might explain the topic differently. If you put ionic equations into YouTube there are lots of videos that may help you. (2 votes) Yu Aoi 3 years agoPosted 3 years ago. Direct link to Yu Aoi's post “I know this may sound sil...” I know this may sound silly, but can we subtract or add a reactant to both sides just like in mathematics? • (2 votes) Richard 3 years agoPosted 3 years ago. Direct link to Richard's post “Mathematically it's compl...” Mathematically it's completely acceptable to do so, however we have to consider the actual chemical makeup of our reaction if we do so. For ionic equations like these it's possible for us to eliminate, essentially subtract out, spectator ions from an equation. So these are ions which are present in the reaction solution, but don't really participate in the actual reaction (they don't change as a product compared to when they were a reactant). So since they're not participating in the reaction, subtract them is allowed because it doesn't affect the reaction if they're absent from the equation. In redox reaction it's common to add water, H+, and OH- ion to the equations when balancing them. Now in this case where we're adding chemicals to the equation it may just seem like we're adding chemicals out of convenience to make the math work out. However if it's an aqueous solution, these added chemicals are technically always present in the reaction solution and what we're actually doing is recognizing that some of them are actually part of the redox reaction. So it's not much that we're adding chemicals rather we're discovering the actual reaction occurring. So we can add/subtract in chemical equations, but its can't just simply make mathematical sense, it also has to make sense in a chemistry context. Hope that helps. (5 votes) wanglx123456789 3 years agoPosted 3 years ago. Direct link to wanglx123456789's post “why can the reaction in "...” why can the reaction in "Try it" happen at all? There is no solid in the products. • (2 votes) Richard 3 years agoPosted 3 years ago. Direct link to Richard's post “A solid precipitate isn't...” A solid precipitate isn't the only thing you look for in net ionic equations, you also look for neutral covalent compounds like water forming. In acid/base reaction it's common for the H+, OH-, and H2O to be the only species left in a net ionic equation after all the other spectator ions have been eliminated. Hope this helps. (3 votes) alsalem318 a year agoPosted a year ago. Direct link to alsalem318's post “how come AgCl doesnt diss...” how come AgCl doesnt dissolve in water is it not a salt like NaCl? what is the difference between the two that makes one not dissolve in water? • (1 vote) Richard a year agoPosted a year ago. Direct link to Richard's post “While both are sodium chl...” While both are sodium chloride and silver chloride are ionic compounds, sodium chloride is soluble and dissolves easily in water while silver chloride is insoluble and does not dissolve much into water. The key is the energy associated with the dissolving process. An energy input is required to break bonds, and energy is subsequently released when bonds are formed. The same is true here. For an ionic solid to dissolve, the solvent (in this case water) has to break the ionic bonds then surround the ions and form new ion-dipole bonds in a solvation shell. For the dissolution process to be successful, we must release more energy than is required to break the bonds. If more energy is required to break the bonds than is released during bond formation, then the solid is insoluble. In sodium chloride, the ion-dipole bonds release more energy than was required to break the ionic bonds so it is soluble, but for silver chloride the ion-dipole bonds release less energy than is required to break the ionic bonds so it is insoluble. Hope that helps. (6 votes)Want to join the conversation?
At this stage, if your acid isn't one of these, it is almost certainly a weak acid.
Most metal hydroxides are strong bases.
If your base isn't one of these, it is probably a weak base.
2H+(aq) + 2OH-(aq) --> 2H20
H+(aq) + OH-(aq) --> H20
Anions are atoms that have gained one or more electrons and therefore have a negative charge.
