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What is the chemical formula for lithium hydroxide? - Socratic LiOH Lithium is a Group 1 metal and commonly forms a M^+ ion Hydroxide anion, ""^(-)OH, has a unit negative charge When they make music together, there is thus 1:1 stoichiometry between ions: Li(s) + H_2O(l) rarr LiOH(aq) + 1 2H_2(g)uarr
What is the formula of #magnesium hydroxide#? - Socratic Mg(OH)_2 Now we know that hydroxides are salts of HO^-, and some metal ion Now if the parent metal has an electronic configuration of 2:8:2, then there are 12 electrons, and the atomic number of the metal is equal to 12 We look on the Periodic Table, and we find that Z=12, for "magnesium metal" As a Group 2 metal, magnesium forms a Mg^(2+) ion, and hence its hydroxide is Mg(OH)_2
What is the value of ΔG°cell? - Socratic They have a cadmium anode, which is oxidized to Cd(OH)2(s) in a basic background electrolyte of concentrated OH–, and a cathode half-reaction in which NiO(OH)(s) is reduced to Ni(OH)2(s) Cd(OH)2 +2e^- -> Cd +2OH- E^o red = -0 403V
What makes for a good leaving group? + Example - Socratic A good leaving group has to be able to part with its electrons easily enough, so typically, it must be a strong acid or weak base relative to other substituents on the same molecule It helps to know the pKa of what would be leaving Let's say you had a mechanism where you are trying to do an E2 reaction to make an -OH (hydroxyl) group leave Maybe you have this compound on hand, sec-butanol
Question #6b9a2 - Socratic "a " 0 02 "mol" "b " 0 89 "g" In order to answer these questions we first need to know the equation representing this chemical reaction
If 50. 0 milliliters of 3. 0 M H_3PO_4 completely . . . - Socratic Mg(OH)_2(s) +H_3PO_4(aq) rarr Mg^(2+)HPO_4^(-)(aq) + 2H_2O(l) With respect to phosphoric acid, we got a molar quantity of 3 0*mol*L^-1xx50xx10^-3*L-=0 150*mol And thus we SUPPOSE it to have neutralized 0 0750*mol magnesium hydroxide which was ostensibly present in a 150*mL volume
Why does neutralisation of any strong acid in an aqueous . . . - Socratic Because its the same reaction A monobasic [monoprotic] acid like HCl has one H atom, which fully dissociates to form a hydrogen ion, H^+ The strong alkali fully dissociates to forman hydroxide ion OH^-, which react to from water This is the ionic equation for neutralisation and occurs for all strong acid strong alkali reactions
Molarity question? - Socratic Step 3: There will be no concentration of #OH^(-)# ions because they are in a solid compound, not dissolved in solution They will no longer be anions in a solid, neutral compound Thus, molarity of #OH^(-)# is 0 Part C: Step 1: Calculate #q# for the heat the water absorbed, not the heat released by the reaction #q=s*m*DeltaT#
Could a buffered solution be made by mixing aqueous . . . - Socratic No, and you've also got two definitions mixed up Two things: The whole point of a buffer is to resist pH change You're not going to do that with two things that dissociate completely "HCl" and "NaOH" are not conjugates of each other What is the definition of a conjugate base or acid? What do they differ by? Any strong acid has a terrible conjugate base that does almost literally nothing in
Question #bcaa2 + Example - Socratic Phenol is hydroxybenzene, which has a proton on the hydroxyl ("OH") group Its "pKa" is about 9 9, which makes it somewhat acidic When you deprotonate phenol, its anionic form has multiple resonance structures: Because of the electron delocalization, the anion (conjugate base) is stabilized (relative to an aliphatic alcohol), and so the phenol molecule itself is more acidic than an aliphatic